   Chapter 16, Problem 13PS

Chapter
Section
Textbook Problem

What is the pH of a 0.0015 M solution of Ba(OH)2?

Interpretation Introduction

Interpretation:

The pH of 0.0015M solution of Ba(OH)2 has to be calculated.

Concept introduction:

pOH is a measure of hydroxide ion concentration, and pH is a measure of hydrogen ion concentration.

pOH=log[OH]

The sum of pH and pOH must be equal to 14 at 25°C.

pH+pOH=14

Explanation

Beacause Ba(OH)2 is a strong base, it dissociates completely into ions in an aqueous solution as follows:

Ba(OH)2Ba+2+2OH

Given:

The concentration of Ba(OH)2 in a solution is 0.0015M.

The Ba(OH)2 after complete dissociation in an aqueous solution gives two moles of hydroxide ions, therefore the concentration of hydroxide ion is twice of concentration of Ba(OH)2.

[OH]=2×0.0015M=0.003M

pOH is a measure of hydroxide ion concentration, and pH is a measure of hydrogen ion concentration.

pOH=log[OH]                                           �

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