   # A 0.015M solution of a base has a pH of 10.09 a) What are the hydronium and hydroxide ion concentrations of this solution? b) Is the base a strong base, a moderately weak base ( K a of about 10 ‒5 ) or a very weak base ( K b of about 10 ‒10 )? ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

#### Solutions

Chapter
Section ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 16, Problem 48PS
Textbook Problem
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## A 0.015M solution of a base has a pH of 10.09 a) What are the hydronium and hydroxide ion concentrations of this solution? b) Is the base a strong base, a moderately weak base (Ka of about 10‒5) or a very weak base (Kb of about 10‒10)?

(a)

Interpretation Introduction

Interpretation: The hydronium and hydroxide ion concentration of the solution has to be calculated.

Concept introduction:

Equilibrium constants:

The equilibrium constant is used to quantitative measurement of the strength of the acid and bases in the water.

Ka is acid constant for equilibrium reactions.

HA + H2OH3O++ A-Ka[H3O+][A-][HA]

Kb is a base constant for equilibrium reaction.

BOH + H2OB++ OH-Ka[B+][OH-][BOH]

Stronger acids have larger Ka value and stronger bases have larger Kb values.

To calculate the hydronium ion concentration and hydroxide ion concentration by using following formula.

pH + pOH=14

### Explanation of Solution

pH = -log[H3O+]The given pH = 10.09 10.09 =  -log[H3O+][H3O+]= 8.1×10-11We know,pH + pOH =14.00pH =10.09         pOH =14 - 10.09                  =3

(b)

Interpretation Introduction

Interpretation:

The ionization constant (Kb) of an unknown base has to be calculated. and the base is a strong base or a moderately weak base or very weak base also to be identified.

Concept introduction:

Equilibrium constants:

The equilibrium constant is used to quantitative measurement of the strength of the acid and bases in the water.

Ka is acid constant for equilibrium reactions.

HA + H2OH3O++ A-Ka[H3O+][A-][HA]

Kb is base constant for equilibrium reaction.

BOH + H2OB++ OH-Ka[B+][OH-][BOH]

Stronger acids have larger Ka value and stronger bases have larger Kb values.

To calculate the hydronium ion concentration and hydroxide ion concentration by using following formula.

pH + pOH=14

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