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.

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Chapter1: Chemical Foundations
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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)
— 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) at
equilibrium.
c) Calculate pH of the solution.
Transcribed Image Text: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) — 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) at equilibrium. c) Calculate pH of the solution.
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