73. Calculate the pH of each solution.(a) [OH-] = 1.9 × 10-7 M(b) [OH-] = 2.6 ×10-8 M(c) [OH-] =7.2 × 10¯ M(d) [OH¯] = 9.5 × 10-2 M

pH of the solution is given by the formula, pH =14-pOH =14-(-log[OH-])

Answered: Calculate the pH of each solution. (a)…

Calculate the pH of each solution. (a) [OH-] = 1.9 × 10-7 M (b) [OH-] = 2.6 × 10-8 M 10-¹¹ M (c) [OH-] = 7.2 × (d) [OH-] = 9.5 × 10-² M

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 10QAP: Calculate [OH-] and pH in a solution in which the hydrogen sulfite ion, HSO3-, is 0.429 M and the...

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Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

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Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

73. Calculate the pH of each solution.
(a) [OH-] = 1.9 × 10-7 M
(b) [OH-] = 2.6 ×
10-8 M
(c) [OH-] =
7.2 × 10¯ M
(d) [OH¯] = 9.5 × 10-2 M

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