(15 points) A buffer solution is prepared from equal volumes of 0.200 M acetic acid and 0.600 M sodium acetate. (a) What is the pH of the solution? (b) Is the solution acidic or basic? (c) What is the pH of a solution that results when 3.00 mL of 0.034 M HCI is added to 0.200 L of the original buffer? CH3CO2H(aq) + H2O(3) H30° (aq) + CH3CO2 (aq) ka = 1.8 x 10-5

(15 points) A buffer solution is prepared from equal volumes of 0.200 M acetic acid and 0.600 M sodium acetate. (a) What is the pH of the solution? (b) Is the solution acidic or basic? (c) What is the pH of a solution that results when 3.00 mL of 0.034 M HCI is added to 0.200 L of the original buffer? CH3CO2H(aq) + H2O(3) H30° (aq) + CH3CO2 (aq) ka = 1.8 x 10-5

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.71PAE: Acrylic acid is used in the polymer industry in the production of acrylates. Its K, is 5.6 X 10“’....

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You prepared 500 mL buffer solution that contains 0.50 moles monoprotic weak acid (HA) and 0.30 moles conjugate base (NaA). The solution has a pH of 4.20. (a) What is the Kp of the conjugate base, NaA? (b) What is the pH of the buffer solution after adding 400 mL of 0.30 M H,SO4? pH = pKa – log(THA), [A*]
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