Detecting the presence of chemical species
|
|
- Letitia Logan
- 5 years ago
- Views:
Transcription
1 Chapter 61 Detecting the presence of chemical species 61.1 Preliminary tests of substances 61.2 Detecting the presence of metallic ions in substances using the flame test 61.3 Detecting the presence of cations 61.4 Detecting the presence of anions 61.5 Detecting the presence of common gases and water P. 1 / 100
2 61.6 Deducing the chemical nature of a salt 61.7 Detecting the presence of various functional groups in carbon compounds 61.8 Possible risks associated with chemical tests Key terms Progress check Summary Concept map P. 2 / 100
3 61.1 Preliminary tests of substances Analytical chemistry Qualitative analysis Identification of a particular substance in a sample Quantitative analysis Determination of the amount of a particular substance in a sample P. 3 / 100
4 Preliminary tests on unknown substances includes observing: their colours their smells their solubilities in water action of heat on their samples the ph values of their aqueous solutions 61.1 Preliminary tests of substances P. 4 / 100
5 Colour Many metal oxides and transition metal compounds are coloured substances. Colour of solid ionic substance Black Yellow Blue Green Inference Copper(II) oxide Iron(II, III) oxide Lead(II) oxide Silver iodide Hydrated iron(iii) chloride Hydrated copper(ii) sulphate Hydrated iron(ii) chloride Hydrated copper(ii) chloride Table 61.1 Inference based on the colours of some solid ionic substances Preliminary tests of substances Think about P. 5 / 100
6 The colour of an aqueous ionic solution gives some ideas about the cation or anion it contains. Colour of aqueous ionic solution Inference of the cation/anion it contains Blue or green Copper(II) ion, Cu 2+ Pale green Iron(II) ion, Fe 2+ Yellow Iron(III) ion, Fe 3+ Purple Orange Permanganate ion, MnO 4 Dichromate ion, Cr 2 O 7 2 Table 61.2 Inference based on the colours of some aqueous ionic solutions Preliminary tests of substances P. 6 / 100
7 Smell Some substances give characteristic smells. Smell Characteristic pungent smell Pungent smell of bleaching solution Choking smell of burning sulphur Smell of bad egg Inference Ammonium salt or aqueous ammonia Chlorine gas Sulphur dioxide gas Hydrogen sulphide gas Table 61.3 Inference based on the characteristic smells of some substances Preliminary tests of substances P. 7 / 100
8 Many gases are harmful and some are even toxic. Never smell a gas by breathing in directly above the test tube containing the gas. Hold the tube about 15 cm away from the nose and then fan a little of the gas towards our nose. Figure 61.1 The proper way to smell a gas Preliminary tests of substances P. 8 / 100
9 Solubility in water The solubility of ionic compounds in water gives important hints on what ions are present. Ionic compound Solubility in water Remarks Potassium, sodium and ammonium salts Nitrates Hydrogencarbonates Halides (chlorides, bromides and iodides) Soluble Soluble Soluble Soluble Except: silver halides (AgCl, AgBr and AgI) lead(ii) halides (PbCl 2, PbBr 2 and PbI 2 ) Table 61.4 Some water-soluble and water-insoluble ionic compounds Preliminary tests of substances P. 9 / 100
10 Ionic compound Sulphates Carbonates Solubility in water Soluble Insoluble Remarks Except: silver sulphate (Ag 2 SO 4 ) lead(ii) sulphate (PbSO 4 ) barium sulphate (BaSO 4 ) calcium sulphate (CaSO 4 ; only sparingly soluble) Except: potassium carbonate (K 2 CO 3 ) sodium carbonate (Na 2 CO 3 ) ammonium carbonate ((NH 4 ) 2 CO 3 ) Table 61.4 Some water-soluble and water-insoluble ionic compounds Preliminary tests of substances P. 10 / 100
11 ph of aqueous solution The ph value of the aqueous solution of an unknown substance helps predict its identity. ph paper or universal indicator is used to find the ph value of a solution. Litmus paper is used to distinguish acidic and alkaline solutions Preliminary tests of substances P. 11 / 100
12 Acidic Neutral Basic Acids Some non-metallic oxides (e.g. SO 2, SO 3, NO 2, P 4 O 10 ) Salts formed from strong acids and weak bases (e.g. NH 4 Cl) Water Some non-metallic oxides (e.g. CO, N 2 O) Salts formed from strong acids and strong bases (e.g. NaCl) Alkalis Some metallic oxides (e.g. CaO, K 2 O, Na 2 O) Salts formed from weak acids and strong bases (e.g. CH 3 COO Na + ) Table 61.5 Examples of acidic, neutral and basic compounds Preliminary tests of substances P. 12 / 100
13 Action of heat on solid sample When the solid sample of an unknown substance is heated, the corresponding observations give some hints about its identity. Observations White solid sublimes Black solid sublimes and violet vapour evolves Yellow when hot, white when cold Orange when hot, yellow when cold Inference Ammonium chloride Iodine Zinc oxide Lead(II) oxide Table 61.6 Inference based on the observations when solid samples are heated Preliminary tests of substances P. 13 / 100
14 Figure 61.2 Action of heat on ammonium chloride. White solid deposits at the cooler part of the tube. Learning tip It seems that ammonium chloride sublimes on heating. In fact, ammonium chloride decomposes on heating. heat NH 4 Cl(s) NH 3 (g) + HCl(g) cool Ammonia and hydrogen chloride recombine to form ammonium chloride on cooling Preliminary tests of substances P. 14 / 100
15 (a) (b) Figure 61.3 Action of heat on zinc oxide (a) yellow when hot (b) white when cold. (a) (b) Figure 61.4 Action of heat on lead(ii) oxide (a) orange when hot (b) yellow when cold Preliminary tests of substances P. 15 / 100
16 In some cases, when a solid sample is heated, it decomposes or burns and a gas evolves. The gas provides useful information on the identity of the sample. Example 61.1 Class practice Preliminary tests of substances P. 16 / 100
17 61.2 Detecting the presence of metallic ions in substances using the flame test The presence of certain metals or their compounds can be inferred by a flame test. Flame colour Inference Lilac Potassium ion, K + Golden yellow Sodium ion, Na + Brick-red Calcium ion, Ca 2+ Bluish green Copper(II) ion, Cu 2+ Table 61.7 Inferences based on the flame colours in a flame test. P. 17 / 100
18 Learning tip Potassium compounds give a lilac colour in the flame test but it appears crimson when viewed through cobalt glass. Simulation (Deducing the chemical nature of a sample) potassium ions (lilac) sodium ions (golden yellow) calcium ions (brick-red) Figure 61.5 Flame colours of some metal ions. copper(ii) ions (bluish green) 61.2 Detecting the presence of metallic ions in substances using the flame test P. 18 / 100
19 61.3 Detecting the presence of cations Test with sodium hydroxide solution To detect the presence of cations in a solution, a few drops of dilute sodium hydroxide solution (NaOH(aq)) is added to the solution. Certain metal ions form insoluble hydroxides with NaOH(aq). Learning tip The reactions between sodium hydroxide and solutions of different metal ions have been discussed in Book 2, Section 14.6, p P. 19 / 100
20 Some insoluble hydroxides are coloured precipitates. Cu 2+ (aq) + 2OH (aq) Cu(OH) 2 (s) pale blue precipitate Fe 2+ (aq) + 2OH (aq) Fe(OH) 2 (s) dirty green precipitate Fe 3+ (aq) + 3OH (aq) Fe(OH) 3 (s) reddish brown precipitate 61.3 Detecting the presence of cations P. 20 / 100
21 (a) (b) (c) Figure 61.6 The coloured precipitates formed by the addition of sodium hydroxide solution to solutions containing (a) Cu 2+ (aq), (b) Fe 2+ (aq) and (c) Fe 3+ (aq) ions respectively Detecting the presence of cations P. 21 / 100
22 Ca 2+ (aq) ions, Mg 2+ (aq) ions, Al 3+ (aq) ions, Zn 2+ (aq) ions and Pb 2+ (aq) ions all form white precipitate with NaOH(aq). Al(OH) 3, Zn(OH) 2 and Pb(OH) 2 dissolve in excess NaOH(aq) to give a colourless solution containing complex ions. Al(OH) 3 (s) + OH (aq) [Al(OH) 4 ] (aq) white precipitate from excess NaOH(aq) tetrahydroxoaluminate ion colourless solution Pb(OH) 2 (s) + 2OH (aq) [Pb(OH) 4 ] 2 (aq) white precipitate from excess NaOH(aq) 61.3 Detecting the presence of cations tetrahydroxoplumbate(ii) ion colourless solution P. 22 / 100
23 Zn(OH) 2 (s) + 2OH (aq) [Zn(OH) 4 ] 2 (aq) white precipitate from excess NaOH(aq) tetrahydroxozincate ion colourless solution add a few drops of NaOH(aq) add excess NaOH(aq) zinc nitrate solution white precipitate colourless solution Figure 61.7 The reaction of zinc nitrate solution with excess sodium hydroxide solution Detecting the presence of cations P. 23 / 100
24 Cation Addition of sodium hydroxide solution Small amount Excess Calcium Ca 2+ Magnesium Mg 2+ Aluminium Al 3+ White precipitate Ca 2+ (aq) + 2OH (aq) Ca(OH) 2 (s) white precipitate White precipitate Mg 2+ (aq) + 2OH (aq) Mg(OH) 2 (s) white precipitate White precipitate Al 3+ (aq) + 3OH (aq) Al(OH) 3 (s) white precipitate Insoluble precipitate Insoluble precipitate Precipitate dissolves to become colourless solution. Al(OH) 3 (s) + OH (aq) [Al(OH) 4 ] (aq) Table 61.8 Effects of adding a small amount and an excess of sodium hydroxide solution to the solutions containing certain cations Detecting the presence of cations P. 24 / 100
25 Cation Addition of sodium hydroxide solution Small amount Excess Zinc Zn 2+ Lead(II) Pb 2+ White precipitate Zn 2+ (aq) + 2OH (aq) Zn(OH) 2 (s) white precipitate White precipitate Pb 2+ (aq) + 2OH (aq) Pb(OH) 2 (s) white precipitate Precipitate dissolves to become colourless solution. Zn(OH) 2 (s) + 2OH (aq) [Zn(OH) 4 ] 2 (aq) Precipitate dissolves to become colourless solution. Pb(OH) 2 (s) + 2OH (aq) [Pb(OH) 4 ] 2 (aq) Table 61.8 Effects of adding a small amount and an excess of sodium hydroxide solution to the solutions containing certain cations Detecting the presence of cations P. 25 / 100
26 Cation Addition of sodium hydroxide solution Small amount Excess Iron(II) Fe 2+ Iron(III) Fe 3+ Copper(II) Cu 2+ Ammonium NH 4 + Dirty green precipitate Fe 2+ (aq) + 2OH (aq) Fe(OH) 2 (s) dirty green precipitate Reddish brown precipitate Fe 3+ (aq) + 3OH (aq) Fe(OH) 3 (s) reddish brown precipitate Pale blue precipitate Cu 2+ (aq) + 2OH (aq) Cu(OH) 2 (s) pale blue precipitate No observable change Insoluble precipitate Insoluble precipitate Insoluble precipitate No observable change Table 61.8 Effects of adding a small amount and an excess of sodium hydroxide solution to the solutions containing certain cations Detecting the presence of cations P. 26 / 100
27 If ammonium ion (NH 4+ ) is present, ammonia gas is produced upon warming with NaOH(aq). Ammonia has a characteristic pungent smell and turns moist red litmus paper blue. NH 4+ (aq) + OH (aq) NH 3 (g) + H 2 O(l) characteristic pungent smell moist red litmus paper turns blue ammonium chloride + sodium hydroxide solution Figure 61.8 Ammonium chloride solution reacts with sodium hydroxide solution to produce ammonia gas, which turns moist red litmus paper blue Detecting the presence of cations P. 27 / 100
28 Test with aqueous ammonia Aqueous ammonia precipitates insoluble hydroxides from solutions containing certain metal ions. Example Fe 2+ (aq) + 2OH (aq) Fe(OH) 2 (s) dirty green precipitate Think about 61.3 Detecting the presence of cations P. 28 / 100
29 A solution containing copper(ii) ions Cu 2+ (aq) + 2OH (aq) Cu(OH) 2 (s) blue pale blue precipitate Cu(OH) 2 (s) + 4NH 3 (aq) [Cu(NH 3 ) 4 ] 2+ (aq) + 2OH (aq) pale blue precipitate tetraamminecopper(ii) ion deep blue solution add a small amount of NH 3 (aq) add excess NH 3 (aq) CuSO 4 (aq) Cu(OH) 2 precipitate solution containing [Cu(NH 3 ) 4 ] 2+ (aq) ions Figure 61.9 The reaction of copper(ii) sulphate solution with a small amount and an excess aqueous ammonia Detecting the presence of cations P. 29 / 100
30 A solution containing zinc ions Zn 2+ (aq) + 2OH (aq) Zn(OH) 2 (s) colourless white precipitate Zn(OH) 2 (s) + 4NH 3 (aq) [Zn(NH 3 ) 4 ] 2+ (aq) + 2OH (aq) white precipitate tetraamminezinc ion colourless precipitate 61.3 Detecting the presence of cations P. 30 / 100
31 Cation Addition of aqueous ammonia Small amount Excess Calcium Ca 2+ Magnesium Mg 2+ Aluminium Al 3+ No observable change * Aqueous ammonia does not provide enough hydroxide ions to precipitate out calcium hydroxide. White precipitate Mg 2+ (aq) + 2OH (aq) Mg(OH) 2 (s) White precipitate white precipitate Al 3+ (aq) + 3OH (aq) Al(OH) 3 (s) white precipitate No observable change Insoluble precipitate Insoluble precipitate Table 61.9 Effects of adding a small amount and an excess of aqueous ammonia to the solutions containing certain cations Detecting the presence of cations P. 31 / 100
32 Cation Addition of aqueous ammonia Small amount Excess Zinc Zn 2+ Lead(II) Pb 2+ Iron(II) Fe 2+ White precipitate Zn 2+ (aq) + 2OH (aq) Zn(OH) 2 (s) white precipitate White precipitate Pb 2+ (aq) + 2OH (aq) Pb(OH) 2 (s) white precipitate Dirty green precipitate Fe 2+ (aq) + 2OH (aq) Fe(OH) 2 (s) dirty green precipitate Precipitate dissolves to become colourless solution. Zn(OH) 2 (s) + 4NH 3 (aq) [Zn(NH 3 ) 4 ] 2+ (aq) + 2OH (aq) Insoluble precipitate Insoluble precipitate Table 61.9 Effects of adding a small amount and an excess of aqueous ammonia to the solutions containing certain cations Detecting the presence of cations P. 32 / 100
33 Cation Iron(III) Fe 3+ Copper(II) Cu 2+ Ammonium NH 4 + Small amount Reddish brown precipitate Fe 3+ (aq) + 3OH (aq) Fe(OH) 3 (s) reddish brown precipitate Pale blue precipitate Cu 2+ (aq) + 2OH (aq) Cu(OH) 2 (s) pale blue precipitate No observable change Addition of aqueous ammonia P. 33 / 100 Excess Insoluble precipitate Precipitate dissolves to become deep blue solution. Cu(OH) 2 (s) + 4NH 3 (aq) [Cu(NH 3 ) 4 ] 2+ (aq) + 2OH (aq) No observable change Table 61.9 Effects of adding a small amount and an excess of aqueous ammonia to the solutions containing certain cations Detecting the presence of cations Class practice 61.2
34 Identifying an unknown cation in a sample of solution K +, Na +, Ca 2+, Mg 2+, Al 3+, Zn 2+, Fe 2+, Fe 3+, Cu 2+ or NH 4 + Add NH 3 (aq) to the first portion Does a precipitate form? No Yes white precipitate dirty green precipitate reddish brown precipitate pale blue precipitate Mg 2+, Al 3+ or Zn 2+ Fe 2+ Fe 3+ Cu 2+ K +, Na +, Ca 2+ or NH + (soluble in 4 excess NH 3 (aq)) Figure A flow chart showing how to identify an unknown cation in a sample solution Detecting the presence of cations P. 34 / 100
35 K +, Na +, Ca 2+ or NH 4 + Does the sample give a characteristic flame colour? Perform flame test on the second portion No NH 4 +? Yes lilac flame golden yellow flame brick-red flame K + Na + Ca 2+ Add NaOH(aq) and warm the mixture Is any pungent colourless gas given off? Yes Test the gas with Is the gas alkaline? Yes moist red litmus paper Figure A flow chart showing how to identify an unknown cation in a sample solution Detecting the presence of cations P. 35 / 100 NH 4 +
36 Mg 2+, Al 3+ or Zn 2+ Add excess NH 3 (aq) Does the precipitate dissolve? Yes Zn 2+ No Mg 2+ or Al 3+ Add excess NaOH(aq) Does the precipitate dissolve? No Yes Al 3+ Example 61.2 Figure A flow chart showing how to identify an unknown cation in a sample solution. Mg 2+ Example 61.3 Class practice Detecting the presence of cations P. 36 / 100
37 61.4 Detecting the presence of anions Test for halide ions Using acidified silver nitrate solution Acidified silver nitrate (AgNO 3 (aq)/h + (aq)) solution is used to test for halide ions. It forms insoluble silver halide (AgX; X = Cl, Br, I) with halide ions. P. 37 / 100
38 Ag + (aq) + Cl (aq) AgCl(s) white precipitate Ag + (aq) + Br (aq) AgBr(s) pale yellow precipitate Ag + (aq) + I (aq) AgI(s) yellow precipitate AgCl AgBr AgI Figure Precipitates (from left to right: silver chloride, silver bromide and silver iodide) form when acidified silver nitrate solution is added to solutions containing halide ions Detecting the presence of anions P. 38 / 100
39 The silver nitrate solution should be acidified by adding dilute nitric acid. Nitric acid dissolves any precipitates formed from the reaction between silver nitrate and other anions like carbonate ions and sulphite ions. Ag 2 CO 3 (s) + 2HNO 3 (aq) 2AgNO 3 (aq) + CO 2 (g) + H 2 O(l) precipitate dissolved by nitric acid Ag 2 SO 3 (s) + 2HNO 3 (aq) 2AgNO 3 (aq) + SO 2 (g) + H 2 O(l) precipitate dissolved by nitric acid AgCl(s) + HNO 3 (aq) No reaction precipitate remains insoluble Concept check 61.4 Detecting the presence of anions P. 39 / 100
40 Test for carbonate ions Heating Most carbonates (except K 2 CO 3, Na 2 CO 3 ) decompose upon heating. They give carbon dioxide as a product. strong heating MgCO 3 (s) MgO(s) + CO 2 (g) colourless gas heating CaCO 3 (s) CaO(s) + CO 2 (g) colourless gas 61.4 Detecting the presence of anions P. 40 / 100
41 Learning tip Hydrogencarbonates (e.g. Mg(HCO 3 ) 2 ) will also decompose upon heating, giving carbon dioxide as a product. Ammonium carbonate decomposes to ammonia, carbon dioxide and water vapour when heating. heating (NH 4 ) 2 CO 3 (s) 2NH 3 (g) + CO 2 (g) + H 2 O(g) 61.4 Detecting the presence of anions P. 41 / 100
42 Using dilute hydrochloric acid Dilute hydrochloric acid reacts with carbonates to produce carbon dioxide. CaCO 3 (s) + 2HCl(aq) CaCl 2 (aq) + CO 2 (g) + H 2 O(l) Learning tip colourless gas Sulphuric acid is not used in the test for carbonate ions in calcium carbonate. This is because the formation of sparingly soluble CaSO 4 will prevent further reaction Detecting the presence of anions P. 42 / 100
43 Test for hypochlorite ions Using litmus paper The bleaching action of a bleach is due to the oxidizing power of hypochlorite ions (OCl ). OCl (aq) + dye Cl (aq) + (dye + O) coloured colourless a solution containing OCl (aq) ions blue litmus paper turns white Figure Action of hypochlorite ions on a piece of blue litmus paper Detecting the presence of anions P. 43 / 100
44 Using dilute hydrochloric acid If dilute HCl is added to a solution containing OCl (aq) ions, chlorine (with pungent smell of bleaching solution) will be produced. 2H + (aq) + Cl (aq) + OCl (aq) Cl 2 (g) + H 2 O(l) greenish yellow gas 61.4 Detecting the presence of anions P. 44 / 100
45 Test for sulphite ions Using oxidizing agents Sulphite ion is a strong reducing agent. A strong oxidizing agent is used to test for it. Oxidizing agent Colour change during test Ionic equation Br 2 (aq) Na 2 SO 3 (aq) Br 2 (aq) yellowish brown colourless Table Tests for sulphite ions by some oxidizing agents Detecting the presence of anions SO 3 2 (aq) + Br 2 (aq) + H 2 O(l) SO 4 2 (aq) + 2Br (aq) + 2H + (aq) P. 45 / 100
46 Oxidizing agent Colour change during test Ionic equation Cr 2 O 7 2 (aq) /H + (aq) Na 2 SO 3 (aq) Cr 2 O 2 7 (aq) /H + (aq) orange green 3SO 3 2 (aq) + Cr 2 O 7 2 (aq) + 8H + (aq) 3SO 4 2 (aq) + 2Cr 3+ (aq) + 4H 2 O(l) MnO 4 (aq) /H + (aq) Na 2 SO 3 (aq) MnO 4 (aq) /H + (aq) purple colourless 5SO 3 2 (aq) + 2MnO 4 (aq) + 6H + (aq) 5SO 4 2 (aq) + 2Mn 2+ (aq) + 3H 2 O(l) Table Tests for sulphite ions by some oxidizing agents Detecting the presence of anions P. 46 / 100
47 Using dilute hydrochloric acid If dilute HCl is added to a solution containing SO 3 2 (aq) ions, sulphur dioxide (with choking smell of burning sulphur) will be produced. SO 3 2 (aq) + 2H + (aq) SO 2 (g) + H 2 O(l) Example 61.4 Experiment 61.1 Experiment Detecting the presence of anions P. 47 / 100
48 Identifying an unknown anion in a sample of solution Cl, Br, I, CO 3 2, OCl or SO 3 2 Add acidified AgNO 3 (aq) Does a precipitate form? No CO 3 2, OCl or SO 3 2 Yes white precipitate pale yellow precipitate yellow precipitate Cl Br I Figure A flow chart showing how to identify an unknown anion in a sample solution Detecting the presence of anions P. 48 / 100
49 CO 3 2, OCl or SO 3 2 Does acidified K 2 Cr 2 O 7 (aq) change from orange to green? No Add acidified K 2 Cr 2 O 7 (aq) Yes SO 3 2 CO 3 2 or OCl Does the litmus paper turn white? No CO 3 2? Test the bleaching power by adding it on a piece of litmus paper Add dilute HCl(aq) Yes 61.4 Detecting the presence of anions OCl Is any colourless gas given off? Yes Test the gas with limewater Class practice 61.4 CO 3 2 Yes Does the limewater turn milky? P. 49 / 100
50 61.5 Detecting the presence of common gases and water Test for hydrogen Hydrogen is a colourless and odourless gas. It is the lightest gas and almost insoluble in water. It can be tested with a burning splint. It burns with a pop sound to produce water. 2H 2 (g) + O 2 (g) 2H 2 O(l) P. 50 / 100
51 Test for oxygen Oxygen is a colourless and odourless gas. It is only slightly soluble in water. It relights a glowing splint. glowing splint gas to be tested glowing splint relighted Figure Testing for oxygen with a glowing splint. Oxygen relights the glowing splint Detecting the presence of common gases and water P. 51 / 100
52 Test for carbon dioxide Carbon dioxide is a colourless and odourless gas. It dissolves in water to give a slightly acidic solution. CO 2 (g) + H 2 O(l) H 2 CO 3 (aq) carbonic acid It can be identified by bubbling it through limewater. It turns limewater milky quickly. Ca(OH) 2 (aq) + CO 2 (g) CaCO 3 (s) + H 2 O(l) colourless white precipitate 61.5 Detecting the presence of common gases and water P. 52 / 100
53 carbon dioxide CO 2 (g) white precipitate of CaCO 3 (s) limewater Figure Carbon dioxide turns limewater from colourless to milky Detecting the presence of common gases and water P. 53 / 100
54 Test for chlorine Chlorine is a greenish yellow gas and has a pungent smell of bleaching solution. When chlorine dissolves in water, hydrochloric acid and hypochlorous acid are produced. Cl 2 (aq) + H 2 O(l) HCl(aq) + HOCl(aq) SBA note Chlorine is toxic. Perform experiments involving chlorine in a fume cupboard Detecting the presence of common gases and water P. 54 / 100
55 Coloured substances can be bleached by chlorine water. The bleaching action is due to the oxidizing power of the hypochlorite ions (OCl ) in hypochlorous acid. Chlorine turns moist blue litmus paper red (by the action of H + (aq) ions) and then white very quickly (by the bleaching action of OCl (aq) ions). moist blue litmus paper moist blue litmus paper turns red, and then white Think about 61.5 Detecting the presence of common gases and water Figure Chlorine turns moist blue litmus paper red, and then white. P. 55 / 100
56 Test for ammonia Ammonia is a colourless gas with a characteristic pungent smell. It is extremely soluble in water to give an alkaline solution. NH 3 (aq) + H 2 O(l) NH 4+ (aq) + OH (aq) SBA note Ammonia is toxic. Perform experiments involving ammonia in a fume cupboard Detecting the presence of common gases and water P. 56 / 100
57 Ammonia turns moist red litmus paper blue. Figure Ammonia turns moist red litmus paper blue Detecting the presence of common gases and water P. 57 / 100
58 The presence of ammonia can be further confirmed by using concentrated hydrochloric acid. NH 3 (g) + HCl(g) NH 4 Cl(s) from NH 3 (aq) from HCl(aq) white white fume containing NH 4 Cl(s) HCl(aq) NH 3 (aq) Figure When ammonia from aqueous ammonia reacts with hydrogen chloride from concentrated hydrochloric acid, a dense white fume forms. (Note: Aqueous ammonia is irritant and concentrated hydrochloric acid is corrosive.) 61.5 Detecting the presence of common gases and water P. 58 / 100
59 Test for hydrogen chloride Hydrogen chloride is a colourless gas with a pungent smell. It is denser than air. It is highly soluble in water to give hydrochloric acid. It turns moist blue litmus paper red. moist blue litmus paper turns red hydrogen chloride 61.5 Detecting the presence of common gases and water Figure Hydrogen chloride turns moist blue litmus paper red. (Note: Hydrogen chloride gas is corrosive. Perform this experiment in fume cupboard.) P. 59 / 100
60 The presence of hydrogen chloride can be further confirmed by using ammonia. When it is placed near ammonia, a dense white fume forms. Test for sulphur dioxide Sulphur dioxide is a colourless gas with a choking smell of burning sulphur. It is denser than air. SBA note Sulphur dioxide is toxic. Perform experiments involving sulphur dioxide in a fume cupboard Detecting the presence of common gases and water P. 60 / 100
61 Sulphur dioxide turns a piece of filter paper soaked with acidified potassium dichromate solution from orange to green. Cr 2 O 7 2 (aq) + 3SO 2 (aq) + 2H + (aq) 2Cr 3+ (aq) + 3SO 4 2 (aq) + H 2 O(l) orange green filter paper soaked with acidified K 2 Cr 2 O 7 (aq) the paper turns from orange to green Figure Sulphur dioxide turns a piece of filter paper soaked with acidified potassium dichromate solution from orange to green Detecting the presence of common gases and water P. 61 / 100
62 Sulphur dioxide turns limewater milky. Ca(OH) 2 (aq) + SO 2 (g) CaSO 3 (s) + H 2 O(l) colourless white precipitate Carbon dioxide is odourless while sulphur dioxide has a strong smell of burning sulphur Detecting the presence of common gases and water P. 62 / 100
63 Test for water Using dry cobalt(ii) chloride paper Add a few drops of the liquid under test to blue dry cobalt(ii) chloride paper. The paper turns pink if the liquid contains water. This method can test for the presence of water vapour. dry cobalt(ii) chloride paper Figure Water turns dry cobalt(ii) chloride paper from blue to pink. water 61.5 Detecting the presence of common gases and water P. 63 / 100
64 Using anhydrous copper(ii) sulphate Add a few drops of the liquid under test to white anhydrous copper(ii) sulphate powder. The powder turns blue if water is present. CuSO 4 (s) + 5H 2 O(l) CuSO 4 5H 2 O(s) white blue anhydrous copper(ii) sulphate Example 61.5 Class practice Detecting the presence of common gases and water Figure Water turns anhydrous copper(ii) sulphate powder from white to blue. P. 64 / 100
65 61.6 Deducing the chemical nature of a salt If a salt is provided, various chemical tests are carried out to identify the cations and anions it contains. Example 61.6 Class practice 61.6 Experiment 61.2 P. 65 / 100
66 61.7 Detecting the presence of various functional groups in carbon compounds Test for carbon-carbon double bond (C=C) Reaction with bromine When an alkene is added to bromine (dissolved in an organic solvent), the colour of bromine changes from red-orange to colourless i.e. bromine solution is decolorized. Learning tip To distinguish alkanes and alkenes by using bromine, carry out the test in shade (not in direct sunlight). In case of alkenes, bromine is decolorized rapidly. For alkanes, the colour of bromine remains unchanged P. 66 / 100
67 Example hex-1-ene + bromine (dissolved in organic solvent) red-orange 1,2-dibromohexane colourless hex-1-ene Br 2 in organic solvent bromine solution decolorized Figure Bromine solution is decolorized when hex-1-ene is added to it Detecting the presence of various functional groups in carbon compounds P. 67 / 100
68 Reaction with acidified potassium permanganate solution When an alkene is added to acidified potassium permanganate solution, the colour of the solution changes from purple to colourless. Learning tip Alkenes can be tested by acidified potassium permanganate solution but not acidified potassium dichromate solution Detecting the presence of various functional groups in carbon compounds P. 68 / 100
69 Example + + hex-1-ene from acidified KMnO 4 (aq) (as an oxidizing agent) hexane-1,2,-diol (hexane-1,2-diol can be further oxidized) hex-1-ene acidified KMnO 4 (aq) KMnO 4 decolorized Figure Acidified potassium permanganate solution is decolorized when hex-1-ene is added to it Detecting the presence of various functional groups in carbon compounds P. 69 / 100
70 Test for hydroxyl group ( OH) Reaction with acidified potassium dichromate solution Acidified potassium dichromate solution changes from orange to green when a primary or secondary alcohol is added to it. Learning tip There is no reaction between acidified potassium dichromate solution and tertiary alcohol Detecting the presence of various functional groups in carbon compounds P. 70 / 100
71 The orange Cr 2 O 7 2 (aq) ions are reduced to green Cr 3+ (aq) ions as the alcohol is oxidized. ethanol acidified potassium dichromate solution solution containing Cr 3+ (aq) ions Figure Acidified potassium dichromate solution changes from orange to green when ethanol is added to it Detecting the presence of various functional groups in carbon compounds P. 71 / 100
72 For 1 alcohol from oxidizing agent [O] [O] 1 alcohol aldehyde carboxylic acid [O] [O] e.g. CH 3 CH 2 OH CH 3 CHO CH 3 COOH ethanol ethanal ethanoic acid 61.7 Detecting the presence of various functional groups in carbon compounds P. 72 / 100
73 For 2 alcohol [O] [O] no reaction 2 alcohol ketone [O] [O] e.g. CH 3 CH(OH)CH 3 CH 3 COCH 3 no reaction propan-2-ol propanone Class practice Detecting the presence of various functional groups in carbon compounds P. 73 / 100
74 Reaction with carboxylic acids When an alcohol is heated with a carboxylic acid in the presence of concentrated sulphuric acid, esterification takes place. During the reaction, an ester forms. The ester gives a characteristic pleasant fruity smell. conc. H 2 SO heat carboxylic acid + alcohol ester + water 61.7 Detecting the presence of various functional groups in carbon compounds P. 74 / 100
75 Test for carbonyl group ( C=O) in aldehydes and ketones Reaction with 2,4-dinitrophenylhydrazine 2,4-dinitrophenylhydrazine reacts with aldehyde or ketone to give yellow, orange or red precipitate of 2,4-dinitrophenylhydrazone. This reaction is used to test for the presence of carbonyl group ( C=O). ketone or aldehyde 2,4-dinitrophenylhydrazine 2,4-dinitrophenylhydrazone 61.7 Detecting the presence of various functional groups in carbon compounds P. 75 / 100
76 Example 1 ethanal 2,4-dinitrophenylhydrazine ethanal 2,4-dinitrophenylhydrazone yellow precipitate yellow precipitate of ethanal 2,4-dinitrophenylhydrazone Figure Ethanal 2,4-dinitrophenylhydrazone forms when ethanal reacts with 2,4-dinitrophenylhydrazine Detecting the presence of various functional groups in carbon compounds P. 76 / 100
77 Example 2 propanone 2,4-dinitrophenylhydrazine propanone 2,4-dinitrophenylhydrazone orange-yellow precipitate orange-yellow precipitate of propanone 2,4-dinitrophenylhydrazone Figure Propanone 2,4-dinitrophenylhydrazone forms when propanone reacts with 2,4-dinitrophenylhydrazine Detecting the presence of various functional groups in carbon compounds P. 77 / 100
78 Reaction with Tollens reagent Tollens reagent is used to distinguish between an aldehyde and a ketone. It is a specific test for aldehydes as Tollens reagent has no reaction with ketones. Tollens reagent is an aqueous solution of silver nitrate in excess ammonia. It contains the diamminesilver(i) ion, [Ag(NH 3 ) 2 ] +, in an alkaline solution Detecting the presence of various functional groups in carbon compounds P. 78 / 100
79 When an aldehyde reacts with Tollens reagent, a silver mirror forms inside the test tube. silver mirror Learning tip Figure Ethanal reacts with Tollens reagent to form a silver mirror. Practically, it is possible to coat silver metal (like a mirror) on the inner wall of the test tube. However, grey or black precipitate forms if the inner wall of the test tube is not clean enough Detecting the presence of various functional groups in carbon compounds P. 79 / 100
80 During the reaction, diamminesilver(i) ion is reduced to silver by the aldehyde. RCHO + 2[Ag(NH 3 ) 2 ] + + 3OH RCOO + 2Ag + 4NH 3 + 2H 2 O diamminesilver(i) ion silver mirror Example CH 3 CHO + 2[Ag(NH 3 ) 2 ] + + 3OH CH 3 COO + 2Ag + 4NH 3 + 2H 2 O ethanal diamminesilver(i) ion ethanoate ion silver mirror 61.7 Detecting the presence of various functional groups in carbon compounds P. 80 / 100
81 Test for carboxyl group ( COOH) Reaction with sodium carbonate/sodium hydrogencarbonate solution When a carboxylic acid reacts with sodium hydrogencarbonate or sodium carbonate solution to form carbon dioxide which turns limewater milky. 2RCOOH + Na 2 CO 3 2RCOO Na + + H 2 O + CO 2 sodium carbonate RCOOH + NaHCO 3 RCOO Na + + H 2 O + CO 2 sodium hydrogencarbonate Think about 61.7 Detecting the presence of various functional groups in carbon compounds P. 81 / 100
82 Reaction with alcohol A carboxylic acid reacts with an alcohol in the presence of concentrated sulphuric acid. After heating, an ester with a characteristic pleasant fruity smell will form. Example 61.7 Example 61.8 Class practice 61.8 Experiment 61.3 Experiment Detecting the presence of various functional groups in carbon compounds P. 82 / 100
83 61.8 Possible risks associated with chemical tests Risk assessment Hazardous nature Hazard warning label Hazardous nature Hazard warning label Explosive Toxic or Oxidizing or Harmful or Flammable or Corrosive or Carcinogenic Irritant or P. 83 / 100
84 Procedure for carrying out risk assessment 1. Identify the hazards (hazardous chemicals used or made, hazardous equipment or procedure). 2. Assess how likely the hazard will cause harm and how serious that harm could be. 3. Decide what safety precautions should be taken to reduce the risk to an acceptable level. For example, (a) use a smaller amount of chemicals or a more dilute solution, (b) use a less hazardous chemical, (c) perform the experiment in the fume cupboard, (d) use personal protective equipment Possible risks associated with chemical tests P. 84 / 100
85 safety spectacles laboratory coat glove Figure Personal protective equipment for performing experiments. 4. Find out how to dispose of the hazardous residues after performing the experiment Possible risks associated with chemical tests P. 85 / 100
86 Risk assessment form Risk assessments are made on a standard form. Example 61.9 Class practice 61.9 Activity Possible risks associated with chemical tests P. 86 / 100
87 Key terms 1. 2,4-dinitrophenylhydrazine 2,4- 二硝基苯肼 2. 2,4-dinitrophenylhydrazone 2,4- 二硝基苯腙 3. qualitative analysis 定性分析 4. quantitative analysis 定量分析 5. risk assessment 風險評估 6. risk assessment form 風險評估表 7. Tollens reagent 托倫斯試劑 P. 87 / 100
88 Progress check 1. How do we deduce the ions present in a sample by observing the colour? 2. How do we make a guess of the identity of a substance by smelling? 3. What are the examples of water-soluble and water-insoluble ionic compounds? 4. What are the examples of acidic, neutral and basic compounds? 5. What are the effects of heat on some ionic compounds? 6. What are the flame colours of compounds of potassium, sodium, calcium and copper? P. 88 / 100
89 7. How do we test for the presence of cations in a solution? 8. How do we test for the presence of anions in a solution? 9. How do we detect the presence of common gases and water by chemical methods? 10.How do we detect the presence of various functional groups in carbon compounds? 11.How do we assess the risks associated with chemical tests? Progress check P. 89 / 100
90 Summary 61.1 Preliminary tests of substances 1. The colour of an ionic compound is usually determined by the ions it contains. Refer to Table 61.2 on p.4 for the colours of some ions in aqueous solutions. 2. Some ionic compounds are soluble in water but others are not. Refer to Table 61.4 on p The ph values of some compounds can be found by using ph paper. Refer to Table 61.5 on p.5 for examples of acidic, neutral and basic compounds. P. 90 / 100
91 4. The action of heat on a solid sample can provide useful information on the identity of the solid. Refer to Table 61.6 on p Detecting the presence of metallic ions in substances using the flame test 5. We can infer the presence of certain metals or their compounds by the flame test. Refer to Table 61.7 on p Detecting the presence of cations 6. Refer to Table S61.1 on p.46 for the summary of some tests for certain cations. Summary P. 91 / 100
92 61.4 Detecting the presence of anions 7. Refer to Table S61.2 on p.47 for the summary of some tests for certain anions Detecting the presence of common gases and water 8. Refer to Table S61.3 on p.48 for the summary of some tests for common gases and water Deducing the chemical nature of a salt 9. If we are provided with a salt, we can carry out various chemical tests to identify the cations and anions it contains. Summary P. 92 / 100
93 61.7 Detecting the presence of various functional groups in carbon compounds 10. Refer to Table S61.4 on p.49 for the summary of some tests for various functional groups in carbon compounds Possible risks associated with chemical tests 11. Risk assessment is a systematic way of identifying the potential hazards in an experiment and deciding the preventive measures to be taken to control these risks. Its procedure can be simplified by completing a risk assessment form. Summary P. 93 / 100
94 Concept map Colour Smell Solubility In water ph of aqueous solution Action of heat on solid sample Preliminary test IDENTIFY AN UNKNOWN SUBSTANCE Test for cations Test for anions P. 94 / 100
95 Test for cations Flame test Test with NaOH(aq) Test with NH 3 (aq) K + Na + Ca 2+ Cu 2+ Lilac Golden yellow Brick-red Bluish green Concept map P. 95 / 100
96 Test for anions Halide Carbonate Hypochlorite Sulphite acidified AgNO 3 Forms precipitate strong heating* Decomposes to give CO 2 dilute acids Gives CO 2 litmus paper Paper turns white HCl(aq) Gives Cl 2 K 2 Cr 2 O 7 (aq)/ H + (aq) Solution changes from orange to green HCl(aq) Gives SO 2 Concept map *except K 2 CO 3 and Na 2 CO 3 P. 96 / 100
97 Burns with a pop sound Relights Turns red and then white Turns milky burning splint glowing splint moist blue litmus paper limewater Hydrogen Oxygen Chlorine Carbon dioxide IDENTIFY AN UNKNOWN SUBSTANCE Concept map P. 97 / 100
98 IDENTIFY AN UNKNOWN SUBSTANCE Ammonia Hydrogen chloride Sulphur dioxide Water moist red litmus paper Turns blue conc. HCl Forms a dense white fume moist blue litmus paper Turns red Solution changes from orange to green NH 3 (aq) K 2 Cr 2 O 7 (aq)/ H + (aq) Forms a dense white fume limewater anhydrous copper(ii) sulphate powder Changes from white to blue Turns milky dry cobalt(ii) chloride paper Changes from blue to pink Concept map P. 98 / 100
99 Turns from red-orange to colourless Turns from purple to colourless Solution changes from orange to green Forms ester Br 2 (dissolved in organic solvent) KMnO 4 (aq)/ H + (aq) K 2 Cr 2 O 7 (aq)/ H + (aq) heat with carboxylic acid Carbon-carbon double bond Hydroxyl group IDENTIFY AN UNKNOWN SUBSTANCE P. 99 / 100
100 IDENTIFY AN UNKNOWN SUBSTANCE Carbonyl group Carboxyl group 2,4-dinitrophenylhydrazine Tollens reagent Na 2 CO 3 (aq)/ NaHCO 3 (aq) heat with alcohol Forms orange/ yellow/red precipitate Forms a silver mirror inside the test tube Gives CO 2 Forms ester P. 100 / 100
Qualitative Analysis Part Two Anions & Gases
Qualitative Analysis Part Two Anions & Gases Qualitative Tests for Anions Which anions must I know the tests for? Describe tests to identify the following anions: Carbonate CO 3 2 (by the addition of dilute
More information9.1 Qualitative Analysis
Chemistry Form 4 Page 44 Ms. R. Buttigieg Test for positive Ions (Cations) 9.1 Qualitative Analysis 1) Flame Tests Nichrome wire is dipped in concentrated hydrochloric acid, then in the salt being tested.
More informationflame test acidified silver nitrate solution added
1 The results of two tests on solid X are shown. test aqueous sodium hydroxide added acidified silver nitrate added observation green precipitate formed yellow precipitate formed What is X? copper(ii)
More informationPRACTICAL NUMBER 1 TESTS FOR METAL IONS IN SOLUTION
PRACTICAL NUMBER 1 TESTS FOR METAL IONS IN SOLUTION INTRODUCTION Most common metals have insoluble hydroxides. They can be precipitated from solution by the addition of either ammonia solution (often referred
More informationPRACTICAL NUMBER 1 TESTS FOR METAL IONS IN SOLUTION
PRACTICAL NUMBER 1 TESTS FOR METAL IONS IN SOLUTION INTRODUCTION Most common metals have insoluble hydroxides. They can be precipitated from solution by the addition of either ammonia solution (often referred
More informationIdentification of ions and gases
For more awesome GSE and level resources, visit us at www.savemyexams.co.uk/ Identification Of ions nd Gases Question Paper Level Subject Exam oard Topic Sub-Topic ooklet O Level hemistry ambridge International
More informationIdentification of Ions and Gases
Identification of Ions and Gases Question Paper 1 Level IGSE Subject hemistry (0620/0971) Exam oard ambridge International Examinations (IE) Topic cids, bases and salts Sub-Topic Identification of ions
More informationPlanet Earth. Topic. Unit 1. Introducing chemistry. Unit 2. The atmosphere. Unit 3. The ocean. Unit 4. Rocks and minerals
Topic 1 Planet Earth Unit 1 Unit 2 Unit 3 Unit 4 Introducing chemistry The atmosphere The ocean Rocks and minerals Key C o ncepts Planet Earth The atmosphere Classification of matter element, mixture and
More informationEXPERIMENTS. Testing products of combustion: Reducing Copper(III) Oxide to Copper. Page 4
APPARATUS Page 2 APPARATUS Page 3 Reducing Copper(III) Oxide to Copper EXPERIMENTS Page 4 Testing products of combustion: EXPERIMENTS Showing that oxygen and water is needed for rusting iron Page 5 Showing
More informationSalts Soluble Insoluble Nitrate salts - All nitrate salts - Carbonate salts - Potassium carbonate, K 2 CO. Except
Chapter 8: Salts 1. Salts - A salt is an ionic compound. - The anion part comes from the acid while the cation part comes from a base. - Example: KCl, KOH(aq) + HCl(aq) KCl(aq) + H 2 O(l) - A salt is a
More informationNCEA Chemistry 2.2 Identify Ions AS 91162
NCEA Chemistry 2.2 Identify Ions AS 91162 What is this NCEA Achievement Standard? When a student achieves a standard, they gain a number of credits. Students must achieve a certain number of credits to
More informationCIE Chemistry A-Level Practicals for Papers 3 and 5
CIE Chemistry A-Level Practicals for Papers 3 and 5 Ion Identification Group 2 Ions Identification Example -3 1. Place 10 drops of 0.1 mol dm barium chloride in a clean test tube. Must be clean to ensure
More informationUNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS General Certificate of Education Advanced Subsidiary Level and Advanced Level CHEMISTRY 9701/03
UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS General Certificate of Education Advanced Subsidiary Level and Advanced Level CHEMISTRY 9701/03 Paper 3 Practical Test Candidates answer on the Question
More informationQualitative Analysis Part One: Cations
Qualitative Analysis Part One: Cations Qualitative analysis is a structured set of methods used to determine the identities (but not the amounts) of the components that make up a mixture. Qualitative
More information2.3 Group 7 The Halogens
2.3 Group 7 The Halogens Physical properties of the Halogens: The melting and boiling point of the halogens increases with atomic number due to increased van der Waals (from increased number of electrons).
More informationCHAPTER 8 SALTS. NaCl. A salt is an ionic substance produced when the hydrogen ion of the acid is replaced by metal ion or an ammonium ion.
CHAPTER 8 SALTS A salt is an ionic substance produced when the hydrogen ion of the acid is replaced by metal ion or an ammonium ion. The salt consists of two parts, cation from base and anion from acid.
More informationAQA Chemistry A-level
AQA Chemistry A-level Required Practical 4 Carry out simple test-tube reactions to identify cations and anions + Cations: Group 2 ions, NH 4 Test for group 2 ions: sodium hydroxide -3 1. Place 10 drops
More informationCore practical 15: Analyse organic and inorganic unknowns
Core practical 15 Teacher sheet Core practical 15: Objectives To research the tests for ions and organic compounds To successfully test unknown substances to establish their identity Safety Wear goggles.
More informationAcid, Bases and Salts (IGCSE Chemistry Syllabus )
Acid, Bases and Salts (IGCSE Chemistry Syllabus 2016-2018) Acid o A compound when dissolved in water produces hydrogen ions (H + ) ; proton (H + ) donor o It turns blue damp litmus paper to red o ph 1
More informationGCE. Chemistry. Support Material. Acceptable Colour Changes and Observations. Revised GCE
GCE Revised GCE Support Material Chemistry Acceptable Colour Changes and Observations AS and A2 Effective from September 2016 N.B. It should be noted that the exact colour of a solution often depends
More informationICSE Board Class X Chemistry Board Paper 2014 Solution SECTION I
ICSE Board Class X Chemistry Board Paper 2014 Solution SECTION I Answer 1 1) D 2) B 3) C 4) A 5) C 6) A 7) D 8) C 9) A 10) D 11) 1 12) Sodium ethoxide 13) CaO is alkaline 14) Downward displacement of air
More informationUNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS General Certificate of Education Advanced Subsidiary Level and Advanced Level CHEMISTRY 9701/03
Centre Number Candidate Number Name UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS General Certificate of Education Advanced Subsidiary Level and Advanced Level CHEMISTRY 9701/03 Paper 3 Practical
More informationmolar mass Avogadro Constant Mass of particle (in gram) Mole of particles Number of particles molar mass Avogadro Constant molar volume molar volume
Short Notes: Form 4 Chemistry Chemical Formulae and Equation Calculation For Solid, liquid or gas number of mole = mass of subtance molar mass For gas (only) volume of gas number of mole = molar volme
More informationFor the element X in the ionic compound MX, explain the meaning of the term oxidation state.
1. (a) By referring to electrons, explain the meaning of the term oxidising agent.... For the element X in the ionic compound MX, explain the meaning of the term oxidation state.... (c) Complete the table
More informationAcids and Bases. Topic. Unit 14 Acids and alkalis. Unit 15 Molarity, ph scale and strengths of acids and alkalis. Unit 16 Salts and neutralization
Topic 4 Acids Bases Unit 14 Acids alkalis Unit 15 Molarity, ph scale strengths of acids alkalis Unit 16 Salts neutralization Unit 17 Concentration of s volumetric analysis Key C o ncepts Molarity, ph scale
More informationUNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS General Certificate of Education Advanced Subsidiary Level and Advanced Level
UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS General Certificate of Education Advanced Subsidiary Level and Advanced Level *4827396477* CHEMISTRY 9701/35 Advanced Practical Skills October/November
More informationUNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS General Certificate of Education Advanced Subsidiary Level and Advanced Level
UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS General Certificate of Education Advanced Subsidiary Level and Advanced Level *5947007489* CHEMISTRY 9701/31 Paper 31 Advanced Practical Skills May/June
More informationCentre Number Candidate Number Candidate Name UNIVERSITY OF CAMBRIDGE LOCAL EXAMINATIONS SYNDICATE General Certificate of Education Ordinary Level CHEMISTRY 5070/3 PAPER 3 Practical MAY/JUNE SESSION 2000
More informationCAMBRIDGE INTERNATIONAL EXAMINATIONS International General Certificate of Secondary Education
Centre Number Candidate Number Name CAMBRIDGE INTERNATIONAL EXAMINATIONS International General Certificate of Secondary Education CHEMISTRY 0620/05 Paper 5 Practical Test Candidates answer on the Question
More informationUNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS General Certificate of Education Advanced Subsidiary Level and Advanced Level
UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS General Certificate of Education Advanced Subsidiary Level and Advanced Level * 5803539249 * CHEMISTRY 9701/35 Paper 31 Advanced Practical Skills May/June
More informationUNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS General Certificate of Education Advanced Subsidiary Level and Advanced Level
UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS General Certificate of Education Advanced Subsidiary Level and Advanced Level *1863307025* CHEMISTRY 9701/34 Advanced Practical Skills October/November
More informationConcentration Units. Solute CONCENTRATION. Solvent. g L -1. (M, molarity) concentration in. mol / litre of solution. mol L -1. molality. molality.
CHAPTER 4 REACTIONS IN AQUEOUS SOLUTION CONCENTRATION Solute Solvent Concentration Units mass NaCl / unit volume of solution g L -1 (M, molarity) concentration in moles per litre of solution c NaCl c B
More informationUNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS General Certificate of Education Advanced Subsidiary Level and Advanced Level *7382672438* CHEMISTRY 9701/33 Advanced Practical Skills October/November
More information1 A solution contains barium ions and silver ions and one type of anion. What could the anion be? chloride only. nitrate only.
For more awesome resources, visit us at www.savemyexams.co.uk/ Identification of Ions and Gases Question Paper 2 Level IGSE Subject hemistry (0620/0971) Exam oard ambridge International Examinations (IE)
More informationCambridge International Examinations Cambridge International Advanced Subsidiary and Advanced Level
Cambridge nternational Examinations Cambridge nternational Advanced Subsidiary and Advanced Level CHEMSTRY 9701/32 Paper 3 Advanced Practical Skills 2 May/June 2014 2 hours Candidates answer on the Question
More informationUNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS General Certificate of Education Ordinary Level CHEMISTRY 5070/03
Centre Number Candidate Number Name UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS General Certificate of Education Ordinary Level CHEMISTRY 5070/03 Paper 3 Practical Test Candidates answer on the
More informationICSE Chemistry Board Paper 2016
2015 Time: 2 hours; Max. Marks: 80 General Instructions: Answers to this Paper must be written on the paper provided separately. You will not be allowed 10 write during the first 15 minutes. This time
More informationSection B: Some Essential Background Chemistry
Section B: Some Essential Background Chemistry Soluble and insoluble salts The importance of knowing whether a salt is soluble or insoluble in water You will remember that acids react with carbonates to
More informationCHEMISTRY PAPER 1999
CHEMISTRY PAPER 1999 (One and a half hours) Answers to this paper must be written on the paper provided separately. You will NOT be allowed to write during the first 15 minutes. This time is to be spent
More informationUNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS General Certifi cate of Education Advanced Subsidiary Level and Advanced Level
UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS General Certifi cate of Education Advanced Subsidiary Level and Advanced Level *0926172746* CHEMISTRY 9701/33 Advanced Practical Skills 1 October/November
More informationChem!stry. Assignment on Acids, Bases and Salts #
Chem!stry Name: ( ) Class: Date: / / Assignment on Acids, Bases and Salts #5 Write your answers in the spaces below: 1. 2. 3. 4. 5. 6. 7. 8. 9. 10. 11. 12. 13. 14. 15. 16. 17. 18. 19. 20. 1. Which of the
More informationAcids and Bases. Part A Unit-based exercise. Topic 4. Unit 14 Acids and alkalis. Fill in the blanks. 1 hydrochloric. 2 Sulphuric. 3 Ethanoic.
Topic 4 Acids and Bases Part A Unit-based exercise Unit 14 Acids and alkalis Fill in the blanks 1 hydrochloric 2 Sulphuric 3 Ethanoic 4 sour 5 red; yellow 6 colourless; red 7 bases 8 dissociate; dissociation
More informationUNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS General Certifi cate of Education Advanced Subsidiary Level and Advanced Level
XtremePapers.com UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS General Certifi cate of Education Advanced Subsidiary Level and Advanced Level *8383886562* CHEMISTRY 9701/34 Advanced Practical Skills
More informationQuestion Bank Ammonia
Question Bank Ammonia 1. Why nitrogenous matter produces ammonia? State a liquid source of ammonia. Ans. When nitrogenous matter (such as animal and vegetable proteins) decays in the absence of air, the
More informationSummary Term 2 Chemistry STPM Prepared by Crystal Goh AI Tuition Centre
Summary Term Chemistry STPM Prepared by Crystal Goh AI Tuition Centre 017713136 Period 3 elements property Na Mg Al Si P (P 4 ) Type of element Metal Metalloid Non-metal Structure Giant metallic lattice
More informationChapter 19 Acids and Bases
Chapter 19 Acids and Bases p.1/11 19.1 Introducing Acids and Alkalis Acids and bases are common stuff in everyday life. Domestic Acids and Alkalis Common domestic acids Many foods and drinks contain acids.
More informationCHAPTER No. 1 CHEMICAL REACTIONS AND EQUATIONS HOTS: (High Order Thinking Skill) Questions with Answers: 1 A compound `X` is used for drinking, has ph =7.Its acidified solution undergoes decomposition
More informationChapter 6. Chemical Reactions. Sodium reacts violently with bromine to form sodium bromide.
Chapter 6 Chemical Reactions Sodium reacts violently with bromine to form sodium bromide. Evidence of Chemical Reactions Chemical Equations Reactants Products Reactant(s): Substance(s) present before the
More informationCambridge International Examinations Cambridge International Advanced Subsidiary and Advanced Level
Cambridge International Examinations Cambridge International Advanced Subsidiary and Advanced Level *9763634822* CHEMISTRY 9701/36 Paper 3 Advanced Practical Skills 2 October/November 2014 2 hours Candidates
More informationAcids and Alkalis. Looking at acids and alkalis. 1 hydrochloric. 2 sour. 3 bases. 4 ionize, ionization. 5 hydrogen. 6 mobile ions.
Topic 4 Acids and Alkalis Section A Fill in the blanks Unit 1 Looking at acids and alkalis 1 hydrochloric 2 sour bases 4 ionize, ionization 5 hydrogen 6 mobile ions 7 basicity 8 monobasic 9 dibasic 10
More informationUNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS General Certificate of Education Advanced Subsidiary Level and Advanced Level
UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS General Certificate of Education Advanced Subsidiary Level and Advanced Level *2331107163* CHEMISTRY 9701/32 Paper 32 Practical Test May/June 2007 2 hours
More informationMAHESH TUTORIALS I.C.S.E.
MAHESH TUTORIALS I.C.S.E. GRADE - X (2017-2018) Exam No. : MT/ICSE/SEMI PRELIM - II - SET -A 020 Periodic Table, Chemical bonding, Acid, Bases and Salts, Practical Work, Mole Concept, Electrolysis Chemistry
More informationElectrodeposition. - Worksheet - Envisioning Chemistry. 1. Write half reactions for the following processes under electrical current.
Electrodeposition 1. Write half reactions for the following processes under electrical current. (1). Formation of copper from copper (II) ion Example: Cu 2+ + 2e --> Cu (2). Formation of tin from tin ion
More informationCHEMICAL REACTIONS & EQUATIONS
CHEMICAL REACTIONS & EQUATIONS PHYSICAL AND CHEMICAL CHANGE In our daily life many processes occur around us. Some of them do not lead to formation of any new substance, while others may lead to formation
More informationChapter 8 Chemical Reactions
Chemistry/ PEP Name: Date: Chapter 8 Chemical Reactions Chapter 8: 1 7, 9 18, 20, 21, 24 26, 29 31, 46, 55, 69 Practice Problems 1. Write a skeleton equation for each chemical reaction. Include the appropriate
More information*8733689660* www.onlineexamhelp.com Cambridge International Examinations Cambridge International Advanced Subsidiary and Advanced Level CHEMISTRY 9701/35 Paper 3 Advanced Practical Skills 1 October/November
More informationCambridge International Examinations Cambridge International Advanced Subsidiary and Advanced Level
Cambridge International Examinations Cambridge International Advanced Subsidiary and Advanced Level CHEMISTRY 9701/31 Paper 3 Advanced Practical Skills 1 May/June 2014 2 hours Candidates answer on the
More informationUNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS General Certifi cate of Education Advanced Subsidiary Level and Advanced Level
*0257891118* UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS General Certifi cate of Education Advanced Subsidiary Level and Advanced Level CHEMISTRY 9701/32 Advanced Practical Skills 2 May/June 2013
More informationUNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS General Certifi cate of Education Advanced Subsidiary Level and Advanced Level
*0974901356* UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS General Certifi cate of Education Advanced Subsidiary Level and Advanced Level CHEMISTRY 9701/31 Advanced Practical Skills 1 May/June 2013
More informationSeparate Award Paper 1. Chemistry
5 th Year Separate Award Paper 1 Chemistry Practice Paper 1 Instructions: Attempt ALL the questions. Make your answers in the spaces provided on the question paper. Mark allocations are given in brackets.
More informationUNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS General Certifi cate of Education Advanced Subsidiary Level and Advanced Level
*0014911874* UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS General Certifi cate of Education Advanced Subsidiary Level and Advanced Level CHEMISTRY 9701/33 Advanced Practical Skills 1 May/June 2012
More informationSystematic Procedure for Inorganic Qualitative Analysis Systematic Analysis of Anion
Systematic Procedure for Inorganic Qualitative Analysis Systematic Analysis of Anion S.No Experiment Observation Inference 1 Preliminary Reactions Colourless Absence of Fe 2+, Fe 3+, Ni 2+, Co 2+. 2 Appearance
More informationTHE UNITED REPUBLIC OF TANZANIA NATIONAL EXAMINATIONS COUNCIL CERTIFICATE OF SECONDARY EDUCATION EXAMINATION
THE UNITED REPUBLIC OF TANZANIA NATIONAL EXAMINATIONS COUNCIL CERTIFICATE OF SECONDARY EDUCATION EXAMINATION 032/1 CHEMISTRY 1 (For Both School and Private Candidates) Time: 3 Hours Thursday, 06 th November
More informationReaction Writing Sheet #1 Key
Reaction Writing Sheet #1 Key Write and balance each of the following reactions and indicate the reaction type(s) present: 1. zinc + sulfur zinc sulfide 8 Zn (s) + S 8 (s) 8 ZnS (s) synthesis 2. potassium
More informationCambridge International Examinations Cambridge International Advanced Subsidiary and Advanced Level
*3682053586* Cambridge International Examinations Cambridge International Advanced Subsidiary and Advanced Level CHEMISTRY 9701/31 Paper 3 Advanced Practical Skills 1 May/June 2015 Candidates answer on
More informationThe characteristic Properties of Acids and
For more awesome GSE and level resources, visit us at www.savemyexams.co.uk/ The haracteristic Properties of cids and ases Question Paper Level Subject Exam oard Topic Sub-Topic ooklet O Level hemistry
More informationFluorine Gas. Chlorine Gas. Bromine Liquid. Iodine Solid
Halogens Fluorine (F 2 ): very pale yellow gas. It is highly reactive Chlorine : ( ) greenish, reactive gas, poisonous in high concentrations Bromine ( ) : red liquid, that gives off dense brown/orange
More information4. Inorganic Chemistry and the Periodic Table 4A: Group 2
4. Inorganic Chemistry and the Periodic Table 4A: Group 2 Atomic radius Atomic radius increases down the Group. As one goes down the group, the atoms have more shells of electrons making the atom bigger.
More informationYear 10 Chemistry. Practice questions. Topics
Year 10 Chemistry Practice questions Topics 1 Group 1 2 Group 7 3 Reactivity series 4 Air and Water 5 Rates of reaction 6 Electrolysis 7 Acids, Alkali and Salts Objective: Evaluate group 1 & 7 reactivity
More informationICSE-Science 2(Chemistry) 2009
ICSE-Science 2(Chemistry) 2009 Answers to this Paper must be written on the paper provided separately. You will not be allowed to write during the first 15 minutes. This time is to be spent in reading
More informationH 2 SO 4. HCl. HNO 3 nitric acid. TOPIC: Acids and Bases. e.g. HCl! H + + Cl - sulphuric acid. hydrochloric acid
TOPIC: Acids and Bases Learn these formulae! H 2 SO 4 sulphuric acid HCl hydrochloric acid Acids, especially concentrated acids, are corrosive: you need eye protection and gloves. HNO 3 nitric acid What
More informationPRACTICAL QUESTIONS TEST TUBE REACTIONS 4&11 Questions. Dr Chris Clay
PRACTICAL QUESTIONS TEST TUBE REACTIONS 4&11 Questions Dr Chris Clay http://drclays-alevelchemistry.com/ Q1.(a) A sample of solid chromium(iii) hydroxide displays amphoteric character when treated separately
More informationChemical Bonds In elements and compounds, the atoms are held together by chemical bonds.
Chemical Bonds In elements and compounds, the atoms are held together by chemical bonds. Forming a bond makes an atom more stable, so atoms form as many bonds are they are able to. Bonds are made using
More informationUNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS General Certifi cate of Education Advanced Subsidiary Level and Advanced Level
*1417984110* UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS General Certifi cate of Education Advanced Subsidiary Level and Advanced Level CHEMISTRY 9701/35 Advanced Practical Skills 1 October/November
More informationUNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS General Certificate of Education Advanced Subsidiary Level and Advanced Level
UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS General Certificate of Education Advanced Subsidiary Level and Advanced Level * 8 2 6337145 4* CHEMISTRY 9701/33 Paper 31 Advanced Practical Skills May/June
More informationsodium carbonate. sodium hydrogencarbonate. sodium nitrate. D sodium sulfate. (Total for Question 9 = mark)
1 ompound X is an anhydrous, white solid which decomposes on heating to form a white solid residue, a colourless gas, and a colourless vapour which condenses to a colourless liquid. ompound X is sodium
More information# Ans Workings / Remarks
# Ans Workings / Remarks 1 B Atomic mass and temperature affects the rate of diffusion of gas. The lower the atomic mass, the lighter the substance. The higher the temperature, the higher the rate of collision
More informationPrelab Assignmet Date, Title, Introduction. You will complete the procedures during the lab period as you plan for each test.
1 Qualitative Analysis Prelab Assignmet Date, Title, Introduction. You will complete the procedures during the lab period as you plan for each test. Introduction In this experiment you will be determining
More informationScience NCERT Exemplar Solutions Chapter 1: Chemical Reactions and Equations
Science NCERT Exemplar Solutions Chapter 1: Chemical Reactions and Equations Multiple Choice Questions (MCQs) Q. 1 Which of the following is not a physical change? (a) Boiling of water to give water vapour
More informationTypes of Reactions: Reactions
1 Reactions On the A.P. Test there will be one question (question #4) that will say: Give the formulas to show the reactants and the products for the following chemical reactions. Each occurs in aqueous
More information5072 CHEMISTRY (NEW PAPERS WITH SPA) BASIC TECHNIQUES 5067 CHEMISTRY (NEW PAPERS WITH PRACTICAL EXAM) BASIC TECHNIQUES
5072 CHEMISTRY (NEW PAPERS WITH SPA) BASIC TECHNIQUES 5067 CHEMISTRY (NEW PAPERS WITH PRACTICAL EXAM) BASIC TECHNIQUES LEARNING OUTCOMES a) Be able to write formulae of simple compounds b) Be able to write
More information4.4. Revision Checklist: Chemical Changes
4.4. Revision Checklist: Chemical Changes Reactivity of metals When metals react with other substances the metal atoms form positive ions. The reactivity of a metal is related to its tendency to form positive
More informationLondon Examinations IGCSE
Centre No. Candidate No. Paper Reference 4 3 3 5 2 H Paper Reference(s) 4335/2H London Examinations IGCSE Chemistry Paper 2H Higher Tier Wednesday 21 May 2008 Afternoon Time: 2 hours Surname Signature
More informationUNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS International General Certifi cate of Secondary Education
*8508882337* UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS International General Certifi cate of Secondary Education CHEMISTRY 0620/53 Paper 5 Practical Test May/June 2013 1 hour 15 minutes Candidates
More informationChem!stry. Assignment on Redox
Chem!stry Name: ( ) Class: Date: / / Assignment on Redox Question 1: Which one of the following elements is the most powerful reducing agent? A Aluminium B Copper C Lead D Potassium Question 2: Which of
More informationMAHESH TUTORIALS I.C.S.E.
MAHESH TUTORIALS I.C.S.E. GRADE - X (2017-2018) Exam No. : MT/ICSE/SEMI PRELIM - I-SET -B 008 Sulphuric acid, Ammonia, Analytical Chemistry, Organic Chemistry HCl, Nitric acid, Metallurgy Chemistry SCIENCE
More informationWhat Do You Think? Investigate GOALS
Cool Chemistry Show Activity 4 Chemical Equations GOALS In this activity you will: Represent chemical changes using word equations and chemical equations. Distinguish between different classes of chemical
More informationICSE Board Class X Chemistry Board Paper 2013 Solution SECTION I
ICSE Board Class X Chemistry Board Paper 2013 Solution SECTION I 1) i. Hydronium ii. Hydroxide iii. Salt iv. Water v. Hydrogen 2) i. C 2 H 6 gas Reaction: ii. Sulphur dioxide gas is evolved. K 2 SO 3 +
More informationUNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS General Certificate of Education Advanced Subsidiary Level and Advanced Level
UNVERSTY OF CAMBRDGE NTERNATONAL EXAMNATONS General Certificate of Education Advanced Subsidiary Level and Advanced Level *7779336909* CHEMSTRY 9701/35 Advanced Practical Skills May/June 2011 2 hours Candidates
More informationDOUBLE DISPLACEMENT REACTIONS. Double your pleasure, double your fun
DOUBLE DISPLACEMENT REACTIONS Double your pleasure, double your fun Industrial processes produce unwanted by-products. Dissolved toxic metal ions-copper, mercury, and cadmium-are common leftovers in the
More informationAS Paper 1 Group VII: The Halogens
AS Paper 1 Group VII: The Halogens South Axholme School Q1.Which one of the following statements is true? A B C D Bromine liberates iodine from aqueous sodium iodide. Chlorine liberates fluorine from aqueous
More informationCambridge International Examinations Cambridge International Advanced Subsidiary and Advanced Level
Cambridge International Examinations Cambridge International Advanced Subsidiary and Advanced Level CHEMISTRY 9701/33 Paper 3 Advanced Practical Skills 1 May/June 2014 2 hours Candidates answer on the
More informationThe Copper Cycle. HCl(aq) H + (aq) + Cl (aq) HCl(aq) + H 2 O(l) H 3 O + (aq) + Cl (aq)
The Copper Cycle Introduction Many aspects of our lives involve chemical reactions from the batteries that power our cars and cell phones to the thousands of processes occurring within our bodies. We cannot
More informationRedox Reactions, Chemical Cells and Electrolysis
Topic 5 Redox Reactions, Chemical Cells and Electrolysis Part A Unit-based exercise Unit 19 Chemical cells in daily life Fill in the blanks 1 chemical; electrical 2 electrolyte 3 voltmeter; multimeter
More information4.4. Revision Checklist: Chemical Changes
4.4. Revision Checklist: Chemical Changes Reactivity of metals When metals react with other substances the metal atoms form positive ions. The reactivity of a metal is related to its tendency to form positive
More informationQ1. Ammonia is used in the production of fertilisers. The flow diagram shows the main stages in the manufacture of ammonia.
Q1. Ammonia is used in the production of fertilisers. The flow diagram shows the main stages in the manufacture of ammonia. Study the flow diagram and then answer the questions. (a) What is the purpose
More information(09) WMP/Jun10/CHEM1
Group 2 and Group 7 9 5 The alkane butane is used as a fuel. 5 (a) (i) Write an equation for the complete combustion of butane. 5 (a) (ii) State a condition which may cause carbon to be formed as a product
More informationCHEMISTRY. SCIENCE Paper 2
CHEMISTRY SCIENCE Paper 2 (Two hours) Answers to this Paper must be written on the paper provided separately. You will not be allowed to write during the first 15 minutes. This time is to be spent in reading
More informationICSE QUESTION PAPER Class X Chemistry (2016) Solution
ICSE QUESTION PAPER Class X Chemistry (016) Solution Section I 1. Metals are good reducing agents because they are electron donors. Electrovalent compounds have high melting points. (iii) Higher the ph
More information9.3 Group VII. Content
9.3 Group VII Content 9.3.1 The similarities and trends in the physical and chemical properties of chlorine, bromine and iodine (i) Characteristic physical properties (ii) The relative reactivity of the
More information