   Chapter 14, Problem 168CWP

Chapter
Section
Textbook Problem

# Calculate the pH of the following solutions:a. 1.2 M CaBr2b. 0.84 M C6H5NH3NO3 (Kb for C6H5NH2 = 3.8 × 10−10)c. 0.57 M KC7H5O2 (Ka for HC7H5O2 = 6.4 × 10−5)

(a)

Interpretation Introduction

Interpretation: The pH of the given solutions is to be calculated.

Concept introduction: Strong acids dissociate completely and rapidly when dissolved in an aqueous solution and have a very large value of Ka and a lower value of pH while the weak acids dissociate partially and slowly in an aqueous solution and have a very low value of Ka.and a higher value of pH.

To determine: The pH of 1.2MCaBr2 solution.

Explanation

The pH of CaBr2 solution is 7_.

The strong salts like CaBr2 are formed by the reaction between a strong acid and a strong base

(b)

Interpretation Introduction

Interpretation: The pH of the given solutions is to be calculated.

Concept introduction: Strong acids dissociate completely and rapidly when dissolved in an aqueous solution and have a very large value of Ka and a lower value of pH while the weak acids dissociate partially and slowly in an aqueous solution and have a very low value of Ka.and a higher value of pH.

To determine: The pH of 0.84MC6H5NH3NO3 solution.

(c)

Interpretation Introduction

Interpretation: The pH of the given solutions is to be calculated.

Concept introduction: Strong acids dissociate completely and rapidly when dissolved in an aqueous solution and have a very large value of Ka and a lower value of pH while the weak acids dissociate partially and slowly in an aqueous solution and have a very low value of Ka.and a higher value of pH.

To determine: The pH of 0.57MKC7H5O2 solution.

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