Principles of Chemistry: A Molecular Approach (3rd Edition)
Principles of Chemistry: A Molecular Approach (3rd Edition)
3rd Edition
ISBN: 9780321971944
Author: Nivaldo J. Tro
Publisher: PEARSON
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Chapter 16, Problem 16.1P
Interpretation Introduction

Interpretation: The pHof a buffer that is 0.200Min HC2H3O2and 0.100Min NaC2H3O2is to be calculated.

Concept introduction: An aqueous solution of mixture of a weak acid and its conjugate base or mixture of weak base with its conjugate acid is known as the buffer solution. It resists in the change of the pHof a solution by neutralizing added amount of acid or base.

The acid in a buffer solution neutralizes the added base and the base present in buffer solution neutralizes the added acid.

To determine: The pHof a buffer that is 0.200Min HC2H3O2and 0.100Min NaC2H3O2 .

Expert Solution & Answer
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Answer to Problem 16.1P

Solution:

The pHof a buffer that is 0.200Min HC2H3O2and 0.100Min NaC2H3O2is 4.44 .

Explanation of Solution

Given information: The concentration of HC2H3O2is 0.200M .

The concentration of NaC2H3O2is 0.100M .

The balanced equation for the ionization of acid HC2H3O2in aqueous solution is,

HC2H3O2(aq)+H2O(l)H3O+(aq)+C2H3O2(aq)

The concentration of HC2H3O2is 0.200M .

The concentration of NaC2H3O2or C2H3O2is 0.100M .

The concentration of H3O+is supposed to be x .

Thus, the concentration of HC2H3O2after removal of H3O+ions is 0.200Mx .

The changed concentration of C2H3O2after the addition of H3O+ is 0.100M+x .

The acid ionization constant is expressed as,

Ka=[C][D][A][B]

Where,

  • [A]and [B] are concentrations of reactants.
  • [C]and [D] are concentrations of products.
  • Ka is the acid ionization constant.
  • The standard value of Kafor acetic acid is 1.8×105 .

Thus, for the given equation the acid ionization constant is expressed as,

Ka=[H3O+][C2H3O2][HC2H3O2]

Substitute the respective values of concentrations and Kain the above equation as,

1.8×105=[x][0.100M+x][0.200Mx]

In the above expression, the value of xis very small. Thus, the value of xcan be neglected from the above equation then the equation becomes as,

1.8×105=[x][0.100M][0.200M]x=(1.8× 10 50.5)x=3.6×105

Therefore, the concentration of H3O+is, x=3.6×105 .

The pHof the buffer is calculated by the expression.

pH=log[H3O+]

Substitute the value of H3O+in the above expression as,

pH=log[3.6×105]=4.44

Hence, the pHof a buffer that is 0.200Min HC2H3O2and 0.100Min NaC2H3O2is 4.44 .

Conclusion

The pHof a buffer that is 0.200Min HC2H3O2and 0.100Min NaC2H3O2is 4.44 .

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Chapter 16 Solutions

Principles of Chemistry: A Molecular Approach (3rd Edition)

Ch. 16 - For Practice 16.8 Calculate the molar solubility...Ch. 16 - Prob. 16.9PCh. 16 - Prob. 16.10PCh. 16 - For Practice 16.11 Which compound, FeCO3 or...Ch. 16 - Prob. 16.12PCh. 16 - For Practice 16.13 A 125.0-mL sample of solution...Ch. 16 - Prob. 1SAQCh. 16 - Prob. 2SAQCh. 16 - Prob. 3SAQCh. 16 - Prob. 4SAQCh. 16 - Prob. 5SAQCh. 16 - Prob. 6SAQCh. 16 - Prob. 7SAQCh. 16 - Prob. 8SAQCh. 16 - Prob. 9SAQCh. 16 - Prob. 10SAQCh. 16 - Prob. 11SAQCh. 16 - Prob. 12SAQCh. 16 - Prob. 13SAQCh. 16 - Prob. 14SAQCh. 16 - Prob. 15SAQCh. 16 - Prob. 1ECh. 16 - Prob. 2ECh. 16 - Prob. 3ECh. 16 - Prob. 4ECh. 16 - 5. Calculate the percent ionization of a 0.15 M...Ch. 16 - 6. Calculate the percent ionization of a 0.13 M...Ch. 16 - Prob. 7ECh. 16 - Prob. 8ECh. 16 - Prob. 9ECh. 16 - Prob. 10ECh. 16 - Prob. 11ECh. 16 - Prob. 12ECh. 16 - Prob. 13ECh. 16 - Prob. 14ECh. 16 - Prob. 15ECh. 16 - Prob. 16ECh. 16 - Prob. 17ECh. 16 - Prob. 18ECh. 16 - Prob. 19ECh. 16 - Prob. 20ECh. 16 - Prob. 21ECh. 16 - 22. A 100.0-mL buffer solution is 0.175 M in HClO...Ch. 16 - Prob. 23ECh. 16 - Prob. 24ECh. 16 - Prob. 25ECh. 16 - Prob. 26ECh. 16 - Prob. 27ECh. 16 - Prob. 28ECh. 16 - Prob. 29ECh. 16 - Prob. 30ECh. 16 - Prob. 31ECh. 16 - Which buffer system is the best choice to create a...Ch. 16 - Prob. 33ECh. 16 - Prob. 34ECh. 16 - Prob. 35ECh. 16 - Prob. 36ECh. 16 - Prob. 37ECh. 16 - Prob. 38ECh. 16 - Prob. 39ECh. 16 - Prob. 40ECh. 16 - Prob. 41ECh. 16 - A 20.0-mL sample of 0.125 M HNO3 titrated with...Ch. 16 - Prob. 43ECh. 16 - Prob. 44ECh. 16 - Prob. 45ECh. 16 - Prob. 46ECh. 16 - Prob. 47ECh. 16 - Prob. 48ECh. 16 - Prob. 49ECh. 16 - Prob. 50ECh. 16 - Prob. 51ECh. 16 - Prob. 52ECh. 16 - Prob. 53ECh. 16 - Prob. 54ECh. 16 - Prob. 55ECh. 16 - Prob. 56ECh. 16 - Prob. 57ECh. 16 - Prob. 58ECh. 16 - Prob. 59ECh. 16 - Prob. 60ECh. 16 - Prob. 61ECh. 16 - Prob. 62ECh. 16 - Prob. 63ECh. 16 - Prob. 64ECh. 16 - Use the Kspvalue from Table 16.2 to calculate the...Ch. 16 - Prob. 66ECh. 16 - Prob. 67ECh. 16 - Calculate the molar solubility of MX (Ksp= 1.27 ...Ch. 16 - Prob. 69ECh. 16 - Calculate the solubility (in grams per 1.00102mL...Ch. 16 - Prob. 71ECh. 16 - Determine if each compound is more soluble in...Ch. 16 - Prob. 73ECh. 16 - Prob. 74ECh. 16 - Prob. 75ECh. 16 - 76. Predict whether or not a precipitate forms...Ch. 16 - Prob. 77ECh. 16 - Prob. 78ECh. 16 - Prob. 79ECh. 16 - Prob. 80ECh. 16 - Prob. 81ECh. 16 - Prob. 82ECh. 16 - Prob. 83ECh. 16 - Prob. 84ECh. 16 - Prob. 85ECh. 16 - Prob. 86ECh. 16 - Prob. 87ECh. 16 - Prob. 88ECh. 16 - Prob. 89ECh. 16 - Prob. 90ECh. 16 - Prob. 91ECh. 16 - Prob. 92ECh. 16 - One of the main components of hard water is CaCO3....Ch. 16 - Prob. 94ECh. 16 - Prob. 95ECh. 16 - Calculate the solubility of silver chloride ii a...Ch. 16 - Prob. 97ECh. 16 - Prob. 98ECh. 16 - Prob. 99ECh. 16 - Prob. 100ECh. 16 - What relative masses of demethyl amine and...Ch. 16 - Prob. 102ECh. 16 - Prob. 103ECh. 16 - Prob. 104ECh. 16 - Since soap and detergent action is hindered by...Ch. 16 - Prob. 106ECh. 16 - Prob. 107ECh. 16 - Determine the solubility of Cul in 0.40 M HCN...Ch. 16 - Prob. 109ECh. 16 - Prob. 110ECh. 16 - Prob. 111ECh. 16 - Prob. 112ECh. 16 - Prob. 113ECh. 16 - Prob. 114ECh. 16 - Prob. 115ECh. 16 - Prob. 116E
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