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QUESTION 7 oe a Analyse the experimental data to determine the relative strength of the acids from strongest to weakest. (A) H SO > H3PO > HCN > CH;COOH (B) H SO >H3PO > CH ;COOH > HCN (C) HCN > CH3COOH > H SO > H3PO 4 (D) HCN > CH3COOH > H3PO > H SO
QUESTION 18 Solution A has a pH of 3 and solution B has a pH of 6. This indicates that solution A 1s (A) (B) (C) (D) less acidic and has 0.5 times the concentration of hydrogen ions in solution B. more acidic and has 2 times the concentration of hydrogen ions in solution B. less acidic and has 0.001 times the concentration of hydrogen ions in solution B. more acidic and has 1000 times the concentration of hydrogen ions in solution B
QUESTION 24 (5 marks) This table shows the effect of temperature on the pH of pure water. Temperature (ÔøΩC) Temperature CO a) Analyse the data to explain whether the self-ionisation of water is endothermic or exothermic. Explain your reasoning. [3 marks] b) Calculate the K of pure water at 50 ÔøΩC. Show your working. [2 marks] (to three significant figures)
QUESTION 5 (17 marks) Compound A reacts with water to produce compound B and hydroxide ions. a) b) c) d) e) CH CH NH (aq) +H O(l) f C HsNH{ (aq) + OH (aq) A B Apply IUPAC rules to name compound A. Identify the Brensted-Lowry acids in the equation. A small amount of hydrochloric acid is added to the equilibrium mixture. Predict the effect of this on the concentration of compound A in the mixture. Explain your reasoning. Calculate the pH of a 2.0 M solution of compound A. State any assumptions. Show your working. (K =5.6x10-*) (to one decimal place) Describe using a balanced chemical equation how Compound A could be made from bromomethane. Include relevant conditions and reagents in your response. [1 mark] [2 marks] [3 marks] [6 marks] [5 marks]
QUESTION 17 Determine the concentration of hydrogen ions (H*) in an aqueous solution containing 1.2 x 10ÔøΩ M hydroxide ions (OH ). (A) 12x10! (B) 83x10? (C) 83x10 (D) 1.2x 10ÔøΩ!ÔøΩ
QUESTION 21 ( marks) Calculate the pH of a 0.1 M aqueous solution of Ba(OH) assuming complete dissociation. Show your working. pH= (to one decimal place)
QUESTION 1 (11 marks) Phosphoric acid (H3PO ) is a common triprotic acid that dissociates fully in three stages. The dissociation equations are shown in the table. to H;PO (aq) +H 0(1) = H PO (aq) +H30*(aq) 71 x103 20 H PO (aq) +H 0(1) = HPO 2-(aq) + H30* (aq) 6.5x10ÔøΩ8 HPO 2 (aq) +H 0(1) = PO 2-(aq)-+ Hy0*(aq) 45x 1073 a) Use the information to determine the strongest Brensted-Lowry acid and its conjugate base. Explain your reasoning. [3 marks] Acid: Conjugate base: Reasoning: b) Identify an amphiprotic species from the dissociation reactions. Explain your reasoning. = /2 marks] c) Determine the Aj value for the strongest conjugate base formed when H3PO has fully dissociated. Show your working. [2 marks] Ky = (to two significant figures) d) Calculate the pH of a 0.05 M solution of dihydrogen phosphate (H PO ). Show your working and state any assumptions made. [4 marks] pH = (to one decimal place)
QUESTION 13 Determine the K of an unknown weak acid (HA) with an aqueous concentration of 0.12 M and a pH of 3.2. (A) 5.2x10ÔøΩ (B) 63x 107 (C) 33x 10ÔøΩ (D) 4.0x 107
QUESTION 22 (2 marks) Calculate the concentration of HF (hydrogen fluoride) in an aqueous solution with a pH of 4.00 (K =7.2 x 10). Show your working. Concentration = mol L7! (to two significant figures)
QUESTION 26 (4 marks) Three unknown 0.1 M solutions A B and C are found to have the following properties. Seiten | HT mett) | pH | pOH a) Determine the pH of solution A. [1 mark] pH= (to one decimal place) b) Determine the concentration of hydrogen ions [HÔøΩ] in solution B. [1 mark] [HÔøΩ] in solution B = mol L ` (to two significant figures) c) Calculate the pOH of solution C. Show your working. [2 marks] pOH = (to one decimal place)
QUESTION 3 (9 marks) A 50.0 mL solution of ethanoic acid (CH;COOH) was titrated with 15.0 mL of 0.10 M sodium hydroxide (NaOH) solution to reach the equivalence point (pK ethanoic acid = 4.76). a) b) Cc) d) Write a balanced chemical equation to indicate how ethanoic acid acts as a Bronsted-Lowry acid during the titration and identify its conjugate base. Determine the Ky of the conjugate base of ethanoic acid. (to two decimal places) Calculate the concentration of the conjugate base at the equivalence point. Show your working. Concentration = M (to three significant figures) Calculate the pH at the equivalence point. Show your working. (to one decimal place) [2 marks] [1 mark] [2 marks] [4 marks]
QUESTION 2 Determine which expression represents the hydrogen ion (H‘) concentration at a pH of 8.4. (A) 1x 10*%*4 (B) 1x 10>° (Cc) 1x 10°? (D) 1x 10°°8
QUESTION 5 (13 marks) The table gives the properties of four monoprotic acids. (a) (b) (Cc) (d —_ (e) a 0.100 4.20 x 102 1.80 x 1074 CH COOH(aq) 0.100 ae 1.78 x 107° HCl(aq) 0.010 1.00 x 102 Determine the relative strength of acids 1 and 2 by contrasting their K values. Write a balanced chemical equation for the dissociation of ethanoic acid (CH ; COOH) in water. Identify whether the conjugate base of ethanoic acid (CH;COOH(aq)) is amphiprotic. Explain your reasoning. Calculate the pH of the aqueous solution of ethanoic acid (CH;COOH). Show your working. Determine the volume of water that would need to be added to 100.0 mL of HCl(aq) to change the pH from 2.00 to 3.00. Explain your reasoning. [3 marks] [2 marks] [2 marks] [3 marks] [3 marks]
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