Solutions for Lecture 21: Acid-Base Equilibrium: Is MIT Water Safe to Drink? | Answer Key - Edubirdie

University:
Massachusetts Institute of Technology
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5.111SC | Principles of Chemical Science
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2019
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Ticaliwm2

LECTURE 21 1. Using the values of Kb provided, calculate the pH and [OH-] for each of the solutions below: (a) 0.30 M ammonia (Kb = 1.8 x 10-5) (b) 0.54 M hydroxylamine (Kb = 1.1 x 10-8) (a) [OH-] = 2.3 x 10-3 M; pH = 11.36 (or 11.37) (b) [OH-] = 7.7 x 10-5 M; pH = 9.89 2. The following reactions are important for buffer creation in biological chemistry labs. Identify the conjugate acid-base pairs. (a) C4H6(OH)3NH2 (aq) + H2O (l) ⇌ C4H6(OH)3NH3+ (aq) + OH- (aq) (b) HPO42- (aq) + HCl (aq) ⇌ H2PO4- (aq) + Cl- (aq) (c) CH3COOH (aq) + H2O (aq) ⇌ CH3COO- (aq) + H3O+ (aq) (a) As written, C4H6(OH)3NH2 is the base and C4H6(OH)3NH3+ (aq) is its conjugate acid. H2O is the acid and OH- is its conjugate base. (b) As written, HPO42- is the base and H2PO4- is its conjugate acid. HCl is the acid and Cl- is its conjugate base. (c) As written, CH3COOH is the acid and CH3COO- is its conjugate base. H2O is the base and H3O+ is its conjugate acid. 3. Ketoacidosis is a serious medical condition caused by a build up of ketone bodies. A 0.50 M solution of one of those ketone bodies, acetoacetic acid, is found to have a pH of 1.95. Determine the Ka of acetoacetic acid. 2.6 x 10-4

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