T8-1P1 [212 marks] [1 mark] Which is an acid-base conjugate pair? A. H3 O / OH B. H2SO 4 / SO4 C. CH3COOH / H3 O D. CH3NH 3 + / CH3NH2.

Size: px
Start display at page:

Download "T8-1P1 [212 marks] [1 mark] Which is an acid-base conjugate pair? A. H3 O / OH B. H2SO 4 / SO4 C. CH3COOH / H3 O D. CH3NH 3 + / CH3NH2."

Transcription

1 T8-1P1 [212 marks] 1. Which is an acid-base conjugate pair? A. H3 O / OH B. H2SO 4 / SO4 C. CH3COOH / H3 O D. CH3NH 3 + / CH3NH2 2. Which of the following is correct? A. A weak acid is a proton donor and its aqueous solution shows good conductivity. B. A weak acid is a proton donor and its aqueous solution shows poor conductivity. C. A weak acid is a proton acceptor and its aqueous solution shows good conductivity. D. A weak acid is a proton acceptor and its aqueous solution shows poor conductivity. 3. Which species produced by the successive dissociations of phosphoric acid, H3PO 4, are amphiprotic? A. HPO 4 2 and PO4 B. H2PO 4 and HPO4 C. H2PO 4 and PO4 D. HPO 4 2 only 4. Which species acts as a Lewis and Brønsted Lowry base? A. [Al(H2O) 6] 3+ B. BF3 C. NH4 D. OH Soluble acids and bases ionize in water. Sodium hypochlorite ionizes in water. OCl (aq) + H2O(l) OH (aq) + HOCl(aq) 5a. Identify the amphiprotic species.

2 5b. Identify one conjugate acid-base pair in the reaction. A solution containing g of an unknown monoprotic acid, HA, was titrated with mol dm 3 NaOH(aq) cm 3 was required to reach the equivalence point. 5c. Calculate the amount, in mol, of NaOH(aq) used. 5d. Calculate the molar mass of the acid. 5e. Calculate [H + ] in the NaOH solution. 6. Which is a conjugate Brønsted Lowry acid-base pair? A. CH COO 3 / H3 O + B. H O / CH COO 2 3 C. H2O / H3 O + D. CH3COOH / H2O

3 7. Which species behave as Brønsted Lowry bases in the following reaction? H2SO 4 + HNO 3 H2NO HSO4 - A. HNO 3 and HSO4 - B. HNO 3 and H2NO 3 + C. H2SO 4 and HSO 4 - D. H2NO 3 + and HSO4 - Phosphine (IUPAC name phosphane) is a hydride of phosphorus, with the formula PH 3. 8a. (i) Draw a Lewis (electron dot) structure of phosphine. (ii) Outline whether you expect the bonds in phosphine to be polar or non-polar, giving a brief reason. (iii) Explain why the phosphine molecule is not planar. [6 marks] (iv) Phosphine has a much greater molar mass than ammonia. Explain why phosphine has a significantly lower boiling point than ammonia.

4 8b. Phosphine is usually prepared by heating white phosphorus, one of the allotropes of phosphorus, with concentrated aqueous sodium hydroxide. The equation for the reaction is: [10 marks] P4 (s) + 3OH (aq) + 3H2O (l) PH 3 (g) + 3H2PO 2 (aq) (i) Identify one other element that has allotropes and list two of its allotropes. Element: Allotrope 1: Allotrope 2: (ii) The first reagent is written as P 4, not 4P. Describe the difference between P 4 and 4P. (iii) The ion H2PO 2 is amphiprotic. Outline what is meant by amphiprotic, giving the formulas of both species it is converted to when it behaves in this manner. (iv) State the oxidation state of phosphorus in P 4 and H2PO 2. P 4: H2PO 2 : (v) Oxidation is now defined in terms of change of oxidation number. Explore how earlier definitions of oxidation and reduction may have led to conflicting answers for the conversion of P 4 to H2PO 2 and the way in which the use of oxidation numbers has resolved this.

5 2.478 g of white phosphorus was used to make phosphine according to the equation: 8c. P (s) +3OH 4 (aq)+3h2o(l) PH 3(g)+3H2PO 2 (aq) [4 marks] (i) Calculate the amount, in mol, of white phosphorus used. (ii) This phosphorus was reacted with cm 3 of 5.00 mol dm 3 aqueous sodium hydroxide. Deduce, showing your working, which was the limiting reagent. (iii) Determine the excess amount, in mol, of the other reagent. (iv) Determine the volume of phosphine, measured in cm 3 at standard temperature and pressure, that was produced.

6 Phosphine (IUPAC name phosphane) is a hydride of phosphorus, with the formula PH 3. 9a. (i) Draw a Lewis (electron dot) structure of phosphine. (ii) State the hybridization of the phosphorus atom in phosphine. [8 marks] (iii) Deduce, giving your reason, whether phosphine would act as a Lewis acid, a Lewis base, or neither. (iv) Outline whether you expect the bonds in phosphine to be polar or non-polar, giving a brief reason. (v) Phosphine has a much greater molar mass than ammonia. Explain why phosphine has a significantly lower boiling point than ammonia. (vi) Ammonia acts as a weak Brønsted Lowry base when dissolved in water. Outline what is meant by the terms weak and Brønsted Lowry base. Weak: Brønsted Lowry base:

7 9b. Phosphine is usually prepared by heating white phosphorus, one of the allotropes of phosphorus, with concentrated aqueous sodium hydroxide. The equation for the reaction is: [8 marks] (i) The first reagent is written as P 4, not 4P. Describe the difference between P 4 and 4P. (ii) The ion H2PO 2 is amphiprotic. Outline what is meant by amphiprotic, giving the formulas of both species it is converted to when it behaves in this manner. (iii) State the oxidation state of phosphorus in P 4 and H2PO 2. P 4: H2PO 2 : (iv) Oxidation is now defined in terms of change of oxidation number. Explore how earlier definitions of oxidation and reduction may have led to conflicting answers for the conversion of P 4 to H2PO 2 and the way in which the use of oxidation numbers has resolved this.

8 9c g of white phosphorus was used to make phosphine according to the equation: [4 marks] (i) Calculate the amount, in mol, of white phosphorus used. (ii) This phosphorus was reacted with cm 3 of 5.00 mol dm 3 aqueous sodium hydroxide. Deduce, showing your working, which was the limiting reagent. (iii) Determine the excess amount, in mol, of the other reagent. (iv) Determine the volume of phosphine, measured in cm 3 at standard temperature and pressure, that was produced.

9 Impurities cause phosphine to ignite spontaneously in air to form an oxide of phosphorus and water. 9d. (i) g of air was heated by the energy from the complete combustion of 1.00 mol phosphine. Calculate the temperature rise using section 1 of the data booklet and the data below. [9 marks] Standard enthalpy of combustion of phosphine, Specific heat capacity of air = 1.00Jg 1K 1=1.00kJkg 1K 1 (ii) The oxide formed in the reaction with air contains 43.6% phosphorus by mass. Determine the empirical formula of the oxide, showing your method. (iii) The molar mass of the oxide is approximately 285 g mol 1. Determine the molecular formula of the oxide. (iv) State the equation for the reaction of this oxide of phosphorus with water. (v) Suggest why oxides of phosphorus are not major contributors to acid deposition. (vi) The levels of sulfur dioxide, a major contributor to acid deposition, can be minimized by either pre-combustion and post-combustion methods. Outline one technique of each method. Pre-combustion: Post-combustion: Across period 3, elements increase in atomic number, decrease in atomic radius and increase in electronegativity. 10a. Define the term electronegativity.

10 10b. Explain why the atomic radius of elements decreases across the period. 10c. State the equations for the reactions of sodium oxide with water and phosphorus(v) oxide with water. 10d. Suggest the ph of the solutions formed in part (c) (i).

11 10e. Describe three tests that can be carried out in the laboratory, and the expected results, to distinguish between 0.10 moldm 3 HCl(aq) and 0.10 moldm 3 CH 3 COOH(aq). [3 marks] 10f. Explain whether BF can act as a Brønsted-Lowry acid, a Lewis acid or both. 3 Describe the bonding and structure of sodium chloride. 10g.

12 10h. State the formula of the compounds formed between the elements below. Sodium and sulfur: Magnesium and phosphorus: 10i. Covalent bonds form when phosphorus reacts with chlorine to form PCl 3. Deduce the Lewis (electron dot) structure, the shape and [4 marks] bond angle in PCl 3 and explain why the molecule is polar. Lewis (electron dot) structure: Name of shape: Bond angle: Explanation of polarity of molecule: When nitrogen gas and hydrogen gas are allowed to react in a closed container, the following equilibrium is established. N 2 (g) + 3H 2 (g) 2NH 3 (g) ΔH = 92.6 kj Outline two characteristics of a reversible reaction in a state of dynamic equilibrium. 11a.

13 Deduce the equilibrium constant expression, K, for the reaction. 11b. c Predict, with a reason, how each of the following changes affects the position of equilibrium. 11c. The volume of the container is increased. Ammonia is removed from the equilibrium mixture. 11d. Define the term activation energy, E a. Ammonia is manufactured by the Haber process in which iron is used as a catalyst. Explain the effect of a catalyst on the rate of 11e. reaction.

14 Sketch the Maxwell Boltzmann energy distribution curve for a reaction, labelling both axes and showing the activation energy with 11f. and without a catalyst. Typical conditions used in the Haber process are 500 C and 200 atm, resulting in approximately 15% yield of ammonia. 11g. [3 marks] (i) Explain why a temperature lower than 500 C is not used. (ii) Outline why a pressure higher than 200 atm is not often used. Define the term base according to the Lewis theory. 11h. 11i. Define the term weak base according to the Brønsted-Lowry theory.

15 Deduce the formulas of conjugate acid-base pairs in the reaction below. 11j. CH 3 NH 2 (aq) + H 2 O(l) CH 3 NH + 3 (aq) + OH (aq) Outline an experiment and its results which could be used to distinguish between a strong base and a weak base. 11k. [3 marks] This question is about the compounds of some period 3 elements. State the equations for the reactions of sodium oxide with water and phosphorus(v) oxide with water. 12a. Explain why the melting point of phosphorus(v) oxide is lower than that of sodium oxide in terms of their bonding and structure. 12b.

16 12c. Predict whether phosphorus(v) oxide and sodium oxide conduct electricity in their solid and molten states. Complete the boxes with yes or no. Predict and explain the ph of the following aqueous solutions, using equations to support your answer. 12d. Ammonium chloride, NH 4 Cl(aq) : [4 marks] Sodium methanoate, HCOONa(aq) :

17 Acids can be described as strong or weak. 13a. (i) Outline the difference in dissociation between strong and weak acids of the same concentration. [4 marks] (ii) Describe three tests that can be carried out in the laboratory, and the expected results, to distinguish between 0.10 moldm 3 HCl(aq) and 0.10 moldm 3 CH 3 COOH(aq).

18 Calculate the ph, using table 15 of the data booklet, of a solution of ethanoic acid made by dissolving 1.40 g of the acid in distilled [4 marks] 13b. water to make a 500 cm 3 solution.

19 13c. Determine the ph at the equivalence point of the titration and the pk a of an unknown acid using the acid-base titration curve below. [3 marks] Identify, using table 16 of the data booklet, a suitable indicator to show the end-point of this titration. 13d.

20 Describe how an indicator, that is a weak acid, works. Use Le Chatelier s principle in your answer. 13e. 13f. State the formula of the conjugate base of chloroethanoic acid, CH 2 ClCOOH. 13g. Determine the ph of the solution resulting when 100 cm 3 of 0.50 moldm 3 CH 2 ClCOOH is mixed with 200 cm 3 of 0.10 moldm 3 NaOH. [4 marks]

21 Describe how chlorine s position in the periodic table is related to its electron arrangement. 13h. SCl and are two sulfur chloride type compounds with sulfur having different oxidation states. Predict the name of the shape, the bond 13i. 2 SClF 5 angle and polarity of these molecules. When nitrogen gas and hydrogen gas are allowed to react in a closed container the following equilibrium is established. N 2 (g) + 3H 2 (g) 2NH 3 (g) ΔH = 92.6 kj Outline two characteristics of a reversible reaction in a state of dynamic equilibrium. 14a.

22 Predict, with a reason, how each of the following changes affects the position of equilibrium. 14b. The volume of the container is increased. Ammonia is removed from the equilibrium mixture. 14c. Define the term activation energy, E a. Ammonia is manufactured by the Haber process in which iron is used as a catalyst. 14d. Explain the effect of a catalyst on the rate of reaction.

23 Typical conditions used in the Haber process are 500 C and 200 atm, resulting in approximately 15% yield of ammonia. 14e. (i) Explain why a temperature lower than 500 C is not used. [3 marks] (ii) Outline why a pressure higher than 200 atm is not often used. 14f. Deduce the equilibrium constant expression, K c, for the reaction on page g. When 1.00 mol of nitrogen and 3.00 mol of hydrogen were allowed to reach equilibrium in a 1.00 dm 3 container at a temperature of 500 C and a pressure of 1000 atm, the equilibrium mixture contained 1.46 mol of ammonia. Calculate the value of K c at 500 C. Define the term base according to the Lewis theory. 14h.

24 Define the term weak base according to the Brønsted Lowry theory. 14i. 14j. Deduce the formulas of conjugate acid-base pairs in the reaction below. CH 3 NH 2 (aq) + H 2 O(l) CH 3 NH + 3 (aq) + OH (aq) (i) Sketch the ph titration curve obtained when 50.0 cm of is added to of 14k moldm 3 NH 3 (aq) 25.0 cm moldm 3 HCl (aq). [4 marks] (ii) Identify an indicator from table 16 of the data booklet that could be used for this titration.

25 15. Which are acid-base pairs according to the Brønsted Lowry theory? I. HNO 3 /NO 3 II. H 3 O + /OH III. HCOOH/HCOO A. I and II only B. I and III only C. II and III only D. I, II and III 16. What is the conjugate base of phenol, C 6 H 5 OH? A. C 6 H OH 4 B. + C 6 H 5 OH2 C. C 6 H 5 O D. C 6 H + 6 OH A sample of magnesium contains three isotopes: magnesium-24, magnesium-25 and magnesium-26, with abundances of 77.44%, 10.00% and 12.56% respectively. Calculate the relative atomic mass of this sample of magnesium correct to two decimal places. 17a. Predict the relative atomic radii of the three magnesium isotopes, giving your reasons. 17b.

26 17c. Describe the bonding in magnesium. State an equation for the reaction of magnesium oxide with water. 17d. Phosphorus(V) oxide, P 4 O 10 (M r = ), reacts vigorously with water (M r = 18.02), according to the equation below. P 4 O 10 (s) + 6H 2 O(l) 4H 3 PO 4 (aq) A student added 5.00 g of P to 1.50 g of water. Determine the limiting reactant, showing your working. 17e. 4 O 10 Calculate the mass of phosphoric(v) acid, H, formed in the reaction. 17f. 3 PO 4

27 State a balanced equation for the reaction of aqueous H with excess aqueous sodium hydroxide, including state symbols. 17g. 3 PO 4 17h. State the formula of the conjugate base of H 3 PO 4. (i) Deduce the Lewis structure of PH. 17i. + 4 [4 marks] (ii) Predict, giving a reason, the bond angle around the phosphorus atom in PH +. 4 (iii) Predict whether or not the P H bond is polar, giving a reason for your choice.

28 Consider the following list of organic compounds. Compound 1: CH 3 CH 2 CH(OH)CH 3 Compound 2: CH 3 CH 2 COCH 3 Compound 3: CH 3 CH 2 CH 2 OH Compound 4: CH 3 CH 2 CH 2 CHO Apply IUPAC rules to state the names of the four compounds. 18a. [4 marks] (i) 18b. Define the term structural isomers. (ii) Identify the two compounds in the list that are structural isomers of each other.

29 (i) Determine the organic product formed when each of the compounds is heated under reflux with excess acidified potassium 18c. dichromate(vi). If no reaction occurs write NO REACTION in the table. [5 marks] (ii) Describe the colour change during the reactions that occur in part (i). (i) Pentanoic acid reacts with ethanol. State the structural formula of the organic product and the name of the functional group it [3 marks] 18d. contains. (ii) State the type of reaction in part (i).

30 Describe what is meant by a weak Brønsted-Lowry base, including an equation for the reaction of ammonia with water. 18e. [3 marks] 19. What are the conjugate acid base pairs in the following reaction? HCO 3 (aq) + H 2 O(l) OH (aq) + H 2 CO 3 (aq) 20. What are the conjugate acid base pairs in the following reaction? HCO 3 (aq) + H 2 O(l) OH (aq) + H 2 CO 3 (aq) 21. Which of the following is an example of a Lewis acid base reaction, but not a Brønsted Lowry acid base reaction? A. B. C. D. 2CrO 2 4 (aq) + 2H+ (aq) Cr 2 O 2 7 (aq) + H 2 O(l) Co(H 2 O) 2+ 6 (aq) + 4HCl(aq) CoCl 2 4 (aq) + 4H+ (aq) + 6H 2 O(l) NH 3 (aq) + H + (aq) NH + 4 (aq) CH 3 COO (aq) + H 2 O(l) CH 3 COOH(aq) + OH (aq) In acidic solution, ions containing titanium can react according to the half-equation below. TiO 2+ (aq) + 2H + (aq) + e Ti 3+ (aq) + H 2 O(l) 22a. State the initial and final oxidation numbers of titanium and hence deduce whether it is oxidized or reduced in this change.

31 22b. Considering the above equilibrium, predict, giving a reason, how adding more acid would affect the strength of the TiO 2+ ion as an oxidizing agent. A reactivity series comparing titanium, cadmium and europium is given below. Least reactive Cd < Ti < Eu Most reactive The half-equations corresponding to these metals are: Eu 2+ (aq) + 2e Eu(s) Ti 3+ (aq) + 3e Ti(s) Cd 2+ (aq) + 2e Cd(s) 22c. Deduce which of the species would react with titanium metal. Deduce the balanced equation for this reaction. 22d. Deduce which of the six species is the strongest oxidizing agent. 22e.

32 A voltaic cell can be constructed using cadmium and europium half-cells. State how the two solutions involved should be connected 22f. and outline how this connection works. Some students were provided with a moldm 3 solution of a monobasic acid, HQ, and given the problem of determining whether HQ was a weak acid or a strong acid. Define a Brønsted Lowry acid. 22g. Distinguish between the terms strong acid and weak acid. 22h. Neelu and Charles decided to solve the problem by determining the volume of moldm sodium hydroxide solution needed 22i. 3 to neutralize 25.0 cm 3 of the acid. Outline whether this was a good choice.

33 Neelu and Charles decided to compare the volume of sodium hydroxide solution needed with those required by known 22j moldm 3 strong and weak acids. Unfortunately they chose sulfuric acid as the strong acid. Outline why this was an unsuitable choice. 22k. State a suitable choice for both the strong acid and the weak acid. Strong acid: Weak acid: 22l. Francisco and Shamiso decided to measure the ph of the initial solution, HQ, and they found that its ph was 3.7. Deduce, giving a reason, the strength (weak or strong) of the acid HQ. Suggest a method, other than those mentioned above, that could be used to solve the problem and outline how the results would 22m. distinguish between a strong acid and a weak acid. International Baccalaureate Organization 2017 International Baccalaureate - Baccalauréat International - Bachillerato Internacional Printed for BLUPS

T8-3P1 [250 marks] [1 mark] What is the ph of mol dm 3 sodium hydroxide, NaOH(aq)? K = A. 3 B. 4 C. 10 D. 11

T8-3P1 [250 marks] [1 mark] What is the ph of mol dm 3 sodium hydroxide, NaOH(aq)? K = A. 3 B. 4 C. 10 D. 11 T8-3P1 [250 marks] 1. What is the ph of 1.0 10 3 mol dm 3 sodium hydroxide, NaOH(aq)? K = 1.0 10 14 w A. 3 B. 4 C. 10 D. 11 Soluble acids and bases ionize in water. Sodium hypochlorite ionizes in water.

More information

D. Ammonia can accept a proton. (Total 1 mark)

D. 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 information

M10/4/CHEMI/SP2/ENG/TZ1/XX+ CHEMISTRY. Wednesday 12 May 2010 (afternoon) Candidate session number. 1 hour 15 minutes INSTRUCTIONS TO CANDIDATES

M10/4/CHEMI/SP2/ENG/TZ1/XX+ CHEMISTRY. Wednesday 12 May 2010 (afternoon) Candidate session number. 1 hour 15 minutes INSTRUCTIONS TO CANDIDATES M10/4/CHEMI/SP2/ENG/TZ1/XX+ 22106111 CHEMISTRY standard level Paper 2 Wednesday 12 May 2010 (afternoon) 1 hour 15 minutes 0 0 Candidate session number INSTRUCTIONS TO CANDIDATES Write your session number

More information

M08/4/CHEMI/SP2/ENG/TZ2/XX CHEMISTRY. Thursday 8 May 2008 (afternoon) Candidate session number. 1 hour 15 minutes INSTRUCTIONS TO CANDIDATES

M08/4/CHEMI/SP2/ENG/TZ2/XX CHEMISTRY. Thursday 8 May 2008 (afternoon) Candidate session number. 1 hour 15 minutes INSTRUCTIONS TO CANDIDATES M08/4/CHEMI/SP2/ENG/TZ2/XX 22086117 CHEMISTRY standard level Paper 2 Thursday 8 May 2008 (afternoon) 1 hour 15 minutes 0 0 Candidate session number INSTRUCTIONS TO CANDIDATES Write your session number

More information

List, with an explanation, the three compounds in order of increasing carbon to oxygen bond length (shortest first).

List, with an explanation, the three compounds in order of increasing carbon to oxygen bond length (shortest first). T4-2P1 [226 marks] 1. Which statement best describes the intramolecular bonding in HCN(l)? A. Electrostatic attractions between H + and CN ions B. Only van der Waals forces C. Van der Waals forces and

More information

M09/4/CHEMI/SP2/ENG/TZ2/XX CHEMISTRY. Monday 18 May 2009 (afternoon) Candidate session number. 1 hour 15 minutes INSTRUCTIONS TO CANDIDATES

M09/4/CHEMI/SP2/ENG/TZ2/XX CHEMISTRY. Monday 18 May 2009 (afternoon) Candidate session number. 1 hour 15 minutes INSTRUCTIONS TO CANDIDATES M09/4/CHEMI/SP2/ENG/TZ2/XX 22096117 CHEMISTRY standard level Paper 2 Monday 18 May 2009 (afternoon) 1 hour 15 minutes 0 0 Candidate session number INSTRUCTIONS TO CANDIDATES Write your session number in

More information

T2-1P1 [187 marks] [1 mark] How many protons, neutrons and electrons are present in each atom of 31 P? [1 mark]

T2-1P1 [187 marks] [1 mark] How many protons, neutrons and electrons are present in each atom of 31 P? [1 mark] T2-1P1 [187 marks] 1. How many protons, neutrons and electrons are present in each atom of 31 P? 2. What is the atomic number of a neutral atom which has 51 neutrons and 40 electrons? A. 40 B. 51 C. 91

More information

N10/4/CHEMI/SP2/ENG/TZ0/XX CHEMISTRY STANDARD LEVEL PAPER 2. Thursday 11 November 2010 (afternoon) Candidate session number.

N10/4/CHEMI/SP2/ENG/TZ0/XX CHEMISTRY STANDARD LEVEL PAPER 2. Thursday 11 November 2010 (afternoon) Candidate session number. N10/4/CHEMI/SP2/ENG/TZ0/XX 88106105 CHEMISTRY STANDARD LEVEL PAPER 2 Thursday 11 November 2010 (afternoon) 1 hour 15 minutes 0 0 Candidate session number INSTRUCTIONS TO CANDIDATES Write your session number

More information

8.1 Theories of acids and bases

8.1 Theories of acids and bases 8. Acids and bases 8.1 Theories of acids and bases Sour-tasting substances (acids) have been known for thousands of years. Lavoisiers early theory: Acid= a compound of oxygen and a nonmetal. Arrhenius

More information

Basic SL Concepts. D. 2.0 (Total 1 mark) When the equation above is balanced, what is the coefficient for oxygen? D.

Basic SL Concepts. D. 2.0 (Total 1 mark) When the equation above is balanced, what is the coefficient for oxygen? D. Basic SL Concepts 1. 3.0 dm 3 of sulfur dioxide is reacted with.0 dm 3 of oxygen according to the equation below. SO(g) + O(g) SO3(g) What volume of sulfur trioxide (in dm 3 ) is formed? (Assume the reaction

More information

1. Which statement is correct for a crystal of iron(ii) sulfate in a state of equilibrium with a saturated solution of iron(ii) sulfate?

1. Which statement is correct for a crystal of iron(ii) sulfate in a state of equilibrium with a saturated solution of iron(ii) sulfate? 1. Which statement is correct for a crystal of iron(ii) sulfate in a state of equilibrium with a saturated solution of iron(ii) sulfate? A. The colour of the solution darkens as the crystal continues to

More information

IB Chemistry 2 Summer Assignment

IB Chemistry 2 Summer Assignment Name IB Chemistry 2 Summer Assignment 1. What is the sum of all coefficients when the following equation is balanced using the smallest possible whole numbers? C 2 H 2 + O 2 CO 2 + H 2 O A. 5 B. 7 C. 11

More information

Titration curves, labelled E, F, G and H, for combinations of different aqueous solutions of acids and bases are shown below.

Titration curves, labelled E, F, G and H, for combinations of different aqueous solutions of acids and bases are shown below. Titration curves, labelled E, F, G and H, for combinations of different aqueous solutions of acids and bases are shown below. All solutions have concentrations of 0. mol dm 3. (a) In this part of the question,

More information

TOPIC 19 ANSWERS & MARK SCHEMES QUESTIONSHEET 1. ph AND K W

TOPIC 19 ANSWERS & MARK SCHEMES QUESTIONSHEET 1. ph AND K W QUESTIONSHEET 1 a) ph - lg [H + ] / lg 1 [H + ] b) Water ionises slightly as follows: H 2 O(l) ž H + (aq) + OH - (aq) [H + (aq)][oh - (aq)] K c [H 2 O(l)] Since the ionisation is very slight, we regard

More information

ANSWERS Unit 14: Review Acids and Bases

ANSWERS Unit 14: Review Acids and Bases ANSWERS Unit 14: Review Acids and Bases 1) CH 3 COOH(aq) + H 2 0(l) H 3 0 + (aq) + CH 3 COO - (aq) In the equilibrium above, what are the two conjugate bases? A. CH 3 COOH and H 2 0 B. CH 3 COO - and H

More information

QUESTIONSHEETS ACID - BASE EQUILIBRIA. ph OF STRONG ACIDS AND BASES. AND pk a. ph OF ACID OR BASE SOLUTIONS. ph OF MIXED SOLUTIONS OF ACID AND BASE

QUESTIONSHEETS ACID - BASE EQUILIBRIA. ph OF STRONG ACIDS AND BASES. AND pk a. ph OF ACID OR BASE SOLUTIONS. ph OF MIXED SOLUTIONS OF ACID AND BASE CHEMISTRY QUESTIONSHEETS A2 Level A2 TOPIC 19 ACID - BASE EQUILIBRIA Questionsheet 1 Questionsheet 2 Questionsheet 3 Questionsheet 4 Questionsheet 5 Questionsheet 6 Questionsheet 7 Questionsheet 8 Questionsheet

More information

CHEM111 UNIT 1 MOLES, FORMULAE AND EQUATIONS QUESTIONS

CHEM111 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 information

M09/4/CHEMI/SP2/ENG/TZ1/XX+ CHEMISTRY. Monday 18 May 2009 (afternoon) Candidate session number. 1 hour 15 minutes INSTRUCTIONS TO CANDIDATES

M09/4/CHEMI/SP2/ENG/TZ1/XX+ CHEMISTRY. Monday 18 May 2009 (afternoon) Candidate session number. 1 hour 15 minutes INSTRUCTIONS TO CANDIDATES M09/4/EMI/SP2/ENG/TZ1/XX+ 22096111 EMISTRY standard level Paper 2 Monday 18 May 2009 (afternoon) 1 hour 15 minutes 0 0 andidate session number INSTRUTINS T ANDIDATES Write your session number in the boxes

More information

Unit 4: General Principles of Chemistry I Rates, Equilibria and Further Organic Chemistry (including synoptic assessment)

Unit 4: General Principles of Chemistry I Rates, Equilibria and Further Organic Chemistry (including synoptic assessment) Write your name here Surname Other names Edexcel GCE Centre Number Candidate Number Chemistry Advanced Unit 4: General Principles of Chemistry I Rates, Equilibria and Further Organic Chemistry (including

More information

A-level CHEMISTRY (7405/1)

A-level CHEMISTRY (7405/1) SPECIMEN MATERIAL A-level CHEMISTRY (7405/1) Paper 1: Inorganic and Physical Chemistry Specimen 2015 Session Time allowed: 2 hours Materials For this paper you must have: the Data Booklet, provided as

More information

Unit Nine Notes N C U9

Unit Nine Notes N C U9 Unit Nine Notes N C U9 I. AcidBase Theories A. Arrhenius Acids and Bases 1. Acids contain hydronium ions (H O ) commonly referred to as hydrogen ions (H ) that dissociate in water a. Different acids release

More information

... [1] (ii) Draw a dot-and-cross diagram to show the bonding in NH 3

... [1] (ii) Draw a dot-and-cross diagram to show the bonding in NH 3 1 Chemists have developed models for bonding and structure which are used to explain different properties. (a) Ammonia, NH 3, is a covalent compound. Explain what is meant by a covalent bond. Draw a dot-and-cross

More information

M11/4/CHEMI/SPM/ENG/TZ2/XX CHEMISTRY STANDARD LEVEL PAPER 1. Monday 9 May 2011 (afternoon) 45 minutes INSTRUCTIONS TO CANDIDATES

M11/4/CHEMI/SPM/ENG/TZ2/XX CHEMISTRY STANDARD LEVEL PAPER 1. Monday 9 May 2011 (afternoon) 45 minutes INSTRUCTIONS TO CANDIDATES M11/4/CHEMI/SPM/ENG/TZ/XX 116116 CHEMISTRY STANDARD LEVEL PAPER 1 Monday 9 May 011 (afternoon) 45 minutes INSTRUCTIONS TO CANDIDATES Do not open this examination paper until instructed to do so. Answer

More information

SACRED HEART COLLEGE

SACRED HEART COLLEGE SACRED HEART COLLEGE PHYSICAL SCIENCE Preliminary Examination (Grade 12) PAPER 2 25 th JULY 2016 TIME: 3 hours + 10 minutes reading time MARKS: 200 EXAMINER: MODERATOR: Mr F Hollingworth Mr D Armour 1.

More information

CHEMISTRY HIGHER LEVEL

CHEMISTRY HIGHER LEVEL *P15* PRE-LEAVING CERTIFICATE EXAMINATION, 2008 CHEMISTRY HIGHER LEVEL TIME: 3 HOURS 400 MARKS Answer eight questions in all These must include at least two questions from Section A All questions carry

More information

, for C 2. COOH is mol dm [1] COOH by adding water until the total volume is cm 3. for C 2 COOH.

, for C 2. COOH is mol dm [1] COOH by adding water until the total volume is cm 3. for C 2 COOH. 1 A student is supplied with 0.500 mol dm 3 potassium hydroxide, KOH, and 0.480 mol dm 3 propanoic acid, C 2 COOH. The acid dissociation constant, K a, for C 2 COOH is 1.35 10 5 mol dm 3. (a) C 2 COOH

More information

M09/4/CHEMI/SPM/ENG/TZ1/XX+ CHEMISTRY. Monday 18 May 2009 (afternoon) 45 minutes INSTRUCTIONS TO CANDIDATES

M09/4/CHEMI/SPM/ENG/TZ1/XX+ CHEMISTRY. Monday 18 May 2009 (afternoon) 45 minutes INSTRUCTIONS TO CANDIDATES M09/4/CHEMI/SPM/ENG/TZ1/XX+ 22096110 CHEMISTRY standard level Paper 1 Monday 18 May 2009 (afternoon) 45 minutes INSTRUCTIONS TO CANDIDATES Do not open this examination paper until instructed to do so.

More information

N09/4/CHEMI/HP2/ENG/TZ0/XX+ CHEMISTRY HIGHER level. Tuesday 3 November 2009 (afternoon) Candidate session number. 2 hours 15 minutes

N09/4/CHEMI/HP2/ENG/TZ0/XX+ CHEMISTRY HIGHER level. Tuesday 3 November 2009 (afternoon) Candidate session number. 2 hours 15 minutes N09/4/CHEMI/HP/ENG/TZ0/XX+ 8809610 CHEMISTRY HIGHER level Paper Tuesday 3 November 009 (afternoon) hours 15 minutes 0 0 Candidate session number INSTRUCTIONS TO CANDIDATES Write your session number in

More information

1. An aqueous solution of which of the following reacts with magnesium metal?

1. An aqueous solution of which of the following reacts with magnesium metal? 1 1. An aqueous solution of which of the following reacts with magnesium metal? A. Ammonia B. Hydrogen chloride C. Potassium hydroxide D. Sodium hydrogencarbonate 2. Which one of the following species

More information

IB Topics 1 & 11 Multiple Choice Practice

IB 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 information

2 Answer all the questions. 1 This question refers to chemistry of d-block elements in Period 4 (Sc Zn).

2 Answer all the questions. 1 This question refers to chemistry of d-block elements in Period 4 (Sc Zn). 2 Answer all the questions. 1 This question refers to chemistry of d-block elements in Period 4 (Sc Zn). (a) For each statement below, select the symbols of the correct element(s). The element that has

More information

Chapter 2: Acids and Bases

Chapter 2: Acids and Bases 1. Which of the following statements is a correct definition for a Brønsted-Lowry acid? A) Proton acceptor C) Electron pair acceptor B) Electron pair donor D) Proton donor 2. Which of the following statements

More information

Topic 1: Quantitative chemistry

Topic 1: Quantitative chemistry covered by A-Level Chemistry products Topic 1: Quantitative chemistry 1.1 The mole concept and Avogadro s constant 1.1.1 Apply the mole concept to substances. Moles and Formulae 1.1.2 Determine the number

More information

CHEM111 UNIT 1 MOLES, FORMULAE AND EQUATIONS QUESTIONS

CHEM111 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 information

IB Chemistry ABS Introduction An acid was initially considered a substance that would produce H + ions in water.

IB Chemistry ABS Introduction An acid was initially considered a substance that would produce H + ions in water. IB Chemistry ABS Introduction An acid was initially considered a substance that would produce H + ions in water. The Brønsted-Lowry definition of an acid is a species that can donate an H + ion to any

More information

(14) WMP/Jun10/CHEM4

(14) WMP/Jun10/CHEM4 Acids, Bases and ph 14 5 In this question, give all values of ph to two decimal places. Calculating the ph of aqueous solutions can involve the use of equilibrium constants such as K w and K a K w is the

More information

Complete the table to show the relative charge of each particle and the number of each particle found in a 140 Ce 2+ ion.

Complete the table to show the relative charge of each particle and the number of each particle found in a 140 Ce 2+ ion. 1 This question is about the elements with atomic numbers between 58 and 70 (a) Cerium, atomic number 58, is a metal Complete the table to show the relative charge of each particle and the number of each

More information

SIR MICHELANGELO REFALO CENTRE FOR FURTHER STUDIES VICTORIA GOZO

SIR MICHELANGELO REFALO CENTRE FOR FURTHER STUDIES VICTORIA GOZO SIR MICHELANGELO REFALO CENTRE FOR FURTHER STUDIES VICTORIA GOZO Page 1 of 7 Half Yearly Exam 2013 Subject: Chemistry 1 st Year Level: Advanced Time: 3 hrs Answer SEVEN (7) questions. All questions carry

More information

(i) State the time taken for all the peroxodisulfate ions to react. [1] (ii) Suggest a method of measuring the rate of this reaction.

(i) State the time taken for all the peroxodisulfate ions to react. [1] (ii) Suggest a method of measuring the rate of this reaction. 9 (i) State the time taken for all the peroxodisulfate ions to react. [1].............................. minutes (ii) Suggest a method of measuring the rate of this reaction. [1]............................................................................................................................................................................................................................................................................................................................................................................................................................................................................................................................................................................................................................................................

More information

What is an acid? What is a base?

What is an acid? What is a base? What is an acid? What is a base? Properties of an acid Sour taste Turns litmus paper red Conducts electric current Some acids are strong and some are weak Properties of a base Bitter taste Slippery to

More information

Exam Review Questions - Multiple Choice

Exam Review Questions - Multiple Choice Exam Review Questions - Multiple Choice The following questions are for review. They are in no particular order. 1. An atom of iron 56 26Fe has... a) 26 protons, 26 electrons, 30 neutrons b) 30 protons,

More information

14-Jul-12 Chemsheets A

14-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 information

PHYSICAL SCIENCES/ P2 1 SEPTEMBER 2015 CAPS CAPE WINELANDS EDUCATION DISTRICT

PHYSICAL 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 information

(Label the Conjugate Pairs) Water in the last example acted as a Bronsted-Lowry base, and here it is acting as an acid. or

(Label the Conjugate Pairs) Water in the last example acted as a Bronsted-Lowry base, and here it is acting as an acid. or Chapter 16 - Acid-Base Equilibria Arrhenius Definition produce hydrogen ions in aqueous solution. produce hydroxide ions when dissolved in water. Limits to aqueous solutions. Only one kind of base. NH

More information

Chapter 6. Acids, Bases, and Acid-Base Reactions

Chapter 6. Acids, Bases, and Acid-Base Reactions Chapter 6 Acids, Bases, and Acid-Base Reactions Chapter Map Arrhenius Acid Definition Anacid is a substance that generates hydronium ions, H 3 O + (often described as H + ), when added to water. An acidic

More information

2 Answer all the questions. CO, in the presence of aqueous hydrochloric acid, HCl(aq).

2 Answer all the questions. CO, in the presence of aqueous hydrochloric acid, HCl(aq). 2 Answer all the questions. 1 A student investigates the reaction between iodine, I 2, and propanone, (CH 3 ) 2 CO, in the presence of aqueous hydrochloric acid, HCl(aq). The results of the investigation

More information

Chapter 4. The Major Classes of Chemical Reactions 4-1

Chapter 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 information

Aims to increases students understanding of: History, nature and practice of chemistry. Applications and uses of chemistry

Aims to increases students understanding of: History, nature and practice of chemistry. Applications and uses of chemistry Aims to increases students understanding of: History, nature and practice of chemistry Applications and uses of chemistry Implications of chemistry for society and the environment 1. Definitions: Lavoisier

More information

Acids and Bases. A strong base is a substance that completely ionizes in aqueous solutions to give a cation and a hydroxide ion.

Acids and Bases. A strong base is a substance that completely ionizes in aqueous solutions to give a cation and a hydroxide ion. Acid-Base Theories Arrhenius Acids and Bases (1884) Acids and Bases An acid is a substance that, when dissolved in water, increases the concentration of hydrogen ions. A base is a substance that, when

More information

Acids and Bases Unit 11

Acids and Bases Unit 11 Mr. B s Chemistry Acids and Bases Unit 11 Name Block Let s start our discussion of acids and bases by defining some terms that are essential to the topics that follow. Arrhenius acids and bases are: acid

More information

Grace King High School Chemistry Test Review

Grace 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 information

AP Chemistry: Acid-Base Chemistry Practice Problems

AP Chemistry: Acid-Base Chemistry Practice Problems Name AP Chemistry: Acid-Base Chemistry Practice Problems Date Due Directions: Write your answers to the following questions in the space provided. For problem solving, show all of your work. Make sure

More information

Kinetics & Equilibrium Review Packet. Standard Level. 1. Which quantities in the enthalpy level diagram are altered by the use of a catalyst?

Kinetics & Equilibrium Review Packet. Standard Level. 1. Which quantities in the enthalpy level diagram are altered by the use of a catalyst? Kinetics & Equilibrium Review Packet Standard Level 1. Which quantities in the enthalpy level diagram are altered by the use of a catalyst? Enthalpy I II III Time A. I and II only B. I and III only C.

More information

CAMBRIDGE INTERNATIONAL EXAMINATIONS General Certificate of Education Advanced Subsidiary Level and Advanced Level

CAMBRIDGE INTERNATIONAL EXAMINATIONS General Certificate of Education Advanced Subsidiary Level and Advanced Level Centre Number Candidate Number Candidate Name CAMBRIDGE INTERNATIONAL EXAMINATIONS General Certificate of Education Advanced Subsidiary Level and Advanced Level CHEMISTRY 9701/2 PAPER 2 OCTOBER/NOVEMBER

More information

Based on the kinetic molecular theory of gases, which one of the following statements is INCORRECT?

Based on the kinetic molecular theory of gases, which one of the following statements is INCORRECT? 1 Based on the kinetic molecular theory of gases, which one of the following statements is INCORRECT? A) The collisions between gas molecules are perfectly elastic. B) At absolute zero, the average kinetic

More information

2 Answer all the questions.

2 Answer all the questions. 2 Answer all the questions. 1 Born Haber cycles provide a model that chemists use to determine unknown enthalpy changes from known enthalpy changes. In this question, you will use a Born Haber cycle to

More information

2 Answer all the questions. 1 Born Haber cycles can be used to determine lattice enthalpies of ionic compounds

2 Answer all the questions. 1 Born Haber cycles can be used to determine lattice enthalpies of ionic compounds 2 Answer all the questions. 1 Born Haber cycles can be used to determine lattice enthalpies of ionic compounds. (a) Define, in words, the term lattice enthalpy............. [2] (b) The Born Haber cycle

More information

A2 LEVEL CHEMISTRY ACIDS, BASES AND BUFFERS TEST

A2 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 information

15 Acids, Bases, and Salts. Lemons and limes are examples of foods that contain acidic solutions.

15 Acids, Bases, and Salts. Lemons and limes are examples of foods that contain acidic solutions. 15 Acids, Bases, and Salts Lemons and limes are examples of foods that contain acidic solutions. Chapter Outline 15.1 Acids and Bases 15.2 Reactions of Acids and Bases 15.3 Salts 15.4 Electrolytes and

More information

M10/4/CHEMI/SPM/ENG/TZ2/XX+ CHEMISTRY. Wednesday 12 May 2010 (afternoon) 45 minutes INSTRUCTIONS TO CANDIDATES

M10/4/CHEMI/SPM/ENG/TZ2/XX+ CHEMISTRY. Wednesday 12 May 2010 (afternoon) 45 minutes INSTRUCTIONS TO CANDIDATES M10/4/CHEMI/SPM/ENG/TZ/XX+ 106116 CHEMISTRY standard level Paper 1 Wednesday 1 May 010 (afternoon) 45 minutes INSTRUCTIONS TO CANDIDATES Do not open this examination paper until instructed to do so. Answer

More information

Level 2 Chemistry, 2015

Level 2 Chemistry, 2015 91166 911660 2SUPERVISOR S Level 2 Chemistry, 2015 91166 Demonstrate understanding of chemical reactivity 9.30 a.m. Monday 23 November 2015 Credits: Four Achievement Achievement with Merit Achievement

More information

2 Answer all the questions. 1 Born Haber cycles can be used to calculate enthalpy changes indirectly.

2 Answer all the questions. 1 Born Haber cycles can be used to calculate enthalpy changes indirectly. 2 Answer all the questions. 1 Born Haber cycles can be used to calculate enthalpy changes indirectly. (a) The table below shows enthalpy changes for a Born Haber cycle involving potassium sulfide, K 2

More information

moulsham high school 1

moulsham high school 1 moulsham high school 1 a) Interpret the natural direction of change (spontaneous change) as the direction of increasing number of ways of sharing energy and therefore of increasing entropy (positive entropy

More information

State the strongest type of interaction that occurs between molecules of hydrogen peroxide and water.

State the strongest type of interaction that occurs between molecules of hydrogen peroxide and water. Q1.A hydrogen peroxide molecule can be represented by the structure shown. (a) Suggest a value for the H O O bond angle. (b) Hydrogen peroxide dissolves in water. (i) State the strongest type of interaction

More information

for more visit

for more visit JUNE 2011 1. (a) Outline the two essential steps needed to prepare a 0.025mol dm -3 solution of sodium oxalate (Na 2C 20 4) in a 250cm 3 volumetric flask. (RMM of Na 2C 20 4= 134) (2 marks) (b) Determine

More information

Acids and Bases Written Response

Acids and Bases Written Response Acids and Bases Written Response January 1999 4. Consider the salt sodium oxalate, Na2C2O4. a) Write the dissociation equation for sodium oxalate. (1 mark) b) A 1.0M solution of sodium oxalate turns pink

More information

Chemistry 40S Acid-Base Equilibrium (This unit has been adapted from

Chemistry 40S Acid-Base Equilibrium (This unit has been adapted from Chemistry 40S Acid-Base Equilibrium (This unit has been adapted from https://bblearn.merlin.mb.ca) Name: 1 Lesson 1: Defining Acids and Bases Goals: Outline the historical development of acid base theories.

More information

A-level CHEMISTRY 7405/1. Paper 1: Inorganic and Physical Chemistry. SPECIMEN MATERIAL v1.2

A-level CHEMISTRY 7405/1. Paper 1: Inorganic and Physical Chemistry. SPECIMEN MATERIAL v1.2 SPECIMEN MATERIAL v1.2 Please write clearly in block capitals. Centre number Candidate number Surname Forename(s) Candidate signature A-level CHEMISTRY Paper 1: Inorganic and Physical Chemistry Specimen

More information

CHEMISTRY HIGHER LEVEL

CHEMISTRY HIGHER LEVEL *P15* Pre-Leaving Certificate Examination, 2012 Triailscrúdú na hardteistiméireachta, 2012 CHEMISTRY HIGHER LEVEL TIME: 3 HOURS 400 MARKS Answer eight questions in all These must include at least two questions

More information

CHEM 200/202. Professor Jing Gu Office: EIS-210. All s are to be sent to:

CHEM 200/202. Professor Jing Gu Office: EIS-210. All  s are to be sent to: CHEM 200/202 Professor Jing Gu Office: EIS-210 All emails are to be sent to: chem200@mail.sdsu.edu My office hours will be held in GMCS-212 on Monday from 9 am to 11 am or by appointment. ANNOUNCEMENTS

More information

Chemistry Assessment Unit AS 1

Chemistry Assessment Unit AS 1 Centre Number 71 Candidate Number ADVANCED SUBSIDIARY (AS) General Certificate of Education January 2008 Chemistry Assessment Unit AS 1 assessing Module 1: General Chemistry ASC11 [ASC11] THURSDAY 17 JANUARY,

More information

Name Date Class ACID-BASE THEORIES

Name Date Class ACID-BASE THEORIES 19.1 ACID-BASE THEORIES Section Review Objectives Define the properties of acids and bases Compare and contrast acids and bases as defined by the theories of Arrhenius, Brønsted-Lowry, and Lewis Vocabulary

More information

The Acidic Environment

The Acidic Environment The Acidic Environment HSC ENRICHMENT DAY Artchaki Chandrasegar & Alexander Comerford Key points of the acidic environment TODAY, WE WILL FOCUS ON: 1. Definitions: Lavoisier / Davy; Arrhenius; Brønsted-Lowry;

More information

Chapter 14. Objectives

Chapter 14. Objectives Section 1 Properties of Acids and Bases Objectives List five general properties of aqueous acids and bases. Name common binary acids and oxyacids, given their chemical formulas. List five acids commonly

More information

Acids, Bases and Buffers

Acids, Bases and Buffers 1 Acids, Bases and Buffers Strong vs weak acids and bases Equilibrium as it relates to acids and bases ph scale: [H+(aq)] to ph, poh, etc ph of weak acids ph of strong acids Conceptual about oxides (for

More information

Chemistry Assessment Unit A2 1

Chemistry Assessment Unit A2 1 entre Number 71 andidate Number ADVANED General ertificate of Education January 2014 hemistry Assessment Unit A2 1 assessing Periodic Trends and Further Organic, Physical and Inorganic hemistry A212 [A212]

More information

Contents and Concepts

Contents and Concepts Chapter 16 1 Learning Objectives Acid Base Concepts Arrhenius Concept of Acids and Base a. Define acid and base according to the Arrhenius concept. Brønsted Lowry Concept of Acids and Bases a. Define acid

More information

T3-2P3 [51 marks] Bromine is a member of group 7, the halogens. [3 marks] Explain the trend in reactivity of the halogens. 1a.

T3-2P3 [51 marks] Bromine is a member of group 7, the halogens. [3 marks] Explain the trend in reactivity of the halogens. 1a. T3-2P3 [51 marks] Bromine is a member of group 7, the halogens. 1a. Explain the trend in reactivity of the halogens. [3 marks] 1b. Deduce, using equations where appropriate, if bromine reacts with sodium

More information

2. If a gas is released in a reaction (ex: Hydrogen gas bubbles off), is it written as a reactant or a product?

2. If a gas is released in a reaction (ex: Hydrogen gas bubbles off), is it written as a reactant or a product? PRE-AP CHEMISTRY SPRING FINAL EXAM REVIEW Name _ Period Exam Date 100% COMPLETION OF THIS REVIEW BY THE DAY OF YOUR FINAL EXAM WILL COUNT AS A 5 POINT BONUS ADDED TO YOUR FINAL EXAM SCORE. THERE WILL BE

More information

Acid-Base Chemistry & Organic Compounds. Chapter 2

Acid-Base Chemistry & Organic Compounds. Chapter 2 Acid-Base Chemistry & Organic Compounds Chapter 2 Brønsted Lowry Acids & Bases! Brønsted-Lowry Acid: Proton (H + ) Donor! Brønsted-Lowry Base: Proton (H + ) Acceptor! General reaction: HA + B: A - + BH

More information

STRUCTURE AND BONDING

STRUCTURE AND BONDING NAME SCHOOL INDEX NUMBER DATE 1. 1989 Q 6 STRUCTURE AND BONDING The table below gives the distance between atoms (bond lengths) in halogen molecules and the energies required to break the bonds (bond energies)

More information

Paper Reference. Unit Test 6B (Synoptic) Thursday 25 January 2007 Afternoon Time: 1 hour 30 minutes

Paper Reference. Unit Test 6B (Synoptic) Thursday 25 January 2007 Afternoon Time: 1 hour 30 minutes Centre No. Candidate No. Paper Reference 6 2 4 6 0 2 Surname Signature Paper Reference(s) 6246/02 Edexcel GCE Chemistry Advanced Unit Test 6B (Synoptic) Thursday 25 January 2007 Afternoon Time: 1 hour

More information

PHYSICAL SCIENCES: PAPER II

PHYSICAL SCIENCES: PAPER II NATIONAL SENIOR CERTIFICATE EXAMINATION NOVEMBER 2017 PHYSICAL SCIENCES: PAPER II Time: 3 hours 200 marks PLEASE READ THE FOLLOWING INSTRUCTIONS CAREFULLY 1. This question paper consists of 19 pages, a

More information

ACIDS AND BASES. HCl(g) = hydrogen chloride HCl(aq) = hydrochloric acid HCl(g) H + (aq) + Cl (aq) ARRHENIUS THEORY

ACIDS AND BASES. HCl(g) = hydrogen chloride HCl(aq) = hydrochloric acid HCl(g) H + (aq) + Cl (aq) ARRHENIUS THEORY ACIDS AND BASES A. CHARACTERISTICS OF ACIDS AND BASES 1. Acids and bases are both ionic compounds that are dissolved in water. Since acids and bases both form ionic solutions, their solutions conduct electricity

More information

SCH4U Chapter 8 review

SCH4U Chapter 8 review Name: Class: Date: SCH4U Chapter 8 review Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Which statement does not describe a characteristic of acidic

More information

Lesmahagow High School AHChemistry Inorganic and Physical Chemistry Lesmahagow High School CfE Advanced Higher Chemistry

Lesmahagow High School AHChemistry Inorganic and Physical Chemistry Lesmahagow High School CfE Advanced Higher Chemistry Lesmahagow High School CfE Advanced Higher Chemistry Unit 1 Inorganic and Physical Chemistry Chemical Equilibrium 1 Dynamic Equilibrium Revision Dynamic equilibrium happens in a closed system when the

More information

2 Answer all the questions.

2 Answer all the questions. 2 Answer all the questions. 1 A sample of the element boron, B, was analysed using a mass spectrometer and was found to contain two isotopes, 10 B and 11 B. (a) (i) Explain the term isotopes. Complete

More information

10.1 Acids and Bases in Aqueous Solution

10.1 Acids and Bases in Aqueous Solution 10.1 Acids and Bases in Aqueous Solution Arrhenius Definition of Acids and Bases An acid is a substance that gives hydrogen ions, H +, when dissolved in water. In fact, H + reacts with water and produces

More information

NANDI CENTRAL DISTRICT JOINT MOCK 2013

NANDI CENTRAL DISTRICT JOINT MOCK 2013 NAME:. SIGNATURE: INDEX NO:. DATE :.. 233/1 CHEMISTRY PAPER 1 THEORY JULY / AUGUST 2013 TIME: 2 HOURS NANDI CENTRAL DISTRICT JOINT MOCK 2013 Kenya Certificate of Secondary Education (K.C.S.E.) CHEMISTRY

More information

I. Multiple Choice Questions (Type-I) is K p

I. Multiple Choice Questions (Type-I) is K p Unit 7 EQUILIBRIUM I. Multiple Choice Questions (Type-I) 1. We know that the relationship between K c and K p is K p K c (RT) n What would be the value of n for the reaction NH 4 Cl (s) NH 3 (g) + HCl

More information

(B) K2O potassium dioxide

(B) K2O potassium dioxide PRACTICE CHEMISTRY EOC TEST 1. Which substance is a conductor of electricity? (A) NaCl(s) (B) NaCl(l) (C) C6H12O6(s) (D) C6H12O6(l) 2. Which formula is correctly paired with its name? (A) MgCl2 magnesium

More information

AREA 1: WATER. Chapter 6 ACIDS AND BASES. 6.1 Properties of acids and bases

AREA 1: WATER. Chapter 6 ACIDS AND BASES. 6.1 Properties of acids and bases AREA 1: WATER Chapter 6 ACIDS AND BASES 6.1 Properties of acids and bases Acids are: Sour May be corrosive Dissolve in water to produce an electrolyte, Turn blue litmus red Neutralised by bases. Bases

More information

4. Draw a concept map showing the classifications of matter. Give an example of each.

4. Draw a concept map showing the classifications of matter. Give an example of each. Name Bring calculator, pencils, and this completed worksheet to the midterm exam. For problems involving an equation, carry out the following steps: 1. Write the equation. 2. Substitute numbers and units.

More information

3.2.1 Energetics. Enthalpy Change. 263 minutes. 259 marks. Page 1 of 41

3.2.1 Energetics. Enthalpy Change. 263 minutes. 259 marks. Page 1 of 41 ..1 Energetics Enthalpy Change 6 minutes 59 marks Page 1 of 41 Q1. (a) Define the term standard molar enthalpy of formation, ΔH f. (b) State Hess s law. (c) Propanone, CO, burns in oxygen as shown by the

More information

CHEMISTRY - HIGHER LEVEL

CHEMISTRY - HIGHER LEVEL M34 AN ROINN OIDEACHAIS AGUS EOLAÍOCHTA LEAVING CERTIFICATE EXAMINATION, 2002 CHEMISTRY - HIGHER LEVEL TUESDAY, 18 JUNE - AFTERNOON 2.00 to 5.00 400 MARKS Answer eight questions in all These must include

More information

SIR MICHELANGELO REFALO

SIR MICHELANGELO REFALO SIR MICELANGELO REFALO SIXT FORM alf-yearly Exam 2014 Name: CEMISTRY ADV 1 ST 3 hrs ANSWER ANY 7 QUESTIONS. All questions carry equal marks. You are reminded of the importance of clear presentation in

More information

1. Read all questions thoroughly and answer each question completely. ALL WORK MUST BE SHOWN IN ORDER TO RECEIVE ANY CREDIT.

1. Read all questions thoroughly and answer each question completely. ALL WORK MUST BE SHOWN IN ORDER TO RECEIVE ANY CREDIT. INSTRUCTIONS: 1. Read all questions thoroughly and answer each question completely. ALL WORK MUST BE SHOWN IN ORDER TO RECEIVE ANY CREDIT. 2. You will be allowed to use only the given sheet of thermodynamic

More information

Chapter 16 Acid Base Equilibria

Chapter 16 Acid Base Equilibria Chapter 16 Acid Base Equilibria 2015 Pearson Education, Inc. Acid Base Equilibria 16.1 : A Brief Review 16.2 Brønsted Lowry 16.3 The Autoionization of Water 16.4 The ph Scale 16.5 Strong Balsamic Vinegar

More information

Chemistry I Notes Unit 10: Acids and Bases

Chemistry I Notes Unit 10: Acids and Bases Chemistry I Notes Unit 10: Acids and Bases Acids 1. Sour taste. 2. Acids change the color of acid- base indicators (turn blue litmus red). 3. Some acids react with active metals and release hydrogen gas,

More information

Candidates Signature.

Candidates Signature. Name:... Index No..... Date. Candidates Signature. 233/2 CHEMISTRY Paper 2 (THEORY) July/Aug 2016 2HOURS GATUND SUB-COUNTY EVALUATION EXAMINATION Instructions to candidates:- a) Write your name and index

More information