Chemistry: The Science in Context (Fifth Edition)
Chemistry: The Science in Context (Fifth Edition)
5th Edition
ISBN: 9780393614046
Author: Thomas R. Gilbert, Rein V. Kirss, Natalie Foster, Stacey Lowery Bretz, Geoffrey Davies
Publisher: W. W. Norton & Company
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Chapter 15, Problem 15.33QP

(a)

Interpretation Introduction

Interpretation: The concentration of the given ions in the described solution is to be calculated.

Concept introduction: The measure of concentration of ions in a solution gives the ionic strength of the solution. Concentration of ions in a solution depends on the mole ratio between the cation and anions and the dissolved substance.

To determine: The concentration of the given ions in the described solution.

(a)

Expert Solution
Check Mark

Answer to Problem 15.33QP

Solution

The concentration of H3O+ ions in the solution is 1.190×1011M_ .

Explanation of Solution

Explanation

Given

The concentration of NaOH is 8.4×104M .

The auto-dissociation of pure water is shown by the reaction,

2H2OH3O++OH

Concentrations of [H3O+] and [OH] in the solution are related according to the following relation,

[H3O+]×[OH]=Kw=1014

The value of pH is calculated by using the expression,

pH=log[H3O+]

The dissociation of NaOH in aqueous solution is expressed by the reaction,

NaOH(aq)Na+(aq)+OH(aq)

Sodium hydroxide (NaOH) , is a strong base as it dissociates completely in aqueous solution. Hence, the concentration of OH ion in the solution is exactly same as the concentration of NaOH .

The concentration of OH ion in the solution is 8.4×104M .

The concentration of [H3O+] in the solution is calculated by using the formula,

[H3O+]=Kw[OH]

Substitute the value of [OH] in the above formula to calculate the concentration of H3O+ .

[H3O+]=10148.4×104M=1.190×1011M_

Hence, the concentration of H3O+ is 1.190×1011M_ .

(b)

Interpretation Introduction

To determine: The concentration of the given ions in the described solution.

(b)

Expert Solution
Check Mark

Answer to Problem 15.33QP

Solution

The concentration of H3O+ ions in the solution is 7.6×1011M_ .

Explanation of Solution

Explanation

Given

The concentration of Ca(OH)2 is 6.6×105M .

The dissociation of Ca(OH)2 in aqueous solution is expressed by the reaction,

Ca(OH)2(aq)Ca+(aq)+2OH(aq)

Calcium hydroxide (Ca(OH)2) , is a strong base as it dissociates completely in aqueous solution. Hence, the concentration of OH ion in the solution is exactly double as the concentration of Ca(OH)2 as it gives two OH ions on dissociation.

The concentration of OH ion in the solution is,

[OH]=2×6.6×105M=1.32×104M

The concentration of OH ion in the solution is 1.32×104M .

The concentration of [H3O+] in the solution is calculated by using the formula,

[H3O+]=Kw[OH]

Substitute the value of [OH] in the above formula to calculate the concentration of H3O+ .

[H3O+]=10141.32×104M=7.6×1011M_

Hence, the concentration of H3O+ is 7.6×1011M_ .

(c)

Interpretation Introduction

To determine: The concentration of the given ions in the described solution.

(c)

Expert Solution
Check Mark

Answer to Problem 15.33QP

Solution

The concentration of OH ions in the solution is 2.2×1012M_ .

Explanation of Solution

Explanation

Given

The concentration of HCl is 4.5×103M .

The dissociation of HCl in aqueous solution is expressed by the reaction,

HCl(aq)+H2O(l)H3O+(aq)+Cl(aq)

Hydrochloric acid (HCl) , is a strong acid as it dissociates completely in aqueous solution. Hence, the concentration of H3O+ ion in the solution is exactly same as the concentration of HCl .

The concentration of H3O+ ion in the solution is 4.5×103M .

The concentration of OH ions in the solution is calculated by using the formula,

[OH]=Kw[H3O+]

Substitute the value of [H3O+] in the above formula to calculate the concentration of OH .

[OH]=10144.5×103M=2.2×1012M_

Hence, the concentration of OH is 2.2×1012M_ .

(d)

Interpretation Introduction

To determine: The concentration of the given ions in the described solution.

(d)

Expert Solution
Check Mark

Answer to Problem 15.33QP

Solution

The concentration of OH ions in the solution is 3.4×1010M_ .

Explanation of Solution

Explanation

Given

The concentration of HCl is 2.9×105M .

The dissociation of HCl in aqueous solution is expressed by the reaction,

HCl(aq)+H2O(l)H3O+(aq)+Cl(aq)

Hydrochloric acid (HCl) , is a strong acid as it dissociates completely in aqueous solution. Hence, the concentration of H3O+ ion in the solution is exactly same as the concentration of HCl .

The concentration of H3O+ ion in the solution is 2.9×105M .

The concentration of OH ions in the solution is calculated by using the formula,

[OH]=Kw[H3O+]

Substitute the value of [H3O+] in the above formula to calculate the concentration of OH .

[OH]=10142.9×105M=3.4×1010M_

Hence, the concentration of OH is 3.4×1010M_ .

Conclusion

  1. a. The concentration of H3O+ ions in the solution is 1.190×1011M_ .
  2. b. The concentration of H3O+ ions in the solution is 7.6×1011M_ .
  3. c. The concentration of OH ions in the solution is 2.2×1012M_ .
  4. d. The concentration of OH ions in the solution is 3.4×1010M_

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Chapter 15 Solutions

Chemistry: The Science in Context (Fifth Edition)

Ch. 15.5 - Prob. 11PECh. 15.5 - Prob. 12PECh. 15.6 - Prob. 13PECh. 15.6 - Prob. 14PECh. 15.7 - Prob. 15PECh. 15.8 - Prob. 16PECh. 15.8 - Prob. 17PECh. 15.8 - Prob. 18PECh. 15 - Prob. 15.1VPCh. 15 - Prob. 15.2VPCh. 15 - Prob. 15.3VPCh. 15 - Prob. 15.4VPCh. 15 - Prob. 15.5VPCh. 15 - Prob. 15.6VPCh. 15 - Prob. 15.7VPCh. 15 - Prob. 15.8VPCh. 15 - Prob. 15.9VPCh. 15 - Prob. 15.10VPCh. 15 - Prob. 15.11QPCh. 15 - Prob. 15.12QPCh. 15 - Prob. 15.13QPCh. 15 - Prob. 15.14QPCh. 15 - Prob. 15.15QPCh. 15 - Prob. 15.16QPCh. 15 - Prob. 15.17QPCh. 15 - Prob. 15.18QPCh. 15 - Prob. 15.19QPCh. 15 - Prob. 15.20QPCh. 15 - Prob. 15.21QPCh. 15 - Prob. 15.22QPCh. 15 - Prob. 15.23QPCh. 15 - Prob. 15.24QPCh. 15 - Prob. 15.25QPCh. 15 - Prob. 15.26QPCh. 15 - Prob. 15.27QPCh. 15 - Prob. 15.28QPCh. 15 - Prob. 15.29QPCh. 15 - Prob. 15.30QPCh. 15 - Prob. 15.31QPCh. 15 - Prob. 15.32QPCh. 15 - Prob. 15.33QPCh. 15 - Prob. 15.34QPCh. 15 - Prob. 15.35QPCh. 15 - Prob. 15.36QPCh. 15 - Prob. 15.37QPCh. 15 - Prob. 15.38QPCh. 15 - Prob. 15.39QPCh. 15 - Prob. 15.40QPCh. 15 - Prob. 15.41QPCh. 15 - Prob. 15.42QPCh. 15 - Prob. 15.43QPCh. 15 - Prob. 15.44QPCh. 15 - Prob. 15.45QPCh. 15 - Prob. 15.46QPCh. 15 - Prob. 15.47QPCh. 15 - Prob. 15.48QPCh. 15 - Prob. 15.49QPCh. 15 - Prob. 15.50QPCh. 15 - Prob. 15.51QPCh. 15 - Prob. 15.52QPCh. 15 - Prob. 15.53QPCh. 15 - Prob. 15.54QPCh. 15 - Prob. 15.55QPCh. 15 - Prob. 15.56QPCh. 15 - Prob. 15.57QPCh. 15 - Prob. 15.58QPCh. 15 - Prob. 15.59QPCh. 15 - Prob. 15.60QPCh. 15 - Prob. 15.61QPCh. 15 - Prob. 15.62QPCh. 15 - Prob. 15.63QPCh. 15 - Prob. 15.64QPCh. 15 - Prob. 15.65QPCh. 15 - Prob. 15.66QPCh. 15 - Prob. 15.67QPCh. 15 - Prob. 15.68QPCh. 15 - Prob. 15.69QPCh. 15 - Prob. 15.70QPCh. 15 - Prob. 15.71QPCh. 15 - Prob. 15.72QPCh. 15 - Prob. 15.73QPCh. 15 - Prob. 15.74QPCh. 15 - Prob. 15.75QPCh. 15 - Prob. 15.76QPCh. 15 - Prob. 15.77QPCh. 15 - Prob. 15.78QPCh. 15 - Prob. 15.79QPCh. 15 - Prob. 15.80QPCh. 15 - Prob. 15.81QPCh. 15 - Prob. 15.82QPCh. 15 - Prob. 15.83QPCh. 15 - Prob. 15.84QPCh. 15 - Prob. 15.85QPCh. 15 - Prob. 15.86QPCh. 15 - Prob. 15.87APCh. 15 - Prob. 15.88APCh. 15 - Prob. 15.89APCh. 15 - Prob. 15.90APCh. 15 - Prob. 15.91APCh. 15 - Prob. 15.92APCh. 15 - Prob. 15.93APCh. 15 - Prob. 15.94APCh. 15 - Prob. 15.95APCh. 15 - Prob. 15.96APCh. 15 - Prob. 15.97APCh. 15 - Prob. 15.98APCh. 15 - Prob. 15.99APCh. 15 - Prob. 15.100AP
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