Chapter 20.7, Problem 1.3ACP

### Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074

Chapter
Section

### Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
Textbook Problem

# What is the concentration of HClO in a 0.010 M solution of ClO−? What is the pH of this solution?

Interpretation Introduction

Interpretation:

The concentration of HClO in a 0.010M solution of ClO and pH of the solution should be determined.

Concept introduction:

• The relation between acidic and basic constants KaandKb with Kw (equilibrium constant for water) is,

Ka=1Kb×KwKw=Kb×Ka

• Kw can be written in another way as Kw=[H3O+][OH]
• pH: The concentration of hydrogen ion is measured using pH scale.  The acidity of aqueous solution is expressed by pH scale.
• pOH: The pOH of a solution is defined as the negative base-10 logarithm of the hydroxide ion [OH-] concentration. pOH scale is analogous to pH scale.
• pH=log[H3O+]
• pOH=log[OH]
Explanation

The balanced chemical reaction equation for the given reaction is,

Cl2(g)+2H2O(l)HClO(aq)+H3O(aq)++Claq

The relation between acidic and basic constants KaandKb with Kw (equilibrium constant for water) is,

Ka=1Kb×KwKw=Kb×Ka

The value of Kb for the reaction is 2.86×107. Considering the concentration of HClO as x,

Then

Kb=KwKa=2.86×10-7=x2(0.010-x)x=5

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