35 mL of 0.25 M HCIO Solution is titrated to the endpoint with a 0.20 M KOH solution. HCIO Ka= 2.9x10^-8 1. calculate the pH of the initial HCIO solution 2. calculate the volume of KOH needed to reach the equivalence point 3. determine the pH of a solution at half equivalence point of the titration 4. Calculate the pH of the solution at the equivalence point of the titration how do I do the math of these equations?
35 mL of 0.25 M HCIO Solution is titrated to the endpoint with a 0.20 M KOH solution. HCIO Ka= 2.9x10^-8 1. calculate the pH of the initial HCIO solution 2. calculate the volume of KOH needed to reach the equivalence point 3. determine the pH of a solution at half equivalence point of the titration 4. Calculate the pH of the solution at the equivalence point of the titration how do I do the math of these equations?
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter14: Equilibria In Acid-base Solutions
Section: Chapter Questions
Problem 48QAP: A 0.2481 M solution of KOH is used to titrate 30.00 mL of 0.269 M hydrobromic acid. Assume that...
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35 mL of 0.25 M HCIO Solution is titrated to the endpoint with a 0.20 M KOH solution. HCIO Ka= 2.9x10^-8
1. calculate the pH of the initial HCIO solution
2. calculate the volume of KOH needed to reach the equivalence point
3. determine the pH of a solution at half equivalence point of the titration
4. Calculate the pH of the solution at the equivalence point of the titration
how do I do the math of these equations?
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