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Practice 4: Calculate the pH, the pOH, the [H3O+] and [OH-] of a 0.356 M HCIO solution.

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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Practice 4: Calculate the pH, the pOH, the [H3O+]
and [OH-] of a 0.356 M HCIO solution.

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An aqueous solution is found to have an OH- concentration ( [OH-] ) of 1.0 x 10-8 M, a) What is the pOH of the solution? b) What is the pH of the solution? c) What is [H3O+]? d) Is the solution acidic, basic, neutral?
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If 0.50 L 0.20 M HF solution is mixed with solution A to make a mixed solution with a total volume of 1.00 L. Kw = 1.00x10-14; Ka(HF) = 6.6x10-4 at T=298K. (a) If solution A is 0.50 L 0.20 M HNO3, calculate the pH of the mixed solution. Ka(HNO3) = 100 (b) If solution A is 0.50 L 0.20 M NH4CI, calculate the pH of the mixed solution. Ko(NH3) = 1.8×10-5 %3D (c) If solution A is 0.50 L 0.20 M HNO2, calculate the pH of the mixed solution. Ka(HNO2) = 5.1×104 Hint: First list an equation that shows electrical neutrality in the solution. Also, neglect the [H*] contribution from water. Then use [H*] and the equilibrium constant(s) to express the anion concentrations in the equation you obtained for electrical neutrality, and you will find there is single unknown [H*] in the equation.
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