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 & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter17: Principles Of Chemical Reactivity: Other Aspects Of Aqueous Equilibria
Section: Chapter Questions
Problem 27PS: Phenol, C6H5OH, is a weak organic acid. Suppose 0.515 g of the compound is dissolved in enough water...
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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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