# 11.6 - concentration will be 0.010 M Calculate the pH of...

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Chem 102B – Discussion Worksheet #19 Weak Acid and Weak Base Calculations 1. I00.00 mL of a 0.10 M solution of acetic acid, CH 3 COOH, has a pH = 2.87 at 25 ° C. Calculate the K a of acetic acid at 25 ° C. a. Write the acid dissociation reaction. b. Write an expression for K a , in terms of the reactants and products of the reaction in (a). c. Write an ICE table for these experimental conditions. d. Solve for [H + ] with the information in your table and equations. You should now have enough information to calculate the value of K a . e. Calculate the % ionization for 0.10 M acetic acid. Can the 5% approximation be used in this case?

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f. If 900.00 mL of water is added to the solution above the new
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Unformatted text preview: concentration will be 0.010 M. Calculate the pH of this 0.010 M solution of acetic acid, using the K a value obtained in (d). g. Calculate the % ionization. Is the % ionization larger or smaller than in the 0.10 M solution? Explain this in terms of Le Chatelierâ€™s principle. (Hint: think about the effects of volume changes on gaseous systems) 2. What is the pH of a 0.0010 M solution of methyl amine, CH 3 NH 2 , with K b = 4.4 x 10-4 . Hint: make sure you check your assumptions. 3. A 0.1 M solution of a monoprotic acid, HA, is 4.2% ionized. What is the K a for this monoprotic acid?...
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## This note was uploaded on 02/14/2011 for the course CHEMISTRY 102 taught by Professor Whitt during the Spring '11 term at University of Illinois, Urbana Champaign.

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11.6 - concentration will be 0.010 M Calculate the pH of...

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