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A 0.15 M solution of HIO2 is being titrated with a 0.15 M solution of NaOH. 20.0 mL of the HIO2 is placed in a beaker with a pH probe and the NaOH is placed in a buret and added to the beaker in small amounts. The Ka of HIO2 is 3.2 x 1o-5. a) What is the pH of the acid before any NaOH is added? QUESTION 5 b) What would be the pH at the equivalence point? QUESTION 6 c) What would be the pH 2.00 mL before the equivalence point? QUESTION 7 d) What would be the pH 2.00 mL after the equivalence point?

A 0.15 M solution of HIO2 is being titrated with a 0.15 M solution of NaOH. 20.0 mL of the HIO2 is placed in a beaker with a pH probe and the NaOH is placed in a buret and added to the beaker in small amounts. The Ka of HIO2 is 3.2 x 1o-5. a) What is the pH of the acid before any NaOH is added? QUESTION 5 b) What would be the pH at the equivalence point? QUESTION 6 c) What would be the pH 2.00 mL before the equivalence point? QUESTION 7 d) What would be the pH 2.00 mL after the equivalence point?

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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A 0.15 M solution of HIO2 is being titrated with a 0.15 M solution of NaOH. 20.0 mL of the HIO2 is placed in a beaker with a pH probe and the NaOH is placed in a buret and added to the beaker in small amounts. The Ka of HIO2 is 3.2 x 10-5. a) What is the pH of the acid before any NaOH is added? QUESTION 5 b) What would be the pH at the equivalence point? QUESTION 6 c) What would be the pH 2.00 mL before the equivalence point? QUESTION 7 d) What would be the pH 2.00 mL after the equivalence point?
Transcribed Image Text:A 0.15 M solution of HIO2 is being titrated with a 0.15 M solution of NaOH. 20.0 mL of the HIO2 is placed in a beaker with a pH probe and the NaOH is placed in a buret and added to the beaker in small amounts. The Ka of HIO2 is 3.2 x 10-5. a) What is the pH of the acid before any NaOH is added? QUESTION 5 b) What would be the pH at the equivalence point? QUESTION 6 c) What would be the pH 2.00 mL before the equivalence point? QUESTION 7 d) What would be the pH 2.00 mL after the equivalence point?
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