Calculate the pH of each solution:(a) 0.0155 M HBr(b) 1.28 × 10?3 M KOH(c) 1.89 × 10?3 M

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

ISBN: 9780321910295 34

Solution for problem 77P Chapter 14

Introductory Chemistry | 5th Edition

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Problem 77P

Calculate the pH of each solution:

(a) 0.0155 M HBr

(b) 1.28 × 10−3 M KOH

(d) 1.54 × 10−4 M Sr(OH)2

Step-by-Step Solution:

Solution:

We have to calculate the pH of each solution

Step 1

(a) 0.0155 M HBr

pH is defined as the negative log of hydrogen or hydronium ion concentration.

pH = - log[H+ ]

pH = - log[H+]

= - log (0.0155)

= - (-1.809)

= 1.809

Thus pH of 0.0155 M HBr is 1.809.

Step 2 of 4

Chapter 14, Problem 77P is Solved

Step 3 of 4

Textbook: Introductory Chemistry

Edition: 5

Author: Nivaldo J Tro

ISBN: 9780321910295

The answer to “Calculate the pH of each solution:(a) 0.0155 M HBr(b) 1.28 × 10?3 M KOH(c) 1.89 × 10?3 M HNO3(d) 1.54 × 10?4 M Sr(OH)2” is broken down into a number of easy to follow steps, and 24 words. This full solution covers the following key subjects: calculate, hbr, hno, koh, solution. This expansive textbook survival guide covers 19 chapters, and 2046 solutions. Introductory Chemistry was written by and is associated to the ISBN: 9780321910295. Since the solution to 77P from 14 chapter was answered, more than 1194 students have viewed the full step-by-step answer. This textbook survival guide was created for the textbook: Introductory Chemistry, edition: 5. The full step-by-step solution to problem: 77P from chapter: 14 was answered by , our top Chemistry solution expert on 05/06/17, 06:45PM.