The interconversions given below have to be done and in each case whether the solution is acidic or basic has to be estimated. Concept Introduction: The relationship between p H a n d p O H is given below. p H + p O H = 14 Other relations are given below. p H = − log [ H 3 O + ] p O H = − log [ O H − ] K w = [ H 3 O + ] [ O H − ] = 10 − 14 If the p H of a solution is less than 7 , then the solution is acidic. If the p H of a solution is greater than 7 , then the solution is basic.

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Answer 1

Question

Chapter 14, Problem 34QRT

Interpretation Introduction

Interpretation:

The interconversions given below have to be done and in each case whether the solution is acidic or basic has to be estimated.

Concept Introduction:

The relationship between pH and pOH is given below.

pH+pOH=14

Other relations are given below.

pH=−log[H3O+]pOH=−log[OH−]Kw=[H3O+][OH−]=10−14

If the pH of a solution is less than 7, then the solution is acidic. If the pH of a solution is greater than 7, then the solution is basic.

Expert Solution & Answer

Explanation of Solution

(a) [H3O+]=6.1×10-7M

The pH of the solution can be calculated as given below.

pH=−log[H3O+]=−log[6.1×10−7]=6.21.

Then,

pH+pOH=14pOH=14−pH=14−6.21=7.79.[OH−]=10−pOH=10−7.79=1.6×10-8M.

As the pH of the solution is less than 7, the solution is acidic.

(b) [OH−]=2.2×10-9M

The pOH of the solution can be calculated as given below.

pOH=−log[OH−]=−log[2.2×10−9]=8.66.

Then,

pH+pOH=14pH=14−pOH=14−8.66=5.34.[H3O+]=10−pH=10−5.34=4.5×10-6M.

As the pH of the solution is greater than 7, the solution is basic.

(c) pH=4.67

The relationship between pH and pOH is given below.

pH+pOH=14

Therefore,

pH+pOH=14pOH=14−pH=14−4.67=9.33.

The concentration of H3O+ and OH− ion can be calculated as given below.

pH=−log[H3O+][H3O+]=10−pH=10−4.67=2.1×10-5M.pOH=−log[OH−][OH−]=10−pOH=10−9.33=4.7×10-10M.

As the pH of the solution is less than 7, the solution is acidic.

(d) [H3O+]=2.5×10-2M

The pH of the solution can be calculated as given below.

pH=−log[H3O+]=−log[2.5×10−2]=1.60.

Then,

pH+pOH=14pOH=14−pH=14−1.60=12.40.[OH−]=10−pOH=10−12.40=4.0×10-13M.

As the pH of the solution is less than 7, the solution is acidic.

(e) pH=9.12

The relationship between pH and pOH is given below.

pH+pOH=14

Therefore,

pH+pOH=14pOH=14−pH=14−9.12=4.88.

The concentration of H3O+ and OH− ion can be calculated as given below.

pH=−log[H3O+][H3O+]=10−pH=10−9.12=7.6×10-10M.pOH=−log[OH−][OH−]=10−pOH=10−4.88=1.3×10-5M.

As the pH of the solution is greater than 7, the solution is basic.

Now, the table can be filled as given below.

Now, the complete table can be given as shown below.

pH	[H3O+]M	[OH−]M	Nature
(a) 6.21	6.1×10-7	1.6×10-8	Acidic
(b) 5.34	4.5×10-6	2.2×10-9	Acidic
(c) 4.67	2.1×10-5	4.7×10-10	Acidic
(d) 1.60	2.5×10-2	4.0×10-13	Acidic
(e) 9.12	7.6×10-10	1.3×10-5	Basic

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Answer 2

Question

Chapter 14, Problem 34QRT

Interpretation Introduction

Interpretation:

The interconversions given below have to be done and in each case whether the solution is acidic or basic has to be estimated.

Concept Introduction:

The relationship between pH and pOH is given below.

pH+pOH=14

Other relations are given below.

pH=−log[H3O+]pOH=−log[OH−]Kw=[H3O+][OH−]=10−14

If the pH of a solution is less than 7, then the solution is acidic. If the pH of a solution is greater than 7, then the solution is basic.

Expert Solution & Answer

Explanation of Solution

(a) [H3O+]=6.1×10-7M

The pH of the solution can be calculated as given below.

pH=−log[H3O+]=−log[6.1×10−7]=6.21.

Then,

pH+pOH=14pOH=14−pH=14−6.21=7.79.[OH−]=10−pOH=10−7.79=1.6×10-8M.

As the pH of the solution is less than 7, the solution is acidic.

(b) [OH−]=2.2×10-9M

The pOH of the solution can be calculated as given below.

pOH=−log[OH−]=−log[2.2×10−9]=8.66.

Then,

pH+pOH=14pH=14−pOH=14−8.66=5.34.[H3O+]=10−pH=10−5.34=4.5×10-6M.

As the pH of the solution is greater than 7, the solution is basic.

(c) pH=4.67

The relationship between pH and pOH is given below.

pH+pOH=14

Therefore,

pH+pOH=14pOH=14−pH=14−4.67=9.33.

The concentration of H3O+ and OH− ion can be calculated as given below.

pH=−log[H3O+][H3O+]=10−pH=10−4.67=2.1×10-5M.pOH=−log[OH−][OH−]=10−pOH=10−9.33=4.7×10-10M.

As the pH of the solution is less than 7, the solution is acidic.

(d) [H3O+]=2.5×10-2M

The pH of the solution can be calculated as given below.

pH=−log[H3O+]=−log[2.5×10−2]=1.60.

Then,

pH+pOH=14pOH=14−pH=14−1.60=12.40.[OH−]=10−pOH=10−12.40=4.0×10-13M.

As the pH of the solution is less than 7, the solution is acidic.

(e) pH=9.12

The relationship between pH and pOH is given below.

pH+pOH=14

Therefore,

pH+pOH=14pOH=14−pH=14−9.12=4.88.

The concentration of H3O+ and OH− ion can be calculated as given below.

pH=−log[H3O+][H3O+]=10−pH=10−9.12=7.6×10-10M.pOH=−log[OH−][OH−]=10−pOH=10−4.88=1.3×10-5M.

As the pH of the solution is greater than 7, the solution is basic.

Now, the table can be filled as given below.

Now, the complete table can be given as shown below.

pH	[H3O+]M	[OH−]M	Nature
(a) 6.21	6.1×10-7	1.6×10-8	Acidic
(b) 5.34	4.5×10-6	2.2×10-9	Acidic
(c) 4.67	2.1×10-5	4.7×10-10	Acidic
(d) 1.60	2.5×10-2	4.0×10-13	Acidic
(e) 9.12	7.6×10-10	1.3×10-5	Basic

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Answer 3

Question

Chapter 14, Problem 34QRT

Interpretation Introduction

Interpretation:

The interconversions given below have to be done and in each case whether the solution is acidic or basic has to be estimated.

Concept Introduction:

The relationship between pH and pOH is given below.

pH+pOH=14

Other relations are given below.

pH=−log[H3O+]pOH=−log[OH−]Kw=[H3O+][OH−]=10−14

If the pH of a solution is less than 7, then the solution is acidic. If the pH of a solution is greater than 7, then the solution is basic.

Expert Solution & Answer

Explanation of Solution

(a) [H3O+]=6.1×10-7M

The pH of the solution can be calculated as given below.

pH=−log[H3O+]=−log[6.1×10−7]=6.21.

Then,

pH+pOH=14pOH=14−pH=14−6.21=7.79.[OH−]=10−pOH=10−7.79=1.6×10-8M.

As the pH of the solution is less than 7, the solution is acidic.

(b) [OH−]=2.2×10-9M

The pOH of the solution can be calculated as given below.

pOH=−log[OH−]=−log[2.2×10−9]=8.66.

Then,

pH+pOH=14pH=14−pOH=14−8.66=5.34.[H3O+]=10−pH=10−5.34=4.5×10-6M.

As the pH of the solution is greater than 7, the solution is basic.

(c) pH=4.67

The relationship between pH and pOH is given below.

pH+pOH=14

Therefore,

pH+pOH=14pOH=14−pH=14−4.67=9.33.

The concentration of H3O+ and OH− ion can be calculated as given below.

pH=−log[H3O+][H3O+]=10−pH=10−4.67=2.1×10-5M.pOH=−log[OH−][OH−]=10−pOH=10−9.33=4.7×10-10M.

As the pH of the solution is less than 7, the solution is acidic.

(d) [H3O+]=2.5×10-2M

The pH of the solution can be calculated as given below.

pH=−log[H3O+]=−log[2.5×10−2]=1.60.

Then,

pH+pOH=14pOH=14−pH=14−1.60=12.40.[OH−]=10−pOH=10−12.40=4.0×10-13M.

As the pH of the solution is less than 7, the solution is acidic.

(e) pH=9.12

The relationship between pH and pOH is given below.

pH+pOH=14

Therefore,

pH+pOH=14pOH=14−pH=14−9.12=4.88.

The concentration of H3O+ and OH− ion can be calculated as given below.

pH=−log[H3O+][H3O+]=10−pH=10−9.12=7.6×10-10M.pOH=−log[OH−][OH−]=10−pOH=10−4.88=1.3×10-5M.

As the pH of the solution is greater than 7, the solution is basic.

Now, the table can be filled as given below.

Now, the complete table can be given as shown below.

pH	[H3O+]M	[OH−]M	Nature
(a) 6.21	6.1×10-7	1.6×10-8	Acidic
(b) 5.34	4.5×10-6	2.2×10-9	Acidic
(c) 4.67	2.1×10-5	4.7×10-10	Acidic
(d) 1.60	2.5×10-2	4.0×10-13	Acidic
(e) 9.12	7.6×10-10	1.3×10-5	Basic

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Answer 4

Question

Chapter 14, Problem 34QRT

Interpretation Introduction

Interpretation:

The interconversions given below have to be done and in each case whether the solution is acidic or basic has to be estimated.

Concept Introduction:

The relationship between pH and pOH is given below.

pH+pOH=14

Other relations are given below.

pH=−log[H3O+]pOH=−log[OH−]Kw=[H3O+][OH−]=10−14

If the pH of a solution is less than 7, then the solution is acidic. If the pH of a solution is greater than 7, then the solution is basic.

Expert Solution & Answer

Explanation of Solution

(a) [H3O+]=6.1×10-7M

The pH of the solution can be calculated as given below.

pH=−log[H3O+]=−log[6.1×10−7]=6.21.

Then,

pH+pOH=14pOH=14−pH=14−6.21=7.79.[OH−]=10−pOH=10−7.79=1.6×10-8M.

As the pH of the solution is less than 7, the solution is acidic.

(b) [OH−]=2.2×10-9M

The pOH of the solution can be calculated as given below.

pOH=−log[OH−]=−log[2.2×10−9]=8.66.

Then,

pH+pOH=14pH=14−pOH=14−8.66=5.34.[H3O+]=10−pH=10−5.34=4.5×10-6M.

As the pH of the solution is greater than 7, the solution is basic.

(c) pH=4.67

The relationship between pH and pOH is given below.

pH+pOH=14

Therefore,

pH+pOH=14pOH=14−pH=14−4.67=9.33.

The concentration of H3O+ and OH− ion can be calculated as given below.

pH=−log[H3O+][H3O+]=10−pH=10−4.67=2.1×10-5M.pOH=−log[OH−][OH−]=10−pOH=10−9.33=4.7×10-10M.

As the pH of the solution is less than 7, the solution is acidic.

(d) [H3O+]=2.5×10-2M

The pH of the solution can be calculated as given below.

pH=−log[H3O+]=−log[2.5×10−2]=1.60.

Then,

pH+pOH=14pOH=14−pH=14−1.60=12.40.[OH−]=10−pOH=10−12.40=4.0×10-13M.

As the pH of the solution is less than 7, the solution is acidic.

(e) pH=9.12

The relationship between pH and pOH is given below.

pH+pOH=14

Therefore,

pH+pOH=14pOH=14−pH=14−9.12=4.88.

The concentration of H3O+ and OH− ion can be calculated as given below.

pH=−log[H3O+][H3O+]=10−pH=10−9.12=7.6×10-10M.pOH=−log[OH−][OH−]=10−pOH=10−4.88=1.3×10-5M.

As the pH of the solution is greater than 7, the solution is basic.

Now, the table can be filled as given below.

Now, the complete table can be given as shown below.

pH	[H3O+]M	[OH−]M	Nature
(a) 6.21	6.1×10-7	1.6×10-8	Acidic
(b) 5.34	4.5×10-6	2.2×10-9	Acidic
(c) 4.67	2.1×10-5	4.7×10-10	Acidic
(d) 1.60	2.5×10-2	4.0×10-13	Acidic
(e) 9.12	7.6×10-10	1.3×10-5	Basic

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Answer 5

Chapter 14, Problem 34QRT

Interpretation Introduction

Interpretation:

The interconversions given below have to be done and in each case whether the solution is acidic or basic has to be estimated.

Concept Introduction:

The relationship between pH and pOH is given below.

pH+pOH=14

Other relations are given below.

pH=−log[H3O+]pOH=−log[OH−]Kw=[H3O+][OH−]=10−14

If the pH of a solution is less than 7, then the solution is acidic. If the pH of a solution is greater than 7, then the solution is basic.

Expert Solution & Answer

Explanation of Solution

(a) [H3O+]=6.1×10-7M

The pH of the solution can be calculated as given below.

pH=−log[H3O+]=−log[6.1×10−7]=6.21.

Then,

pH+pOH=14pOH=14−pH=14−6.21=7.79.[OH−]=10−pOH=10−7.79=1.6×10-8M.

As the pH of the solution is less than 7, the solution is acidic.

(b) [OH−]=2.2×10-9M

The pOH of the solution can be calculated as given below.

pOH=−log[OH−]=−log[2.2×10−9]=8.66.

Then,

pH+pOH=14pH=14−pOH=14−8.66=5.34.[H3O+]=10−pH=10−5.34=4.5×10-6M.

As the pH of the solution is greater than 7, the solution is basic.

(c) pH=4.67

The relationship between pH and pOH is given below.

pH+pOH=14

Therefore,

pH+pOH=14pOH=14−pH=14−4.67=9.33.

The concentration of H3O+ and OH− ion can be calculated as given below.

pH=−log[H3O+][H3O+]=10−pH=10−4.67=2.1×10-5M.pOH=−log[OH−][OH−]=10−pOH=10−9.33=4.7×10-10M.

As the pH of the solution is less than 7, the solution is acidic.

(d) [H3O+]=2.5×10-2M

The pH of the solution can be calculated as given below.

pH=−log[H3O+]=−log[2.5×10−2]=1.60.

Then,

pH+pOH=14pOH=14−pH=14−1.60=12.40.[OH−]=10−pOH=10−12.40=4.0×10-13M.

As the pH of the solution is less than 7, the solution is acidic.

(e) pH=9.12

The relationship between pH and pOH is given below.

pH+pOH=14

Therefore,

pH+pOH=14pOH=14−pH=14−9.12=4.88.

The concentration of H3O+ and OH− ion can be calculated as given below.

pH=−log[H3O+][H3O+]=10−pH=10−9.12=7.6×10-10M.pOH=−log[OH−][OH−]=10−pOH=10−4.88=1.3×10-5M.

As the pH of the solution is greater than 7, the solution is basic.

Now, the table can be filled as given below.

Now, the complete table can be given as shown below.

pH	[H3O+]M	[OH−]M	Nature
(a) 6.21	6.1×10-7	1.6×10-8	Acidic
(b) 5.34	4.5×10-6	2.2×10-9	Acidic
(c) 4.67	2.1×10-5	4.7×10-10	Acidic
(d) 1.60	2.5×10-2	4.0×10-13	Acidic
(e) 9.12	7.6×10-10	1.3×10-5	Basic

Answer 6

Chapter 14, Problem 34QRT

Interpretation Introduction

Interpretation:

The interconversions given below have to be done and in each case whether the solution is acidic or basic has to be estimated.

Concept Introduction:

The relationship between pH and pOH is given below.

pH+pOH=14

Other relations are given below.

pH=−log[H3O+]pOH=−log[OH−]Kw=[H3O+][OH−]=10−14

If the pH of a solution is less than 7, then the solution is acidic. If the pH of a solution is greater than 7, then the solution is basic.

Expert Solution & Answer

Explanation of Solution

(a) [H3O+]=6.1×10-7M

The pH of the solution can be calculated as given below.

pH=−log[H3O+]=−log[6.1×10−7]=6.21.

Then,

pH+pOH=14pOH=14−pH=14−6.21=7.79.[OH−]=10−pOH=10−7.79=1.6×10-8M.

As the pH of the solution is less than 7, the solution is acidic.

(b) [OH−]=2.2×10-9M

The pOH of the solution can be calculated as given below.

pOH=−log[OH−]=−log[2.2×10−9]=8.66.

Then,

pH+pOH=14pH=14−pOH=14−8.66=5.34.[H3O+]=10−pH=10−5.34=4.5×10-6M.

As the pH of the solution is greater than 7, the solution is basic.

(c) pH=4.67

The relationship between pH and pOH is given below.

pH+pOH=14

Therefore,

pH+pOH=14pOH=14−pH=14−4.67=9.33.

The concentration of H3O+ and OH− ion can be calculated as given below.

pH=−log[H3O+][H3O+]=10−pH=10−4.67=2.1×10-5M.pOH=−log[OH−][OH−]=10−pOH=10−9.33=4.7×10-10M.

As the pH of the solution is less than 7, the solution is acidic.

(d) [H3O+]=2.5×10-2M

The pH of the solution can be calculated as given below.

pH=−log[H3O+]=−log[2.5×10−2]=1.60.

Then,

pH+pOH=14pOH=14−pH=14−1.60=12.40.[OH−]=10−pOH=10−12.40=4.0×10-13M.

As the pH of the solution is less than 7, the solution is acidic.

(e) pH=9.12

The relationship between pH and pOH is given below.

pH+pOH=14

Therefore,

pH+pOH=14pOH=14−pH=14−9.12=4.88.

The concentration of H3O+ and OH− ion can be calculated as given below.

pH=−log[H3O+][H3O+]=10−pH=10−9.12=7.6×10-10M.pOH=−log[OH−][OH−]=10−pOH=10−4.88=1.3×10-5M.

As the pH of the solution is greater than 7, the solution is basic.

Now, the table can be filled as given below.

Now, the complete table can be given as shown below.

pH	[H3O+]M	[OH−]M	Nature
(a) 6.21	6.1×10-7	1.6×10-8	Acidic
(b) 5.34	4.5×10-6	2.2×10-9	Acidic
(c) 4.67	2.1×10-5	4.7×10-10	Acidic
(d) 1.60	2.5×10-2	4.0×10-13	Acidic
(e) 9.12	7.6×10-10	1.3×10-5	Basic

Answer 7

Chapter 14, Problem 34QRT

Interpretation Introduction

Interpretation:

The interconversions given below have to be done and in each case whether the solution is acidic or basic has to be estimated.

Concept Introduction:

The relationship between pH and pOH is given below.

pH+pOH=14

Other relations are given below.

pH=−log[H3O+]pOH=−log[OH−]Kw=[H3O+][OH−]=10−14

If the pH of a solution is less than 7, then the solution is acidic. If the pH of a solution is greater than 7, then the solution is basic.

Answer 8

Expert Solution & Answer

Explanation of Solution

(a) [H3O+]=6.1×10-7M

The pH of the solution can be calculated as given below.

pH=−log[H3O+]=−log[6.1×10−7]=6.21.

Then,

pH+pOH=14pOH=14−pH=14−6.21=7.79.[OH−]=10−pOH=10−7.79=1.6×10-8M.

As the pH of the solution is less than 7, the solution is acidic.

(b) [OH−]=2.2×10-9M

The pOH of the solution can be calculated as given below.

pOH=−log[OH−]=−log[2.2×10−9]=8.66.

Then,

pH+pOH=14pH=14−pOH=14−8.66=5.34.[H3O+]=10−pH=10−5.34=4.5×10-6M.

As the pH of the solution is greater than 7, the solution is basic.

(c) pH=4.67

The relationship between pH and pOH is given below.

pH+pOH=14

Therefore,

pH+pOH=14pOH=14−pH=14−4.67=9.33.

The concentration of H3O+ and OH− ion can be calculated as given below.

pH=−log[H3O+][H3O+]=10−pH=10−4.67=2.1×10-5M.pOH=−log[OH−][OH−]=10−pOH=10−9.33=4.7×10-10M.

As the pH of the solution is less than 7, the solution is acidic.

(d) [H3O+]=2.5×10-2M

The pH of the solution can be calculated as given below.

pH=−log[H3O+]=−log[2.5×10−2]=1.60.

Then,

pH+pOH=14pOH=14−pH=14−1.60=12.40.[OH−]=10−pOH=10−12.40=4.0×10-13M.

As the pH of the solution is less than 7, the solution is acidic.

(e) pH=9.12

The relationship between pH and pOH is given below.

pH+pOH=14

Therefore,

pH+pOH=14pOH=14−pH=14−9.12=4.88.

The concentration of H3O+ and OH− ion can be calculated as given below.

pH=−log[H3O+][H3O+]=10−pH=10−9.12=7.6×10-10M.pOH=−log[OH−][OH−]=10−pOH=10−4.88=1.3×10-5M.

As the pH of the solution is greater than 7, the solution is basic.

Now, the table can be filled as given below.

Now, the complete table can be given as shown below.

pH	[H3O+]M	[OH−]M	Nature
(a) 6.21	6.1×10-7	1.6×10-8	Acidic
(b) 5.34	4.5×10-6	2.2×10-9	Acidic
(c) 4.67	2.1×10-5	4.7×10-10	Acidic
(d) 1.60	2.5×10-2	4.0×10-13	Acidic
(e) 9.12	7.6×10-10	1.3×10-5	Basic