2. A 0.0560 g quantity of acetic acid is dissolved in enough water to make50.0 mL of solution. Calculate the concentrations of H3O*, CH3COO andCH3COOH at equilibrium. What is the pH of the solution? (Ka = 1.8x10-5)— СНCOО- (аq) + НзО* (аq)CH:COOH(аq)a) Calculate the initial concentration of CH3COOH. (C:12; H:1; 0:16)b) Calculate the concentration of CH3COO- (aq) and H3O* (aq) atequilibrium.c) Calculate pH of the solution.

2. A 0.0560 g quantity of acetic acid is dissolved in enough water to make 50.0 mL of solution. Calculate the concentrations of H3O*, CH3COO and CH3COOH at equilibrium. What is the pH of the solution? (Ka = 1.8x10-5) = CH3COO- (aq) + H30* (aq) %3D CH;COOH(aq) a) Calculate the initial concentration of CH3COOH. (C:12; H:1; 0:16) b) Calculate the concentration of CH3COO- (aq) and H3O* (aq) at equilibrium. c) Calculate pH of the solution.

2. A 0.0560 g quantity of acetic acid is dissolved in enough water to make 50.0 mL of solution. Calculate the concentrations of H3O, CH3COO and CH3COOH at equilibrium. What is the pH of the solution? (Ka = 1.8x10-5) = CH3COO- (aq) + H30 (aq) %3D CH;COOH(aq) a) Calculate the initial concentration of CH3COOH. (C:12; H:1; 0:16) b) Calculate the concentration of CH3COO- (aq) and H3O* (aq) at equilibrium. c) Calculate pH of the solution.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter15: Additional Aqueous Equilibria

Section: Chapter Questions

Problem 124QRT

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