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Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425

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BuyFindarrow_forward

Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425
Textbook Problem
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. Strong buses are bases that completely ionize in water to produce hydroxide ion, OH-. The strong bases include the hydroxides of the Group I elements. For example, if 1.0 mole of NaOH is dissolved per liter, the concentration of OH ion is 1.0 M. Calculate the [OH-], pOH, and pH for each of the following strong base solutions.

a. 1.10 M NaOH

b. 2.0 × 10 4 M KOH

c. 6.2 × 10 3 M CsOH

d. 0.0001 M NaOH

Interpretation Introduction

(a)

Interpretation:

The pOH, pH and concentration of OH- ions should be calculated.

Concept Introduction:

A strong base ionized 100 % and releases OH- ions in its solution. The relation between pOH, pH and concentration of OH- ions is:

pOH = - log [OH-]pH + pOH = 14pH = 14 - pOH.

Explanation

Since, [NaOH] = 0.10 M

And, NaOHNa++ OH-

Thus, [NaOH] = [OH-] = 0

(b)

Interpretation Introduction

Interpretation:

The pOH, pH and concentration of OH- ions should be calculated.

Concept Introduction:

A strong base ionized 100 % and releases OH- ions in its solution. The relation between pOH, pH and concentration of OH- ions is:

pOH = - log [OH-]pH + pOH = 14pH = 14 - pOH.

(c)

Interpretation Introduction

Interpretation:

The pOH, pH and concentration of OH- ions should be calculated.

Concept Introduction:

A strong base ionized 100 % and releases OH- ions in its solution. The relation between pOH, pH and concentration of OH- ions is:

pOH = - log [OH-]pH + pOH = 14pH = 14 - pOH.

(d)

Interpretation Introduction

Interpretation:

The pOH, pH and concentration of OH- ions should be calculated.

Concept Introduction:

A strong base ionized 100 % and releases OH- ions in its solution. The relation between pOH, pH and concentration of OH- ions is:

pOH = - log [OH-]pH + pOH = 14pH = 14 - pOH.

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