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Chemistry In Focus

7th Edition
Tro + 1 other
Publisher: Cengage Learning,
ISBN: 9781337399692

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BuyFindarrow_forward

Chemistry In Focus

7th Edition
Tro + 1 other
Publisher: Cengage Learning,
ISBN: 9781337399692
Chapter 13, Problem 36E
Textbook Problem
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A chemist makes a 0 .001-M NaOH solution and a 0 .001 -M NH 3 solution. The pH of the NaOH solution is 11. Would you expect the pH of the NH 3 solution to be greater than or less than 11? Explain.

Interpretation Introduction

Interpretation:

The change in pH of an NH3 solution is to be explained.

Concept Introduction:

The pH of an aqueous solution is the measurement of hydrogen ion activity. Here, pH stands for potential of hydrogen. It is represented as

pH=log[H+].

Based on the hydrogen and hydroxide ion concentrations, solutions maybe neutral, acidic, or basic in nature.

If the concentrations of hydrogen ions and hydroxide ions are equal, then the solution will be neutral; if the concentration of hydrogen ions is greater than hydroxide ions, then the solution will be acidic in nature; if the concentration of hydroxide ions is greater than hydrogen ions, then the solution will be basic in nature.

Explanation of Solution

Given information: The pH of NaOH solution is 11.

Water does not react with large number of NH3 molecules in a solution and therefore concentrations of NH3, NH4+ and OH in NH3 solution are high

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Chapter 13 Solutions

Chemistry In Focus
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