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ChemistryChemistry: An Atoms First Approach2nd Edition
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Calculate the pH of a 5.0 × 10 −3 - M solution of H 2 SO 4 .

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Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

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Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 13, Problem 112E
Textbook Problem
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Calculate the pH of a 5.0 × 10−3-M solution of H2SO4.

Interpretation Introduction

Interpretation: The pH of the given 5.0×10−3 M solution of H2SO4 is to be calculated.

Concept introduction: The pH of a solution is define as a figure that expresses the acidity of the alkalinity of a given solution.

The pH of a solution is calculated by the formula, pH=−log[H+]

The sum, pH+pOH=14

Explanation of Solution

Explanation

To determine: The pH of the given 5.0×10−3 M solution of H2SO4 .

The [H+] from the first reaction is 5.0×10-3 M_ .

The initial dissociation reaction is,

H2SO4(aq)⇌H+(aq)+HSO4−(aq)

H2SO4 is a strong acid. Hence, in the first step it dissociates into 5.0×10−3 M [H+] and 5.0×10−3 M [HSO4−] .

Therefore, the [H+] from the first reaction is 5.0×10-3 M_ .

The initial [HSO4−] is 5.0×10-3 M_ .

H2SO4 is a strong acid. Hence, in the first step it dissociates into 5.0×10−3 M [H+] and 5.0×10−3 M [HSO4−] .

Therefore, the [HSO4−] from the first reaction is 5.0×10-3 M_ .

The [H+] from second reaction is 0.003 M_ .

The change in concentration of HSO4− is assumed to be x .

The ICE table for the stated reaction is,

HSO4−(aq)⇌H+(aq)+SO42−(aq)Inititial5.0×10−35.0×10−30Change−x+x+xEquilibrium(5.0×10−3)−x(5.0×10−3)+xx

The equilibrium concentration of [HSO4−] is ((5

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