   Chapter 14, Problem 112E

Chapter
Section
Textbook Problem

# Calculate the pH of a 5.0 × 10−3-M solution of H2SO4.

Interpretation Introduction

Interpretation: The pH of the given 5.0×103M 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

Explanation

To determine: The pH of the given 5.0×103M solution of H2SO4 .

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

The initial dissociation reaction is,

H2SO4(aq)H+(aq)+HSO4(aq)

H2SO4 is a strong acid. Hence, in the first step it dissociates into 5.0×103M [H+] and 5.0×103M [HSO4] .

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

The initial [HSO4] is 5.0×10-3M_ .

H2SO4 is a strong acid. Hence, in the first step it dissociates into 5.0×103M [H+] and 5.0×103M [HSO4] .

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

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

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)Inititial5.0×1035.0×1030Changex+x+xEquilibrium(5.0×103)x(5.0×103)+xx

The equilibrium concentration of [HSO4] is ((5

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