The sample of 30.00 mL of 0.015 M HClO is titrated with a 20.00 mL of a 0.015 M NaOH solution. (a) Show the reaction between HClO and OH–. (b) What is the final volume after two solutions were mixed?
The sample of 30.00 mL of 0.015 M HClO is titrated with a 20.00 mL of a 0.015 M NaOH solution. (a) Show the reaction between HClO and OH–. (b) What is the final volume after two solutions were mixed?
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter16: Acid-base Equilibria
Section: Chapter Questions
Problem 16.42QP: A chemist wanted to determine the concentration of a solution of lactic acid, HC3H5O3. She found...
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The sample of 30.00 mL of 0.015 M HClO is titrated with a 20.00 mL of a 0.015 M NaOH solution.
(a) Show the reaction between HClO and OH–.
(b) What is the final volume after two solutions were mixed?
(c) What is the final molarity of HClO after the reaction with OH–?
(d) What is the pH after 20.0 mL of the NaOH solution is added? (Ka of HClO is 3.0*10–8)?
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