TOPIC 3 ANSWERS & MARK SCHEMES QUESTIONSHEET 1 MOLAR SOLUTIONS (1)
|
|
- Neal Thomas
- 5 years ago
- Views:
Transcription
1 QUESTIONSHEET 1 MOLAR SOLUTIONS a) Molar concentration The number of moles of solute dissolved in 1 dm 3 of solution Molar solution One which contains 1 mol of solute in 1 dm 3 of solution b) (i) (HCl) = 36.5 Concentration = 146/36.5 = 4.00 mol dm -3 (ii) (KI) = 166 Concentration = 300/166 = 1.81 mol dm -3 c) (i) Concentration = = 5.92 g dm -3 (ii) (H 2.2H 2 O) = 126 Concentration = 5.92/126 = mol dm -3 d) 1 M Na 2 contains 106 g dm M Na 2 contains = 5.30 g dm -3 in 250 cm 3 there is 5.30/4 = g Na 2 e) Number of moles in solution = molarity volume (in dm 3 ) = = (NaOH) = 40 Mass = = 1.96 g
2 QUESTIONSHEET 2 PREPARATION OF A STANDARD SOLUTION a) (i) A substance which can be weighed out directly to give a solution of known concentration (ii) Must be readily available in a very pure state Must be stable / must not deteriorate on standing Must be non-hygroscopic / must not absorb water vapour Should have a high so that a substantial amount is weighed out / so that weighing errors are negligible (Accept any 3) b) (i) For accuracy (ii) To prevent the sodium carbonate from soiling / damaging the balance pan if it was spilt (iii) To allow for particles of sodium carbonate which adhered to the weighing bottle / which were not transferred (iv) Tap water contains dissolved substances which could affect the titration (v) To avoid errors due to some sodium carbonate solution remaining in the beaker (vi) To avoid overfilling the flask (vii) When the bottom of the liquid meniscus coincided with the graduation mark (viii)to get a uniform / homogeneous solution Or to avoid a concentration gradient in the flask (ix) To give the air bubble a chance to move up and down / to ensure that the solution became properly mixed (x) Discarded the solution / started again
3 QUESTIONSHEET 3 a) H 2 (aq) + 2KOH(aq) K 2 (aq) + 2H 2 O SIMPLE VOLUMETRIC CALCULATIONS n (H 2 ) = n (KOH) / 2 = 20.0(10-3 )0.5 / 2 = mol H 2 Volume required = 5(10-3 ) / 0.2 = 25 x 10-3 dm 3 = 25.0 cm 3 b) NaOH(aq) + HCl(aq) NaCl(aq) + H 2 O n (NaOH) = n (HCl) = 19.8(10-3 ) 0.15 = mol NaOH c (NaOH) = 2.97(10-3 ) / 25.0(10-3 ) = mol dm -3 = mol dm -3 c) CH 3 COOH(aq) + NaOH(aq) CH 3 COO - Na + (aq) + H 2 n (NaOH) = n (CH 3 COOH) = 0.148/60 = mol Volume required = 2.47(10-3 )/ = dm 3 = 24.9 cm 3 d) Na 2 (aq) + 2HCl(aq) 2NaCl(aq) + CO 2 (g) + H 2 O n (Na 2 ) = n (HCl)/2 = 19.6(10-3 ) 0.103/2 = mol m (Na 2 ) = 1.01(10-3 ) 106 = g
4 QUESTIONSHEET 4 CALCULATIONS REQUIRING MOLAR CONCENTRATION OF PRIMARY STANDARD a) n (Na 2 ) = 1.547/106 = mol c (Na 2 ) = (10 3 )/250 = mol dm -3 Na 2 (aq) + H 2 (aq) Na 2 (aq) + CO 2 (g) + H 2 n (H 2 ) = n (Na 2 ) = 25.0(10-3 ) = mol c (H 2 ) = 1.46(10-3 )/24.6(10-3 ) = mol dm -3 b) (i) Solid sodium hydroxide is deliquescent / absorbs water vapour from the air Hence solutions will be more dilute than calculated (ii) n (H 2.2H 2 O) = 14.6/126 = mol c (H 2.2H 2 O) = 0.116(10 3 )/250 = mol dm -3 H 2 (aq) + 2NaOH(aq) Na 2 (aq) + 2H 2 n (NaOH) = n (H 2.2H 2 O) 2 = 25.0(10-3 ) (0.464) 2 = mol c (NaOH) = /24.1(10-3 ) = mol dm -3 (iii) H 2 (aq) + 2NaOH(aq) Na 2 (aq) + 2H 2 n (H 2 ) = n (NaOH)/2 = 20.7(10-3 ) 0.963/2 = mol c (H 2 ) = 9.97(10-3 )/2.00(10-3 ) = 4.98 mol dm = 488 g dm -3
5 QUESTIONSHEET 5 DILUTION QUESTIONS a) A very large volume of titrant would otherwise be required / the burette would have to be refilled during the titration b) HCl(aq) + NaOH(aq) NaCl(aq) + H 2 n (HCl) = n (NaOH) = 23.6(10-3 ) = mol c (diluted HCl) = 2.34(10-3 )/25.0(10-3 ) = mol dm -3 c (concentrated HCl) = (10 3 )/10.0 = 9.36 mol dm -3 c) (i) CH 3 COOH(aq) + NaOH(aq) CH 3 COO - Na + (aq) + H 2 O (l) n (CH 3 COOH) = n (NaOH) = 25.5(10-3 ) = mol c (diluted CH 3 COOH) = 2.60(10-3 )/25.0(10-3 ) = mol dm -3 c (original CH 3 COOH) = 0.104(200)/25.0 = mol dm (350)/10 3 = mol per 350 cm (60) = 17.5 g per 350 cm 3 (ii) From (i), c = mol dm (1.14) = mol per 1.14 dm (60) = 56.9 g per 1.14 dm 3 (iii) n (NaOH) = n (CH 3 COOH) = 0.832(25.0)/10 3 = mol Volume required = /0.102 = dm 3 = 204 cm 3
6 QUESTIONSHEET 6 WATER OF CRYSTALLISATION a) (i) H 2 (aq) + 2NaOH(aq) Na 2 (aq) + 2H 2 n (H 2 ) = n (NaOH)/2 = 21.1(10-3 ) (0.100)/2 = mol in 25 cm 3 n (anhydrous H 2 ) in 1 dm 3 = 1.055(10-3 ) (10 3 )/25 = mol (ii) (H 2 ) = 90 m (anhydrous H 2 ) in 1 dm 3 = (90) = 3.80 g (iii) m (hydrated H 2 ) in 1 dm 3 = 1.33(4) = 5.32 g m (H 2 O) in 1 dm 3 = = 1.52 g (iv) n (H 2 O) in 1 dm 3 = 1.52/18 = mol (v) n (H 2 ) : n (H 2 O) = : = 1 : 2 Or no. of moles of water of crystallisation = 2 b) H 2 (aq) + K 2 (aq) K 2 (aq) + H 2 O + CO 2 (g) n (K 2 ) = n (H 2 ) = 30.0(10-3 ) (0.0125) = mol in 25 cm 3 in l dm 3 there are 3.75(10-4 )(40) = mol K 2 (K 2 ) = 138 in 1 dm 3 there are 0.015(138) = 2.07 g K 2 Hence, mass of water of crystallisation = = g 0.405/18 = mol H 2 O with mol K 2 x = /0.015 = 1.5
7 QUESTIONSHEET 7 a) (i) Absorption of carbon dioxide from the air (ii) Ca(OH) 2 (s) + CO 2 (g) Ca (s) + H 2 PERCENTAGE PURITY b) (i) Ca would have reacted with HCl(aq) Hence too much HCl(aq) would have been used in the titration (ii) Ca(OH) 2 (aq) + 2HCl(aq) CaCl 2 (aq) + 2H 2 n (Ca(OH) 2 ) = n (HCl)/2 = 20.8(10-3 ) 0.210/2 = mol (Ca(OH) 2 ) = 74 m (Ca(OH) 2 ) = 2.18(10-3 ) 74 = g Purity = 0.162(100)/0.204 = 79.4% c) Na 2 (aq) + 2HCl(aq) 2NaCl(aq) + CO 2 (g) + H 2 Note NaCl does not react with hydrochloric acid. n (Na 2 ) = n (HCl)/2 = 18.6(10-3 )0.105/2 = mol in 25 cm mol Na 2 in 250 cm 3 (Na 2 ) = 106 m (Na 2 ) = 9.77(10-3 )106 = 1.04 g m (NaCl) = = 4.03 g Purity = 4.03(100)/5.07 = 79.5%
8 QUESTIONSHEET 8 TEST QUESTION I a) Let the acid be represented by HA; then, since it is monobasic, n (HA) = n (NaOH) = 25.0(10-3 )0.1 = mol in 25.0 cm 3 there were 10( ) = mol HA in 250 cm 3 (HA) = 1.15 / ( ) = g mol -1 b) Mg (s) + 2HNO 3 (aq) Mg(NO 3 ) 2 (aq) + CO 2 (g) + H 2 (Mg ) = 84 n (Mg ) = 1.00/84 = mol n (HNO 3 ) = 2n (Mg ) = 2(0.0119) = mol Volume required = /0.40 = dm 3 = 59.5 cm 3 c) (i) Ca (s) + 2HCl(aq) CaCl 2 (aq) + CO 2 (g) + H 2 n (Ca ) = n (HCl)/2 = 10(10 3 )/2 = 5000 mol (Ca ) = 100 m (Ca ) = 5000 (100) = 500,000 g = 500 kg (ii) Reason 1 Ca is naturally occurring and hence cheap Reason 2 Any excess NaOH would pollute the environment but Ca being insoluble would not do so
9 QUESTIONSHEET 9 TEST QUESTION II a) (i) HCl(aq) + NaOH(aq) NaCl(aq) + H 2 (ii) n (NaOH) = 0.5(19.2/1000) = 9.6 x 10-3 mol n (HCl) = n (NaOH) = 9.6 x 10-3 mol c (HCl) = 9.6 x 10-3 / (25.0/1000) = M b) (i) Na 2 (aq) + 2HCl(aq) 2NaCl(aq) + H 2 O(l) + CO 2 (g) (2) Award for correct reactants and products and for correct balancing. (ii) n (HCl) = 0.384(19.1/1000) = x 10-3 mol n (Na 2 ) = n (HCl) / 2 = x 10-3 / 2 = x 10-3 mol c (Na 2 ) = x 10-3 / (25/1000) = M (iii) Moles Na 2 in 25 cm 3 = x 10-3 moles Na 2 in 1 dm 3 = (3.667 x 10-3 / 25) x 1000 = Mass Na 2 in 1 dm 3 = x 106 = 15.6 g percentage Na 2 = (15.6/20.0) x 100 = 78% c) 500 g Econosoda contains 500(78/100) = 390 g Na g Deluxwash contains 500(98/100) = 490 g Na 2 Econosoda costs 175/390 = 0.45p per gram Na 2 (½) Deluxwash costs 245/490 = 0.50p per gram Na 2 (½) Econosoda is the better value for money
10 QUESTIONSHEET 10 TEST QUESTION III a) HCl(aq) + NaH (aq) NaCl(aq) + H 2 O(l) + CO 2 (g) b) (i) m (NaH ) = 5.00(85/100) = 4.25 g n (NaH ) = 4.25/84 = mol c = / (250/1000) = mol dm -3 (ii) n (NaH ) = (25/1000) = 5.06 x 10-3 mol n (HCl) = n (NaH ) = 5.06 x 10-3 mol V (HCl) = 5.06 x 10-3 / 0.15 = dm 3 = 33.7 cm 3 c) n (H 2 ) = 2(10/1000) = 0.02 mol 2 mol NaH 1 mol H 2 n (NaH ) = 0.02 x 2 = 0.04 mol m (NaH ) = 0.04 x 84 = 3.36 g one 5.0 g tablet is sufficient d) 1 In a suspension particles have a larger surface area than in a tablet reaction with acid occurs more rapidly 2 1 mol of Mg(OH) 2 produces 2 mol of OH - (aq) Mg(OH) 2 is twice as effective as NaH 3 Mg(OH) 2, unlike NaH, does not produce CO 2 which can cause flatulence Maximum 4 marks
11 QUESTIONSHEET 11 EXPERIMENT TO FIND THE EQUATION FOR A REACTION a) (i) moles of iron used = 0.512/55.8 = (ii) moles of copper formed = 0.614/63.5 = (iii) ratio of moles of copper formed: moles of iron reacted = / = 1.05 (iv) Hence write the equation for the reaction Fe + Cu Fe + Cu Or Fe(s) + Cu 2+ (aq) Fe 2+ (aq) + Cu(s) b) (i) Any three of: only carried out once not all iron reacted solid not dry solid lost when liquid removed (ii) (iii) Any one of: value is close to 1:1 only one value Any three of: repeat and average use finer iron filings filter off solid dry to constant mass Quality of language: at least two sentences in which the meaning is clear
12 QUESTIONSHEET 12 ESTIMATING THE CONCENTRATION OF SALTS IN SEA WATER a) Sample x 1000/25 = 28.1 g Sample x 1000/25 = 26.0 g Three significant figures b) Wide variation, result unreliable c) Incomplete evaporation of water Loss of residue due to spitting d) Heat to constant mass Heat in a flask Quality of language: at least two sentences in which the meaning is clear
13 QUESTIONSHEET 13 EXPERIMENT TO FIND THE EQUATION FOR A REACTION DECOMPOSITION OF POTASSIUM HYDROGEN CARBONATE a) Loss in mass = = g % Loss in mass = x100 = 30% b) i. % Loss in mass = 62 x100 = 31% 200 ii. % Loss in mass = 18 x100 = 9% 200 iii. % Loss in mass = 46 x100 = 23% 200 iv. % Loss in mass = 106 x100 = 53% 200 v. % Loss in mass = 50 x100 = 25% 200 c) A. 2KH (s) K 2 (s) + H 2 O(l) + CO 2 (g) d) Any three of: Only carried out once. Small mass % error high. Further decomposition. Spitting. (3) e) Reliable because of the close agreement between experimental and theoretical values, or unreliable because there is only one value. f) Any three of: Repeat. Use larger mass. Use an oven for temperature control. Put on lid (3) Quality of language: at least two sentences in which the meaning is clear
QUESTIONSHEETS ACID-BASE TITRATIONS PREPARATION OF A STANDARD SOLUTION SIMPLE VOLUMETRIC CALCULATIONS
CHEMISTRY QUESTIONSHEETS AS Level AS TOPIC 3 ACID-BASE TITRATIONS Questionsheet 1 Questionsheet 2 Questionsheet 3 Questionsheet 4 Questionsheet 5 Questionsheet 6 Questionsheet 7 Questionsheet 8 Questionsheet
More informationAcids, Bases and Titrations Chapter 4 M. Shozi CHEM110 / 2014
Acids, Bases and Titrations Chapter 4 M. Shozi CHEM110 / 2014 ACID-BASE REACTIONS ACIDS Arrhenius: Compounds that contain an ionisable H and able to ionise in aqueous solution to form H + or H 3 O + Strong
More informationName Class Date. volume of solution molarity of solution amount of solute in moles
Skills Worksheet Problem Solving Titrations Chemists have many methods for determining the quantity of a substance present in a solution or other mixture. One common method is titration, in which a solution
More informationIGCSE (9-1) Edexcel - Chemistry
IGCSE (9-1) Edexcel - Chemistry Principles of Chemistry Chemical Formulae, Equations and Calculations NOTES 1.25: Write word equations and balanced chemical equations (including state symbols): For reactions
More information5 Formulae, equations and amounts of substance Answers to Exam practice questions
Pages 147 149 Exam practice questions 1 a) Cu 2 S(s) + 2O 2 (g) 2CuO(s) + SO 2 (g) All numbers correct [1] b) 2FeS(s) + O 2 (g) + 2SiO 2 (s) 2FeSiO (s) + 2SO 2 (g) All five numbers correct [], four numbers
More informationChapter 4 Reactions in Aqueous Solutions. Copyright McGraw-Hill
Chapter 4 Reactions in Aqueous Solutions Copyright McGraw-Hill 2009 1 4.1 General Properties of Aqueous Solutions Solution - a homogeneous mixture Solute: the component that is dissolved Solvent: the component
More informationName. Practice Test 2 Chemistry 111
Name Practice Test 2 Chemistry 111 1) In the aqueous reaction of K 2 SO 4 (aq) + Ba(NO 3 ) 2 (aq) BaSO 4 (s) + 2KNO 3 (aq), which ions are the spectator ions? A) Ba 2+ 2- and SO 4 B) Ba 2+ and K + C) Ba
More informationStoichiometry ( ) ( )
Stoichiometry Outline 1. Molar Calculations 2. Limiting Reactants 3. Empirical and Molecular Formula Calculations Review 1. Molar Calculations ( ) ( ) ( ) 6.02 x 10 23 particles (atoms or molecules) /
More informationFACTFILE: GCSE CHEMISTRY: UNIT 2.6
FACTFILE: GCSE CHEMISTRY: UNIT Quantitative Chemistry Learning outcomes Students should be able to:.1 calculate the concentration of a solution in mol/dm 3 given the mass of solute and volume of solution;.2
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 informationSTUDYING CHEMICAL REACTIONS BY TITRATION ANALYSIS
STUDYING CHEMICAL REACTIONS BY TITRATION ANALYSIS OBJECTIVES: Study the relationship of reactants & products in solution phase chemical reactions, Learn how to prepare solutions from solid and liquid stock,
More information1.24 Calculations and Chemical Reactions
1.24 Calculations and Chemical Reactions Converting quantities between different substances using a balanced equation A balanced chemical equation tells us the number of particles of a substance which
More informationEquation Writing for a Neutralization Reaction
Equation Writing for a Neutralization Reaction An Acid-Base reaction is also called a Neutralization reaction because the acid (generates H + or H 3 O + ) and base (generates OH ) properties of the reactants
More information19.4 Neutralization Reactions > Chapter 19 Acids, Bases, and Salts Neutralization Reactions
Chapter 19 Acids, Bases, and Salts 19.1 Acid-Base Theories 19.2 Hydrogen Ions and Acidity 19.3 Strengths of Acids and Bases 19.4 Neutralization Reactions 19.5 Salts in Solution 1 Copyright Pearson Education,
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 informationSection 10.3: Acid Base Stoichiometry
Section 10.3: Acid Base Stoichiometry Tutorial 1 Questions, page 481 1. It is necessary to keep the volume of indicator used to a minimum because many acid base indicators are weak acids. Some of the base
More informationQuantitative Chemistry. AQA Chemistry topic 3
Quantitative Chemistry AQA Chemistry topic 3 3.1 Conservation of Mass and Balanced Equations Chemical Reactions A chemical reaction is when atoms are basically rearranged into something different. For
More informationVolumetric analysis involving acids and alkalis
Chapter 19 Volumetric analysis involving acids and alkalis 19.1 Standard solutions 19.2 Acid-alkali titrations 19.3 Calculations on volumetric analysis 19.4 Writing a laboratory report on volumetric analysis
More informationWrite the ionic equation for this neutralisation reaction. Include state symbols.
Q1.Sodium hydroxide neutralises sulfuric acid. The equation for the reaction is: 2NaOH + H 2 SO 4 Na 2 SO 4 + 2H 2 O (a) Sulfuric acid is a strong acid. What is meant by a strong acid? (b) Write the ionic
More informationTitrations. Method for Titration. N Goalby chemrevise.org 1. Using the pipette
Titrations Titrations are done often to find out the concentration of one substance by reacting it with another substance of known concentration. They are often done with neutralisation reactions, but
More informationIB Topics 1 & 11 Multiple Choice Practice
IB Topics 1 & 11 Multiple Choice Practice 1. How many atoms of nitrogen are there in 0.50 mol of (NH 4) 2CO 3? 1 2 3.01 10 23 6.02 10 23 2. What is the value of x when 32.2 g of Na 2SO 4 xh 2O are heated
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 informationChapter 4. Reactions in Aqueous Solution
Chapter 4 Reactions in Aqueous Solution Topics General properties of aqueous solutions Precipitation reactions Acid base reactions Oxidation reduction reactions Concentration of solutions Aqueous reactions
More informationProblem Solving. ] Substitute this value into the equation for poh.
Skills Worksheet Problem Solving In 1909, Danish biochemist S. P. L Sørensen introduced a system in which acidity was expressed as the negative logarithm of the H concentration. In this way, the acidity
More informationChem 115 POGIL Worksheet - Week #6 Oxidation Numbers, Redox Reactions, Solution Concentration, and Titrations
Chem 115 POGIL Worksheet - Week #6 Oxidation Numbers, Redox Reactions, Solution Concentration, and Titrations Why? In addition to metathetical reactions, electron transfer reactions often occur in solutions.
More informationChapter 4. Chemical Quantities and Aqueous Reactions
Lecture Presentation Chapter 4 Chemical Quantities and Aqueous Reactions Reaction Stoichiometry: How Much Carbon Dioxide? The balanced chemical equations for fossilfuel combustion reactions provide the
More informationSolubility Rules See also Table 4.1 in text and Appendix G in Lab Manual
Ch 4 Chemical Reactions Ionic Theory of Solutions - Ionic substances produce freely moving ions when dissolved in water, and the ions carry electric current. (S. Arrhenius, 1884) - An electrolyte is a
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 informationReview of Chemistry 11
Review of Chemistry 11 HCl C 3 H 8 SO 2 NH 4 Cl KOH H 2 SO 4 H 2 O AgNO 3 PbSO 4 H 3 PO 4 Ca(OH) 2 Al(OH) 3 P 2 O 5 Ba(OH) 2 CH 3 COOH 1. Classify the above as ionic or covalent by making two lists. Describe
More informationF321: Atoms, Bonds and Groups Acids
F321: Atoms, Bonds and Groups Acids 49 Marks 1. A student carries out experiments using acids, bases and salts. Calcium nitrate, Ca(NO 3 ) 2, is an example of a salt. The student prepares a solution of
More informationGraspIT AQA GCSE Quantitative changes
A. Chemical measurements part 1 Chemical changes and conservation of mass 1. A piece of magnesium was heated in a crucible. a) Write a balance equation to show how the magnesium reacts with oxygen. (2)
More informationWorked solutions to student book questions Chapter 4 Analysing acids and bases
Q. Antacid tablets should normally be chewed before they are swallowed. Why? A. Antacid tablets are normally chewed to provide a larger surface area for faster reaction with stomach acids. Q. A laboratory
More informationIons in Solution. Solvent and Solute
Adapted from Peer-led Team Learning Begin at the beginning and go on till you come to the end: then stop." Early ideas of atoms and compounds, developed primarily through the reactions of solids and gases,
More informationChapter 4. Reactions in Aqueous Solution
Chapter 4. Reactions in Aqueous Solution 4.1 General Properties of Aqueous Solutions A solution is a homogeneous mixture of two or more substances. A solution is made when one substance (the solute) is
More informationCaCO 3(s) + 2HCl (aq) CaCl 2(aq) + H 2 O (l) + CO 2(g) mole mass 100g 2(36.5g) 111g 18g 44g
STOICHIOMETRY II Stoichiometry in chemical equations means the quantitative relation between the amounts of reactants consumed and product formed in chemical reactions as expressed by the balanced chemical
More informationTYPES OF CHEMICAL REACTIONS
TYPES OF CHEMICAL REACTIONS Precipitation Reactions Compounds Soluble Ionic Compounds 1. Group 1A cations and NH 4 + 2. Nitrates (NO 3 ) Acetates (CH 3 COO ) Chlorates (ClO 3 ) Perchlorates (ClO 4 ) Solubility
More informationPRACTICE EXAMINATION QUESTIONS FOR 1.2 AMOUNT OF SUBSTANCE
PRACTICE EXAMINATION QUESTIONS FOR 1.2 AMOUNT OF SUBSTANCE 1. Nitroglycerine, C 3 H 5 N 3 O 9, is an explosive which, on detonation, decomposes rapidly to form a large number of gaseous molecules. The
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 informationChapter 4 Reactions in Aqueous Solution
Chapter 4 Reactions in Aqueous Solution Homework Chapter 4 11, 15, 21, 23, 27, 29, 35, 41, 45, 47, 51, 55, 57, 61, 63, 73, 75, 81, 85 1 2 Chapter Objectives Solution To understand the nature of ionic substances
More informationChem 110 Acids, Bases, ph, and Redox
Chem 110 Acids, Bases, ph, and Redox 1. If 10.0 ml of 0.100 M HCl is titrated with 0.200 M NaOH, what volume of sodium hydroxide solution is required to neutralize the acid? HCl(aq) + NaOH(aq) NaCl(aq)
More informationUnit 4: Reactions and Stoichiometry
Unit 4: Reactions and Stoichiometry Reactions Chemical equation Expression representing a chemical reaction Formulas of reactants on the left side Formulas of products on the right side Arrow(s) connect(s)
More informationVolumetric Analysis Acids & Bases HL
Name: Volumetric Analysis 1. Concentrations of Solutions 3. Volumetric Analysis Objectives -define solution -define concentration -define molarity -express concentration of solutions in mol/l(molarity),
More information9/24/12. Chemistry Second Edition Julia Burdge. Reactions in Aqueous Solutions
Chemistry Second Edition Julia Burdge 4 Reactions in Aqueous Solutions Copyright (c) The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1 4 Reactions in Aqueous Solutions
More informationStoichiometric relationships 1
Stoichiometric relationships 1 Chapter outline Describe the three states of matter. Recall that atoms of diff erent elements combine in fi xed ratios to form compounds which have diff erent properties
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 information1.22 Concentration of Solutions
1.22 Concentration of Solutions A solution is a mixture formed when a solute dissolves in a solvent. In chemistry we most commonly use water as the solvent to form aqueous solutions. The solute can be
More informationFigure 1. Oxygen. (g) +... (g)... SO 3. The pressure of the reacting gases was increased.
Q1. Figure 1 represents a reaction in the production of sulfuric acid. Figure 1 Oxygen Sulfur dioxide Sulfur trioxide (a) Complete and balance the equation for the reaction.... SO 2 (g) +... (g)... SO
More informationCHEM1109 Answers to Problem Sheet Isotonic solutions have the same osmotic pressure. The osmotic pressure, Π, is given by:
CHEM1109 Answers to Problem Sheet 5 1. Isotonic solutions have the same osmotic pressure. The osmotic pressure, Π, is given by: Π = MRT where M is the molarity of the solution. Hence, M = Π 5 (8.3 10 atm)
More informationmohd faisol mansor/chemistry form 4/chapter 7 CHAPTER 7 ACIDS AND BASES HCl (g) H 2 O H + (aq) + Cl - (aq) NaOH(s) H 2 O Na + (aq) + OH - (aq)
CHAPTER 7 ACIDS AND BASES Arrhenius Theory An acid is a chemical compound that produces hydrogen ions, H + or hydroxonium ions H3O + when dissolve in water. A base defined as a chemical substance that
More informationGrace King High School Chemistry Test Review
CHAPTER 19 Acids, Bases & Salts 1. ACIDS Grace King High School Chemistry Test Review UNITS 7 SOLUTIONS &ACIDS & BASES Arrhenius definition of Acid: Contain Hydrogen and produce Hydrogen ion (aka proton),
More informationChemical Reaction Defn: Chemical Reaction: when starting chemical species form different chemicals.
Chemistry 11 Notes on Chemical Reactions Chemical Reaction Defn: Chemical Reaction: when starting chemical species form different chemicals. Evidence to indicate that a chemical reaction has occurred:
More informationChapter 4. Types of Chemical Reactions and Solution Stoichiometry
Chapter 4 Types of Chemical Reactions and Solution Stoichiometry Chapter 4 Table of Contents 4.1 Water, the Common Solvent 4.2 The Nature of Aqueous Solutions: Strong and Weak Electrolytes 4.3 The Composition
More informationDo Now April 24, 2017
Do Now April 24, 2017 Obj: Observe and describe neutralization reactions. Copy: Neutralization is when an acid and base react to product a salt and water. e.g. HCl + NaOH NaCl + H 2 O acid base salt water
More informationChemistry 143 Acid Base Titration Dr. Caddell. Titrating Acid
Titrating Acid In this lab you will first determine the concentration of sodium hydroxide in a stock solution that you prepare. You will then use that stock sodium hydroxide solution to titrate a solution
More informationChapter 4. The Major Classes of Chemical Reactions 4-1
Chapter 4 The Major Classes of Chemical Reactions 4-1 The Major Classes of Chemical Reactions 4.1 The Role of Water as a Solvent 4.2 Writing Equations for Aqueous Ionic Reactions 4.3 Precipitation Reactions
More informationChapter 4. Reactions in Aqueous Solution. Lecture Presentation. John D. Bookstaver St. Charles Community College Cottleville, MO
Lecture Presentation Chapter 4 in Solution 2012 Pearson Education, Inc. John D. Bookstaver St. Charles Community College Cottleville, MO Properties of Solutions Solute: substance in lesser quantity in
More informationUnit 3 Chemistry - Volumetric Analysis
Unit 3 Chemistry Volumetric Analysis Volumetric analysis is a quantitative chemical analysis used to determine the unknown concentration of one reactant [the analyte] by measuring the volume of another
More information1 Atoms, molecules and stoichiometry try
1 Atoms, molecules and stoichiometry try DEFINITION: Relative atomic mass (Ar) is the average mass of one atom compared to one twelfth of the mass of one atom of carbon-12 DEFINITION: Relative Isotopic
More informationCh. 14/15: Acid-Base Equilibria Sections 14.6, 14.7, 15.1, 15.2
Ch. 14/15: Acid-Base Equilibria Sections 14.6, 14.7, 15.1, 15.2 Creative Commons License Images and tables in this file have been used from the following sources: OpenStax: Creative Commons Attribution
More information2. Relative molecular mass, M r - The relative molecular mass of a molecule is the average mass of the one molecule when compared with
Chapter 3: Chemical Formulae and Equations 1. Relative atomic mass, A r - The relative atomic mass of an element is the average mass of one atom of an element when compared with mass of an atom of carbon-12
More information2.1.3 Amount of substance
2.1.3 Amount of substance The mole is the key concept for chemical calculations DEFINITION: The mole is the amount of substance in grams that has the same number of particles as there are atoms in 12 grams
More informationAcid Base Titration Experiment ACID - BASE TITRATION LAB
ACID - BASE TITRATION LAB MATERIALS and CHEMICALS Burette 50 ml Burette clamp Ring stand Stirring rod Plastic funnel Beakers (50 ml, 100 ml, 400 ml) Graduated cylinder (25 ml, 50 ml) 0.10 M NaOH 0.10 M
More informationStep 2 Calculate the concentration to the correct number of significant figures.
Q1. Calculate the molarity of these solutions: a 1.5 mol of HCl dissolved in 3.0 L of solution b 0.64 g of H 2 SO 4 dissolved in 500 ml of solution c 2.1 g of NaHCO 3 dissolved in 1.00 L of solution A1.
More informationChapter 4. Reactions in Aqueous Solution. Solutions. 4.1 General Properties of Aqueous Solutions
Chapter 4 in Solution 4.1 General Properties of Solutions Solutions Solutions are defined as homogeneous mixtures of two or more pure substances. The solvent is present in greatest abundance. All other
More informationLecture 5. Percent Composition. etc. Professor Hicks General Chemistry II (CHE132) Percent Composition. (aka percent by mass) 100 g.
Lecture 5 Professor Hicks General Chemistry II (CHE132) Percent Composition (aka percent by mass) % by mass component 1 = mass component 1 mass sample 100% sample component 1 100 g sample component 1 component
More information(a) Explain what is happening in stages 1 and 2. (3) (b) (i) Identify the products formed in stages 5, 6 and 7.
1 Hydrated magnesium nitrate, Mg(NO 3 ) 2.6H 2 O, is heated in a boiling tube and the following observations are made. Stage 1 Stage 2 Stage 3 Stage 4 Stage 5 Stage 6 Stage 7 The white solid forms a clear,
More informationRCOOH + R / OH. = 100) is obtained from 1.0 g of RCOOR / (M r. D 75% (Total 1 mark)
Q. An ester is hydrolysed as shown by the following equation. RCOOR / + H O RCOOH + R / OH What is the percentage yield of RCOOH when 0.50 g of RCOOH (M r = 00) is obtained from.0 g of RCOOR / (M r = 50)?
More information5. Formulae, equations and amounts of substance
5. Formulae, equations and amounts of substance The mole is the key concept for chemical calculations DEFINITION: The mole is the amount of substance in grams that has the same number of particles as there
More informationCHEM111 UNIT 1 MOLES, FORMULAE AND EQUATIONS QUESTIONS
Lesson 1 1. (a) Deduce the number of protons, neutrons and electrons in the following species: (i) 37 Cl - (ii) 1 H + (iii) 45 Sc 3+ (b) Write symbols for the following species: (i) 8 protons, 8 neutrons,
More informationChapter 4 Types of Chemical Reaction and Solution Stoichiometry
Chapter 4 Types of Chemical Reaction and Solution Stoichiometry Water, the Common Solvent One of the most important substances on Earth. Can dissolve many different substances. A polar molecule because
More information14-Jul-12 Chemsheets A
www.chemsheets.co.uk 14-Jul-12 Chemsheets A2 009 1 BRONSTED-LOWRY ACIDS & BASES Bronsted-Lowry acid = proton donor (H + = proton) Bronsted-Lowry base = proton acceptor (H + = proton) Bronsted-Lowry acid-base
More informationAP Chemistry. Reactions in Solution
AP Chemistry Reactions in Solution S o l u t i o n s solution: a homogeneous mixture of two or more substances -- The solvent is present in greatest quantity. -- Any other substance present is called a.
More informationA student wanted to make 11.0 g of copper chloride
Q1.A student investigated the reactions of copper carbonate and copper oxide with dilute hydrochloric acid. In both reactions one of the products is copper chloride. (a) Describe how a sample of copper
More informationChemical Reaction Defn: Chemical Reaction: when starting chemical species form different chemicals.
Chemical Reaction Defn: Chemical Reaction: when starting chemical species form different chemicals. Evidence to indicate that a chemical reaction has occurred: Temperature change Different coloured materials
More informationChemistry 143 Experiment #11 Acid Base Titration Dr. Caddell. Titrating Acid
Titrating Acid In this lab you will first determine the concentration of sodium hydroxide in a stock solution that you prepare. You will then use that stock sodium hydroxide solution to titrate a solution
More informationGrade A buffer: is a solution that resists changes in its ph upon small additions of acid or base.sq1
Chapter 15 Lesson Plan Grade 12 402. The presence of a common ion decreases the dissociation. BQ1 Calculate the ph of 0.10M CH 3 COOH. Ka = 1.8 10-5. [H + ] = = ( )( ) = 1.34 10-3 M ph = 2.87 Calculate
More informationCH 221 Chapter Four Part II Concept Guide
CH 221 Chapter Four Part II Concept Guide 1. Solubility Why are some compounds soluble and others insoluble? In solid potassium permanganate, KMnO 4, the potassium ions, which have a charge of +1, are
More information4. Magnesium has three natural isotopes with the following masses and natural abundances:
Exercise #1. Determination of Weighted Average Mass 1. The average mass of pennies minted after 1982 is 2.50 g and the average mass of pennies minted before 1982 is 3.00 g. Suppose that a bag of pennies
More informationTypes of chemical reactions
PowerPoint to accompany Types of chemical reactions Chapters 3 & 16.1 M. Shozi CHEM110 / 2013 General Properties of Aqueous Solutions Solutions are mixtures of two or more pure substances. The solvent
More informationnot to be republished NCERT YOU are already aware that a substance is analysed to establish its qualitative TITRIMETRIC ANALYSIS UNIT-6
UNIT-6 TITRIMETRIC ANALYSIS YOU are already aware that a substance is analysed to establish its qualitative and quantitative chemical composition. Thus, chemical analysis can be categorised as qualitative
More informationRevision Checklist :4.3 Quantitative Chemistry
Revision Checklist :4.3 Quantitative Chemistry Conservation of Mass The law of conservation of mass states that no atoms are lost or made during a chemical reaction so the mass of the products equals the
More informationPage 1. Exam 2 Review Summer A 2002 MULTIPLE CHOICE. 1. Consider the following reaction: CaCO (s) + HCl(aq) CaCl (aq) + CO (g) + H O(l)
Page 1 MULTIPLE CHOICE 1. Consider the following reaction: CaCO (s) + HCl(aq) CaCl (aq) + CO (g) + H O(l) The coefficient of HCl(aq) in the balanced reaction is. a) 1 b) 2 c) 3 d) 4 e) 0 2. Given the information
More informationChapter 7 Solution Chemistry. 7.1 The Nature of Solutions. Warm Up (p. 364) and Quick Check (p. 365)
Chapter 7 Solution Chemistry 7.1 The Nature of Solutions Warm Up (p. 364) and Quick Check (p. 365) Car exhaust Tap water Carbon dioxide Freshly squeezed orange juice Stainless steel Tea Diamond Cigarette
More informationA2 LEVEL CHEMISTRY ACIDS, BASES AND BUFFERS TEST
A2 LEVEL CHEMISTRY 5.1.3 ACIDS, BASES AND BUFFERS TEST Answer all questions Max 50 marks Name.. Mark../50...% Grade Paddington Academy 1 1. A student carried out an investigation with aqueous solutions
More information5. Formulae, equations and amounts of substance
5. Formulae, equations and amounts of substance The mole is the key concept for chemical calculations DEFINITION: The mole is the amount of substance in grams that has the same number of particles as there
More information5. Formulae, equations and amounts of substance
5. Formulae, equations and amounts of substance The mole is the key concept for chemical calculations DEFINITION: The mole is the amount of substance in grams that has the same number of particles as there
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 informationName: C4 TITRATIONS. Class: Question Practice. Date: 97 minutes. Time: 96 marks. Marks: GCSE CHEMISTRY ONLY. Comments:
C4 TITRATIONS Question Practice Name: Class: Date: Time: 97 minutes Marks: 96 marks Comments: GCSE CHEMISTRY ONLY Page of 3 Sodium hydroxide neutralises sulfuric acid. The equation for the reaction is:
More informationH H H H H O H O. Role of Water. Role of Water. Chapter 4. Chemical Reactions in Aqueous Solution H 2 H H H 2 O. Role of H 2 O(l) as solvent.
Role of Water Role of Water Chemical Reactions in Aqueous Solution Role of H 2 O(l) as solvent The polar nature of water molecule Two key features: 1. The distribution of bonding electrons O H covalent
More informationUnit-8 Equilibrium. Rate of reaction: Consider the following chemical reactions:
Unit-8 Equilibrium Rate of reaction: Consider the following chemical reactions: 1. The solution of sodium chloride and silver nitrate when mixed, there is an instantaneous formation of a precipitate of
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 informationPHYSICAL SCIENCES/ P2 1 SEPTEMBER 2015 CAPS CAPE WINELANDS EDUCATION DISTRICT
PHYSICAL SCIENCES/ P2 1 SEPTEMBER 2015 CAPE WINELANDS EDUCATION DISTRICT MARKS 150 TIME 3 hours This question paper consists of 15 pages and 4 data sheets. PHYSICAL SCIENCES/ P2 2 SEPTEMBER 2015 INSTRUCTIONS
More informationChapter 15 Solutions
Chapter 15 Solutions 1. A homogeneous mixture is a combination of two (or more) pure substances that is uniform in composition and appearance throughout. Examples of homogeneous mixtures in the real world
More informationCHEM 1413 Chapter 4 Homework Questions TEXTBOOK HOMEWORK
CHEM 1413 Chapter 4 Homework Questions TEXTBOOK HOMEWORK Chapter 3 3.68 Calculate each of the following quantities: (a) Mass (g) of solute in 185.8 ml of 0.267 M calcium acetate (b) Molarity of 500. ml
More informationAcid-Base Titrations
Chem 1252, General Chemistry I Lab Johnson Acid-Base Titrations Introduction Titration is a convenient quantitative method for accurately determining unknown concentrations of solutions. A necessary requirement
More informationReactions in Aqueous Solution
1 Reactions in Aqueous Solution Chapter 4 For test 3: Sections 3.7 and 4.1 to 4.5 Copyright The McGrawHill Companies, Inc. Permission required for reproduction or display. 2 A solution is a homogenous
More informationVolumetric Analysis: Acids & Bases OL
Name: Volumetric Analysis 1. Concentrations of Solutions Objectives -define solution -define concentration -define molarity -express concentration of solutions in mol/l(molarity), g/l and also in % (v/v)
More informationD. Ammonia can accept a proton. (Total 1 mark)
1. Which statement explains why ammonia can act as a Lewis base? A. Ammonia can donate a lone pair of electrons. B. Ammonia can accept a lone pair of electrons. C. Ammonia can donate a proton. D. Ammonia
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 informationCHM 134 General Chemistry I Exam 2 Review, Dr. Steel. 1. Give the oxidation number of sulfur in each of these compounds.
CHM 1 General Chemistry I Exam Review, Dr. Steel Name 1. Give the oxidation number of sulfur in each of these compounds. H S SO H SO SO -. In the lab you reacted magnesium metal and oxygen gas to produce
More information