1 .		Does the pH increase, decrease, or remain the same on addition of each of the following? (i) NaNO2 to a solution of HNO2, (ii) HCl to a solution of NaC2H3O2 Online Text [Hint]
2 .		Which one of the following changes is incorrect? Online Text [Hint]
3 .		Which one of the following will lower the pH of a citric acid solution? Online Text [Hint]
4 .		Calculate the pH of a solution of 0.080 M potassium propionate, KC3H5O2, and 0.16 M propionic acid, HC3H5O2 (Ka = 1.3 x 10-5). Online Text [Hint]
5 .		Calculate the pH of a solution containing 0.818 M acetic acid (Ka = 1.76 x 10-5) and 0.172 M sodium acetate. Online Text [Hint]
6 .		Calculate the pH of a solution that is both 0.50 M CH3COOH and 0.50 M CH3COONa (Ka (CH3COOH) is 1.8 x 10-5). Online Text [Hint]
7 .		Calculate the [NH4+] in solution that is 0.25 M NH3 and 0.20 M NaOH (Kb (NH3) = 1.8 x 10-5). Online Text [Hint]
8 .		Calculate the percent ionization of 0.10 M butanoic acid (Ka = 1.5 x 10-5) in a solution containing 0.050 M sodium butanoate. Online Text [Hint]
9 .		Calculate the pH of a buffer that is 0.20 M in formic acid and 0.15 M in sodium formate (Ka = 1.8 x 10-4). Online Text [Hint]
10 .		What is the pH of a buffer prepared from 0.30 M formic acid and 0.15 M potassium formate (Ka = 1.8 x 10-4)? Online Text [Hint]
11 .		What is the ratio of [HCO3-] to [H2CO3] in blood at pH 7.40 (Ka = 4.3 x 10-7)? Online Text [Hint]
12 .		What ratio of the concentration of the bicarbonate ion to the concentration of carbonic acid is necessary to give a buffer with a pH of 7.00 (Ka = 4.3 x 10-7)? Online Text [Hint]
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