# Chapter 16, Problem 16.26QP

### Chemistry: Atoms First

3rd Edition
Julia Burdge + 1 other
ISBN: 9781259638138

Chapter
Section

### Chemistry: Atoms First

3rd Edition
Julia Burdge + 1 other
ISBN: 9781259638138

(a)

Interpretation Introduction

Interpretation: The pH of the given solutions has to be calculated

Concept Information:

pH definition:

The concentration of hydrogen ion is measured using pH scale. The acidity of aqueous solution is expressed by pH scale.

The pH of a solution is defined as the negative base-10 logarithm of the hydrogen or hydronium ion concentration.

pH=-log[H+]

Relationship between pH and pOH

pOH is similar to pH .  The only difference is that in pOH the concentration of hydroxide ion is used as a scale while in pH , the concentration of hydronium ion is used.

The equation of equilibrium for autoionization of water is,

Kw=[H+][OH-]

The equilibrium expression for water at 25oC is,

[H+][OH-]= 1×10-14

Taking negative logarithm on both sides, we get

log([H+][OH-])= -log(1×10-14)(log[H+])+(-log[OH-])= 14)

The relationship between the hydronium ion concentration and the hydroxide ion concentration is given by the equation,

pH+pOH=14,at25oC

As pOH and pH are opposite scale, the total of both has to be equal to 14.

To Calculate: The pH of the given solutions

(b)

Interpretation Introduction

Interpretation: The pH of the given solutions has to be calculated

Concept Information:

pH definition:

The concentration of hydrogen ion is measured using pH scale. The acidity of aqueous solution is expressed by pH scale.

The pH of a solution is defined as the negative base-10 logarithm of the hydrogen or hydronium ion concentration.

pH=-log[H+]

Relationship between pH and pOH

pOH is similar to pH .  The only difference is that in pOH the concentration of hydroxide ion is used as a scale while in pH , the concentration of hydronium ion is used.

The equation of equilibrium for autoionization of water is,

Kw=[H+][OH-]

The equilibrium expression for water at 25oC is,

[H+][OH-]= 1×10-14

Taking negative logarithm on both sides, we get

log([H+][OH-])= -log(1×10-14)(log[H+])+(-log[OH-])= 14)

The relationship between the hydronium ion concentration and the hydroxide ion concentration is given by the equation,

pH+pOH=14,at25oC

As pOH and pH are opposite scale, the total of both has to be equal to 14.

To Calculate: The pH of the given solutions

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