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Calculate the pH of each solution.(a) [OH?] = 2.8 × 10?11

Introductory Chemistry | 5th Edition | ISBN: 9780321910295 | Authors: Nivaldo J Tro ISBN: 9780321910295 34

Solution for problem 74P Chapter 14

Introductory Chemistry | 5th Edition

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Introductory Chemistry | 5th Edition | ISBN: 9780321910295 | Authors: Nivaldo J Tro

Introductory Chemistry | 5th Edition

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Problem 74P

Calculate the pH of each solution.

(a) [OH−] = 2.8 × 10−11 M

(b) [OH−] = 9.6 × 10−3 M

(c) [OH−] = 3.8 × 10−12 M

(d) [OH−] = 6.4 × 10−4 M

Step-by-Step Solution:

Solution 74P :

Step 1:

Here, we have to pH of each solution :

pOH is the measure of concentration of hydroxide ion (OH-) in the solution. It is used to measure the alkalinity of a solution.

To calculate the pOH of a solution we should know the concentration of the hydroxide ion in moles per liter, i.e the molarity of the solution.

pOH is calculated using the expression:                                        pOH =  - log [OH-]

Step 2 of 2

Chapter 14, Problem 74P is Solved
Textbook: Introductory Chemistry
Edition: 5
Author: Nivaldo J Tro
ISBN: 9780321910295

Since the solution to 74P from 14 chapter was answered, more than 244 students have viewed the full step-by-step answer. This full solution covers the following key subjects: calculate, solution. This expansive textbook survival guide covers 19 chapters, and 2045 solutions. Introductory Chemistry was written by and is associated to the ISBN: 9780321910295. This textbook survival guide was created for the textbook: Introductory Chemistry, edition: 5. The answer to “Calculate the pH of each solution.(a) [OH?] = 2.8 × 10?11 M(b) [OH?] = 9.6 × 10?3 M(c) [OH?] = 3.8 × 10?12 M(d) [OH?] = 6.4 × 10?4 M” is broken down into a number of easy to follow steps, and 30 words. The full step-by-step solution to problem: 74P from chapter: 14 was answered by , our top Chemistry solution expert on 05/06/17, 06:45PM.

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