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AQUEOUS EQUILIBRIA PROBLEM SET

This problem set covers key concepts in aqueous equilibria, focusing on pH calculations and buffer preparation. It includes practical scenarios such as mixing weak acids and bases, calculating hydrogen ion concentrations in different solutions, and determining the ratio of components required to create a specific pH buffer. Students will calculate pH changes upon the addition of strong acids to weak base solutions, as well as apply the Henderson-Hasselbalch equation and Kb values for various substances.

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AQUEOUS EQUILIBRIA PROBLEM SET

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  1. AQUEOUS EQUILIBRIA PROBLEM SET

  2. 1. Calculate the [H+] in a solution formed by mixing 50.0 ml of 0.10 M HCN (Ka = 4.95 x 10-10) with 50.0 mL of 0.50 M NaCN.  2. To make a buffer of pH = 4.25 from acetic acid (Ka = 1.80 x 10-5) and sodium acetate, what is the ratio of NaC2H3O2 to HC2H3O2 needed?  3. A solution contains 1.0 M NH4Cl and 1.0 M NH3. Kb = 1.8 x 10-5 a. Calculate the pH. b. Calculate the pH after 0.10 mole HCl gas is bubbled into 1.0 L of the original solution.

  3. 4. A solution is made by combining 500.0 mL of 2.00 M C5H5N (pyridine) and 500.0 mL of 0.200 M C5H5NHCl (pyridinium chloride). (Kb = 1.7 x 10-9 for pyridine) a. Calculate the [OH-] in this solution. b. Calculate the [OH-] in the solution after 0.0080 mole of KOH is added.  5. Consider a solution of the weak base aniline C6H5NH2 (Kb = 4.0 x 10-10). What is the pH of a solution prepared by adding 50.0 mL of 0.10 M aniline to 50.0 mL of 0.10 M HCl?

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