تكلم مع الذكاء الاصطناعي
Deck 17: Additional Aspects of Aqueous Equilibria
ملء الشاشة (f)
سؤال
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The Henderson-Hasselbalch equation is ________.
A)[H+] = Ka +![<strong>The Henderson-Hasselbalch equation is ________.</strong> A)[H<sup>+</sup>] = K<sub>a</sub> + B)pH = pK<sub>a</sub> - log C)pH = pK<sub>a</sub> + log D)pH = pK<sub>a</sub> + log E)pH = log <div style=padding-top: 35px>](https://d2lvgg3v3hfg70.cloudfront.net/TB1194/11ea7e7c_6162_c997_9a0a_8fa4c2398b13_TB1194_11.jpg)
B)pH = pKa - log![<strong>The Henderson-Hasselbalch equation is ________.</strong> A)[H<sup>+</sup>] = K<sub>a</sub> + B)pH = pK<sub>a</sub> - log C)pH = pK<sub>a</sub> + log D)pH = pK<sub>a</sub> + log E)pH = log <div style=padding-top: 35px>](https://d2lvgg3v3hfg70.cloudfront.net/TB1194/11ea7e7c_6162_c998_9a0a_1b43014d9f2e_TB1194_11.jpg)
C)pH = pKa + log![<strong>The Henderson-Hasselbalch equation is ________.</strong> A)[H<sup>+</sup>] = K<sub>a</sub> + B)pH = pK<sub>a</sub> - log C)pH = pK<sub>a</sub> + log D)pH = pK<sub>a</sub> + log E)pH = log <div style=padding-top: 35px>](https://d2lvgg3v3hfg70.cloudfront.net/TB1194/11ea7e7c_6162_c999_9a0a_7973f922a195_TB1194_11.jpg)
D)pH = pKa + log![<strong>The Henderson-Hasselbalch equation is ________.</strong> A)[H<sup>+</sup>] = K<sub>a</sub> + B)pH = pK<sub>a</sub> - log C)pH = pK<sub>a</sub> + log D)pH = pK<sub>a</sub> + log E)pH = log <div style=padding-top: 35px>](https://d2lvgg3v3hfg70.cloudfront.net/TB1194/11ea7e7c_6162_f0aa_9a0a_4d2381041ab6_TB1194_11.jpg)
E)pH = log![<strong>The Henderson-Hasselbalch equation is ________.</strong> A)[H<sup>+</sup>] = K<sub>a</sub> + B)pH = pK<sub>a</sub> - log C)pH = pK<sub>a</sub> + log D)pH = pK<sub>a</sub> + log E)pH = log <div style=padding-top: 35px>](https://d2lvgg3v3hfg70.cloudfront.net/TB1194/11ea7e7c_6162_f0ab_9a0a_e1acd2d4bb9e_TB1194_11.jpg)
A)[H+] = Ka +
B)pH = pKa - log
C)pH = pKa + log
D)pH = pKa + log
E)pH = log
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The pH of a solution prepared by dissolving 0.550 mol of solid methylamine hydrochloride (CH3NH3Cl)in 
of 
methylamine (CH3NH2)is ________.The Kb for methylamine is 
(Assume the final volume is 1.00 L.)
A)11.03
B)2.97
C)3.75
D)10.64
E)10.25
of methylamine (CH3NH2)is ________.The Kb for methylamine is (Assume the final volume is 1.00 L.)A)11.03
B)2.97
C)3.75
D)10.64
E)10.25
سؤال
A 25.0 mL sample of 0.723 M HClO4 is titrated with a 
KOH solution.The H3O+ concentration after the addition of 
of KOH is ________ M.
A)0.4
B)1 × 10-7
C)0.7
D)3 × 10-13
E)4 × 10-2
KOH solution.The H3O+ concentration after the addition of of KOH is ________ M.A)0.4
B)1 × 10-7
C)0.7
D)3 × 10-13
E)4 × 10-2
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The Ka of benzoic acid is 6.30 × 10-5.The pH of a buffer prepared by combining 50.0 mL of 
potassium benzoate and 50.0 mL of 1.00 M benzoic acid is ________.
A)1.705
B)0.851
C)3.406
D)4.201
E)2.383
potassium benzoate and 50.0 mL of 1.00 M benzoic acid is ________.A)1.705
B)0.851
C)3.406
D)4.201
E)2.383
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Calculate the pH of a solution prepared by dissolving 
of benzoic acid and 
of sodium benzoate in water sufficient to yield 
of solution.The Ka of benzoic acid is 
A)2.516
B)3.892
C)4.502
D)10.158
E)4.195
of benzoic acid and of sodium benzoate in water sufficient to yield of solution.The Ka of benzoic acid is A)2.516
B)3.892
C)4.502
D)10.158
E)4.195
سؤال
Calculate the pH of a solution prepared by dissolving 
of acetic acid and 
of sodium acetate in water sufficient to yield 
of solution.The Ka of acetic acid is 
A)2.516
B)3.892
C)4.502
D)10.158
E)5.056
of acetic acid and of sodium acetate in water sufficient to yield of solution.The Ka of acetic acid is A)2.516
B)3.892
C)4.502
D)10.158
E)5.056
سؤال
The pH of a solution prepared by dissolving 0.350 mol of acid in 
of 
of conjugate base is ________.The Kb for the conjugate base is 
(Assume the final volume is 1.00 L.)
A)11.23
B)1.66
C)11.14
D)2.77
E)none of the above
of of conjugate base is ________.The Kb for the conjugate base is (Assume the final volume is 1.00 L.)A)11.23
B)1.66
C)11.14
D)2.77
E)none of the above
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The solubility of lead (II)chloride (PbCl2)is 
What is the Ksp of PbCl2?
A)5.0 × 10-4
B)4.1 × 10-6
C)3.1 × 10-7
D)1.6 × 10-5
E)1.6 × 10-2
What is the Ksp of PbCl2?A)5.0 × 10-4
B)4.1 × 10-6
C)3.1 × 10-7
D)1.6 × 10-5
E)1.6 × 10-2
سؤال
What is the solubility (in M)of PbCl2 in a 
solution of HCl? The Ksp of PbCl2 is 
A)2.0 × 10-3
B)1.1 × 10-4
C)1.8 × 10-4
D)7.1 × 10-4
E)1.6 × 10-5
solution of HCl? The Ksp of PbCl2 is A)2.0 × 10-3
B)1.1 × 10-4
C)1.8 × 10-4
D)7.1 × 10-4
E)1.6 × 10-5
سؤال
The concentration of iodide ions in a saturated solution of silver iodide is ________ M.The solubility product constant of AgI is 
A)3.8 × 10-11
B)3.0 × 10-10
C)9.1 × 10-9
D)3.5 × 10-9
E)1.4 × 10-8
A)3.8 × 10-11
B)3.0 × 10-10
C)9.1 × 10-9
D)3.5 × 10-9
E)1.4 × 10-8
سؤال
Calculate the pH of a solution that is 0.278 M in sodium formate ( 
)and 
in formic acid 
The 
of formic acid is 1.77 × 
.
A)3.843
B)3.647
C)13.90
D)10.16
E)4.954
)and in formic acid The of formic acid is 1.77 × .A)3.843
B)3.647
C)13.90
D)10.16
E)4.954
سؤال
The concentration of iodide ions in a saturated solution of lead (II)iodide is ________ M.The solubility product constant of PbI2 is 
A)3.8 × 10-4
B)3.0 × 10-3
C)1.5 × 10-3
D)3.5 × 10-9
E)1.4 × 10-8
A)3.8 × 10-4
B)3.0 × 10-3
C)1.5 × 10-3
D)3.5 × 10-9
E)1.4 × 10-8
سؤال
Calculate the percent ionization of formic acid ( 
H)in a solution that is 0.322 M in formic acid and 0.178 M in sodium formate ( 
).The 
of formic acid is 1.77 × 
.
A)35.6
B)0.1011
C)10.8
D)1.03 × 10-3
E)3.488
H)in a solution that is 0.322 M in formic acid and 0.178 M in sodium formate ( ).The of formic acid is 1.77 × .A)35.6
B)0.1011
C)10.8
D)1.03 × 10-3
E)3.488
سؤال
Calculate the maximum concentration (in M)of silver ions (Ag+)in a solution that contains 
of CO32-.The Ksp of Ag2CO3 is 
A)1.8 × 10-5
B)1.4 × 10-6
C)2.8 × 10-6
D)3.2 × 10-10
E)8.1 × 10-12
of CO32-.The Ksp of Ag2CO3 is A)1.8 × 10-5
B)1.4 × 10-6
C)2.8 × 10-6
D)3.2 × 10-10
E)8.1 × 10-12
سؤال
What is the percent ionization of nitrous acid in a solution that is 0.222 M in nitrous acid (HNO2)and 0.278 M in potassium nitrite (KNO2)? The acid dissociation constant of nitrous acid is 
A)55.6
B)15.5
C)2.78 ×
D)3.448
E)0.162
A)55.6
B)15.5
C)2.78 ×
D)3.448
E)0.162
سؤال
A 50.0 mL sample of an aqueous H2SO4 solution is titrated with a 
NaOH solution.The equivalence point is reached with 
of the base.The concentration of H2SO4 is ________ M.
A)0.234
B)0.469
C)0.150
D)0.300
E)0.938
NaOH solution.The equivalence point is reached with of the base.The concentration of H2SO4 is ________ M.A)0.234
B)0.469
C)0.150
D)0.300
E)0.938
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The concentration of fluoride ions in a saturated solution of barium fluoride is ________ M.The solubility product constant of BaF2 is 
A)3.8 × 10-4
B)3.0 × 10-3
C)1.5 × 10-2
D)7.5 × 10-3
E)1.4 × 10-4
A)3.8 × 10-4
B)3.0 × 10-3
C)1.5 × 10-2
D)7.5 × 10-3
E)1.4 × 10-4
سؤال
What is the percent ionization of nitrous acid in a solution that is 0.189 M in nitrous acid? The acid dissociation constant of nitrous acid is 
A)0.0450
B)8.51 × 10-5
C)0.594
D)4.20
E)4.88
A)0.0450
B)8.51 × 10-5
C)0.594
D)4.20
E)4.88
سؤال
Calculate the percent ionization of formic acid ( 
H)in a solution that is 0.152 M in formic acid.The 
of formic acid is 1.77 × 
.
A)2.74 ×
B)0.0180
C)3.44
D)0.581
E)8.44
H)in a solution that is 0.152 M in formic acid.The of formic acid is 1.77 × .A)2.74 ×
B)0.0180
C)3.44
D)0.581
E)8.44
سؤال
The solubility of manganese (II)hydroxide (Mn(OH)2)is 
What is the Ksp of Mn(OH)2?
A)1.1 × 10-14
B)4.3 × 10-14
C)2.1 × 10-14
D)4.8 × 10-10
E)2.2 × 10-5
What is the Ksp of Mn(OH)2?A)1.1 × 10-14
B)4.3 × 10-14
C)2.1 × 10-14
D)4.8 × 10-10
E)2.2 × 10-5
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Determine the Ksp for magnesium hydroxide (Mg(OH)2)where the solubility of Mg(OH)2 is 
.
A)2.7 × 10-12
B)1.1 × 10-11
C)2.0 × 10-8
D)3.9 × 10-8
E)1.4 × 10-4
.A)2.7 × 10-12
B)1.1 × 10-11
C)2.0 × 10-8
D)3.9 × 10-8
E)1.4 × 10-4
سؤال
Calculate the pH of a solution that is 0.322 M in nitrous acid ( 
)and 0.178 M in potassium nitrite (KNO2).The acid dissociation constant of nitrous acid is 4.50 × 
.
A)3.093
B)3.607
C)14.26
D)10.91
E)4.589
)and 0.178 M in potassium nitrite (KNO2).The acid dissociation constant of nitrous acid is 4.50 × .A)3.093
B)3.607
C)14.26
D)10.91
E)4.589
سؤال
Calculate the maximum concentration (in M)of calcium ions (Ca2+)in a solution that contains 
of CO32-.The Ksp of CaCO3 is 
A)5.8 × 10-5
B)6.8 × 10-9
C)3.4 × 10-9
D)6.2 × 10-8
E)1.9 × 10-10
of CO32-.The Ksp of CaCO3 is A)5.8 × 10-5
B)6.8 × 10-9
C)3.4 × 10-9
D)6.2 × 10-8
E)1.9 × 10-10
سؤال
What is the pH of a buffer solution that is 0.266 M in lactic acid and 0.111 M in sodium lactate? The 
of lactic acid is 1.4 × 
.
A)14.38
B)10.53
C)5.38
D)3.47
E)4.23
of lactic acid is 1.4 × .A)14.38
B)10.53
C)5.38
D)3.47
E)4.23
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The 
of some weak acid HA is 1.76 × 
.The pH of a buffer prepared by combining 15.0 mL of 
A- and 50.0 mL of 1.00 M HA is ________.
A)1.705
B)4.232
C)0.851
D)2.383
E)3.406
of some weak acid HA is 1.76 × .The pH of a buffer prepared by combining 15.0 mL of A- and 50.0 mL of 1.00 M HA is ________.A)1.705
B)4.232
C)0.851
D)2.383
E)3.406
سؤال
A solution is prepared by dissolving 0.23 mol of hypochlorous acid and 0.27 mol of sodium hypochlorite in water sufficient to yield 1.00 L of solution.The addition of 0.05 mol of HCl to this buffer solution causes the pH to drop slightly.The pH does not decrease drastically because the HCl reacts with the ________ present in the buffer solution.The 
of hypochlorous acid is 1.36 × 10-3.
A)
O
B)
C)hypochlorite ion
D)hypochlorous acid
E)This is a buffer solution: the pH does not change upon addition of acid or base.
of hypochlorous acid is 1.36 × 10-3.A)
OB)
C)hypochlorite ion
D)hypochlorous acid
E)This is a buffer solution: the pH does not change upon addition of acid or base.
سؤال
The 
of ammonia is 1.76 × 
.What is the pH of a buffer which is prepared by combining 50.0 mL of 1.00 M ammonia and 45.0 mL of 1.00 M ammonium nitrate?
A)9.372
B)4.632
C)4.742
D)9.291
E)none of the above
of ammonia is 1.76 × .What is the pH of a buffer which is prepared by combining 50.0 mL of 1.00 M ammonia and 45.0 mL of 1.00 M ammonium nitrate?A)9.372
B)4.632
C)4.742
D)9.291
E)none of the above
سؤال
A buffer solution with a pH of 4.31 is prepared with 
and 
The Ka of H 
is 
A)0.37
B)0.74
C)4.2 × 10-6
D)8.8 × 10-10
E)0.18
and The Ka of H is A)0.37
B)0.74
C)4.2 × 10-6
D)8.8 × 10-10
E)0.18
سؤال
0.78 M Na 
and 
are required to prepare a buffer solution with a pH of 4.40 .The 
of H 
is 
A)3.5
B)4.1 × 104
C)1.7
D)0.86
E)0.35
and are required to prepare a buffer solution with a pH of 4.40 .The of H is A)3.5
B)4.1 × 104
C)1.7
D)0.86
E)0.35
سؤال
What is the pH of a solution which is prepared by dissolving 0.850 mol of N 
and 
of 
in water sufficient to yield 1.00 L of solution? The 
of ammonia is 
A)9.700
B)5.204
C)8.781
D)8.796
E)4.300
and of in water sufficient to yield 1.00 L of solution? The of ammonia is A)9.700
B)5.204
C)8.781
D)8.796
E)4.300
سؤال
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Calculate the pH of a solution prepared by dissolving 0.270 mol of weak acid HA and 0.260 mol of its conjugate base in water sufficient to yield 1.00 L of solution.The 
of HA is 
A)2.099
B)3.736
C)10.264
D)3.952
E)2.307
of HA is A)2.099
B)3.736
C)10.264
D)3.952
E)2.307
سؤال
acid and 
formate are required to prepare a buffer solution with a pH of 4.78 .The 
of formic acid is 
A)0.17
B)0.083
C)3.3 × 103
D)0.041
E)9.8
سؤال
A 25.0 mL sample of 0.150 M acetic acid is titrated with a 0.150 M NaOH solution.What is the pH at the equivalence point? The 
of acetic acid is 4.50 × 10-4.
A)11.74
B)9.26
C)4.74
D)7.00
E)8.81
of acetic acid is 4.50 × 10-4.A)11.74
B)9.26
C)4.74
D)7.00
E)8.81
سؤال
What is the pH of a solution that contains 0.800 M weak acid ( 
= 1.76 × 
)and 0.172 M of its conjugate base?
A)8.578
B)5.422
C)8.370
D)4.087
E)9.913
= 1.76 × )and 0.172 M of its conjugate base?A)8.578
B)5.422
C)8.370
D)4.087
E)9.913
سؤال
How many milliliters of 0.0839 M NaOH are required to titrate 25.0 mL of 
to the equivalence point?
A)29.5
B)0.332
C)4.57
D)0.208
E)21.2
to the equivalence point?A)29.5
B)0.332
C)4.57
D)0.208
E)21.2
سؤال
The addition of hydrofluoric acid and ________ to water produces a buffer solution.
A)NaF
B)HF
C)NaN
D)NaBr
E)KI
A)NaF
B)HF
C)NaN
D)NaBr
E)KI
سؤال
A solution is prepared by dissolving 0.23 mol of benzoic acid and 0.27 mol of sodium benzoate in water sufficient to yield 1.00 L of solution.The addition of 0.05 mol of NaOH to this buffer solution causes the pH to increase slightly.The pH does not increase drastically because the NaOH reacts with the ________ present in the buffer solution.The 
of benzoic acid is 6.3 × 10-5.
A)
O
B)
C)benzoate
D)benzoic acid
E)This is a buffer solution: the pH does not change upon addition of acid or base.
of benzoic acid is 6.3 × 10-5.A)
OB)
C)benzoate
D)benzoic acid
E)This is a buffer solution: the pH does not change upon addition of acid or base.
سؤال
What is the pH of a buffer solution that is 0.172 M in hypochlorous acid (HClO)and 0.131 M in sodium hypochlorite? The 
of hypochlorous acid is 3.8 × 
.
A)14.12
B)6.70
C)9.07
D)7.54
E)7.30
of hypochlorous acid is 3.8 × .A)14.12
B)6.70
C)9.07
D)7.54
E)7.30
سؤال
Calculate the pH of a solution prepared by dissolving 0.250 mol of benzoic acid ( 
H)and 
of sodium benzoate (Na 
)in water sufficient to yield 1.00 L of solution.The 
of benzoic acid is 
A)4.409
B)3.965
C)10.035
D)9.591
E)5.190
H)and of sodium benzoate (Na )in water sufficient to yield 1.00 L of solution.The of benzoic acid is A)4.409
B)3.965
C)10.035
D)9.591
E)5.190
سؤال
A buffer solution with a pH of 4.63 is prepared with 
acid and 
formate. The 
of formic acid is 
A)1.1
B)2.1
C)5.4 × 10-6
D)3.0 × 10-8
E)0.54
acid and formate. The of formic acid is A)1.1
B)2.1
C)5.4 × 10-6
D)3.0 × 10-8
E)0.54
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العب
ملء الشاشة (f)
Deck 17: Additional Aspects of Aqueous Equilibria
1
Which of the following could be added to a solution of NaF to prepare a buffer?
A)HBr
B)NaOH
C)LiC2H3O2
D)KF
E)NH3
A)HBr
B)NaOH
C)LiC2H3O2
D)KF
E)NH3
HBr
2
Which of the following could be added to a solution of sodium acetate to produce a buffer?
A)acetic acid only
B)acetic acid or hydrochloric acid
C)hydrochloric acid only
D)potassium acetate only
E)sodium chloride or potassium acetate
A)acetic acid only
B)acetic acid or hydrochloric acid
C)hydrochloric acid only
D)potassium acetate only
E)sodium chloride or potassium acetate
acetic acid or hydrochloric acid
3
Which of the following could be added to a solution of HC2H3O2 to prepare a buffer?
A)HBr
B)HNO3
C)KOH
D)more HC2H3O2
E)None of the above can be added to an acetic acid solution to prepare a buffer.
A)HBr
B)HNO3
C)KOH
D)more HC2H3O2
E)None of the above can be added to an acetic acid solution to prepare a buffer.
KOH
4
The Henderson-Hasselbalch equation is ________.
A)[H+] = Ka +
B)pH = pKa - log
C)pH = pKa + log
D)pH = pKa + log
E)pH = log
A)[H+] = Ka +
B)pH = pKa - log
C)pH = pKa + log
D)pH = pKa + log
E)pH = log
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5
The addition of HCl and ________ to water produces a buffer solution.
A)HC6H5O
B)C2H5NH2
C)KOH
D)KCl
E)none of the above
A)HC6H5O
B)C2H5NH2
C)KOH
D)KCl
E)none of the above
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6
Which one of the following pairs cannot be mixed together to form a buffer solution?
A)C5H5N, C5H5NHCl
B)HC2H3O2, NaOH (C2H3O2- = acetate)
C)KOH, HI
D)NH2CH3, HCl
E)NaClO, HNO3
A)C5H5N, C5H5NHCl
B)HC2H3O2, NaOH (C2H3O2- = acetate)
C)KOH, HI
D)NH2CH3, HCl
E)NaClO, HNO3
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7
A solution containing which one of the following pairs of substances will be a buffer solution?
A)KI, HI
B)AgBr, HBr
C)CuCl, HCl
D)CsI, HI
E)none of the above
A)KI, HI
B)AgBr, HBr
C)CuCl, HCl
D)CsI, HI
E)none of the above
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8
Which one of the following pairs cannot be mixed together to form a buffer solution?
A)HONH2, HONH3Cl
B)NaCl, HCl
C)RbOH, HF
D)KOH, HNO2
E)H2SO3, KHSO3
A)HONH2, HONH3Cl
B)NaCl, HCl
C)RbOH, HF
D)KOH, HNO2
E)H2SO3, KHSO3
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9
Which solution has the greatest buffering capacity?
A)0.335M HC2H3O2 and 0.497 M NaC2H3O2
B)0.520 M HC2H3O2 and 0.116 M NaC2H3O2
C)0.820 M HC2H3O2 and 0.715 M NaC2H3O2
D)0.120 M HC2H3O2 and 0.115 M NaC2H3O2
A)0.335M HC2H3O2 and 0.497 M NaC2H3O2
B)0.520 M HC2H3O2 and 0.116 M NaC2H3O2
C)0.820 M HC2H3O2 and 0.715 M NaC2H3O2
D)0.120 M HC2H3O2 and 0.115 M NaC2H3O2
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10
What is the primary buffer system that controls the pH of the blood?
A)carbonate, bicarbonate
B)carbon dioxide, carbonate
C)carbonic acid, bicarbonate
D)carbonic acid, carbon dioxide
E)carbonate, carbonic acid
A)carbonate, bicarbonate
B)carbon dioxide, carbonate
C)carbonic acid, bicarbonate
D)carbonic acid, carbon dioxide
E)carbonate, carbonic acid
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11
In a solution,when the concentrations of a weak acid and its conjugate base are equal,________.
A)the system is not at equilibrium
B)the buffering capacity is significantly decreased
C)the -log of the [H+] and the -log of the Ka are equal
D)All of the above are true.
A)the system is not at equilibrium
B)the buffering capacity is significantly decreased
C)the -log of the [H+] and the -log of the Ka are equal
D)All of the above are true.
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12
The addition of HCl and ________ to water produces a buffer solution.
A)NH3
B)HC6H5O
C)KOH
D)KNO3
E)HNO3
A)NH3
B)HC6H5O
C)KOH
D)KNO3
E)HNO3
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13
Which solution has the greatest buffering capacity?
A)0.335 M NH3 and 0.100 M NH4Cl
B)0.085 M NH3 and 0.090 M NH4Cl
C)0.540 M NH3 and 0.550 M NH4Cl
D)0.200 M NH3 and 0.565 M NH4Cl
E)They are all buffer solutions and would all have the same capacity.
A)0.335 M NH3 and 0.100 M NH4Cl
B)0.085 M NH3 and 0.090 M NH4Cl
C)0.540 M NH3 and 0.550 M NH4Cl
D)0.200 M NH3 and 0.565 M NH4Cl
E)They are all buffer solutions and would all have the same capacity.
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14
Which of the following could be added to a solution of acetic acid to prepare a buffer?
A)sodium acetate only
B)sodium acetate or sodium hydroxide
C)nitric acid only
D)hydrofluoric acid or nitric acid
E)sodium hydroxide only
A)sodium acetate only
B)sodium acetate or sodium hydroxide
C)nitric acid only
D)hydrofluoric acid or nitric acid
E)sodium hydroxide only
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15
What change will be caused by addition of a small amount of HCl to a solution containing fluoride ions and hydrogen fluoride?
A)The concentration of hydronium ions will increase significantly.
B)The concentration of fluoride ions will increase as will the concentration of hydronium ions.
C)The concentration of hydrogen fluoride will decrease and the concentration of fluoride ions will increase.
D)The concentration of fluoride ion will decrease and the concentration of hydrogen fluoride will increase.
E)The fluoride ions will precipitate out of solution as its acid salt.
A)The concentration of hydronium ions will increase significantly.
B)The concentration of fluoride ions will increase as will the concentration of hydronium ions.
C)The concentration of hydrogen fluoride will decrease and the concentration of fluoride ions will increase.
D)The concentration of fluoride ion will decrease and the concentration of hydrogen fluoride will increase.
E)The fluoride ions will precipitate out of solution as its acid salt.
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16
The addition of HF and ________ to water produces a buffer solution.
A)HBr
B)KNO3
C)KOH
D)NaCl
E)NaBr
A)HBr
B)KNO3
C)KOH
D)NaCl
E)NaBr
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17
The ________ and ________ are the principal organs that regulate the pH of the carbonic acid-bicarbonate buffer system in the blood.
A)kidneys, liver
B)lungs, skin
C)lungs, kidneys
D)brain stem, heart
E)spleen, liver
A)kidneys, liver
B)lungs, skin
C)lungs, kidneys
D)brain stem, heart
E)spleen, liver
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18
Which one of the following pairs cannot be mixed together to form a buffer solution?
A)NH3, NH4Cl
B)NaC2H3O2, HCl (C2H3O2- = acetate)
C)RbOH, HBr
D)KOH, HF
E)H3PO4, KH2PO4
A)NH3, NH4Cl
B)NaC2H3O2, HCl (C2H3O2- = acetate)
C)RbOH, HBr
D)KOH, HF
E)H3PO4, KH2PO4
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19
The addition of KOH and ________ to water produces a buffer solution.
A)HI
B)NH3
C)KF
D)LiC2H3O2
E)none of the above
A)HI
B)NH3
C)KF
D)LiC2H3O2
E)none of the above
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20
A solution containing which one of the following pairs of substances will be a buffer solution?
A)NaI, HI
B)KBr, HBr
C)RbCl, HCl
D)CsF, HF
E)none of the above
A)NaI, HI
B)KBr, HBr
C)RbCl, HCl
D)CsF, HF
E)none of the above
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21
The pH of a solution prepared by dissolving 0.550 mol of solid methylamine hydrochloride (CH3NH3Cl)in of methylamine (CH3NH2)is ________.The Kb for methylamine is (Assume the final volume is 1.00 L.)
A)11.03
B)2.97
C)3.75
D)10.64
E)10.25
of methylamine (CH3NH2)is ________.The Kb for methylamine is (Assume the final volume is 1.00 L.)A)11.03
B)2.97
C)3.75
D)10.64
E)10.25
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22
A 25.0 mL sample of 0.723 M HClO4 is titrated with a KOH solution.The H3O+ concentration after the addition of of KOH is ________ M.
A)0.4
B)1 × 10-7
C)0.7
D)3 × 10-13
E)4 × 10-2
KOH solution.The H3O+ concentration after the addition of of KOH is ________ M.A)0.4
B)1 × 10-7
C)0.7
D)3 × 10-13
E)4 × 10-2
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23
A 25.0 mL sample of a solution of an unknown compound is titrated with a 0.115 M NaOH solution.The titration curve above was obtained.The unknown compound is ________.
A)a strong acid
B)a strong base
C)a weak acid
D)a weak base
E)neither an acid nor a base
A)a strong acid
B)a strong base
C)a weak acid
D)a weak base
E)neither an acid nor a base
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24
Which compound listed below has the greatest molar solubility in water?
A)CdCO3
B)Cd(OH)2
C)AgI
D)CaF2
E)ZnCO3
A)CdCO3
B)Cd(OH)2
C)AgI
D)CaF2
E)ZnCO3
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25
Which one of the following is not amphoteric?
A)Al(OH)3
B)Ca(OH)2
C)Cr(OH)3
D)Zn(OH)2
E)Sn(OH)2
A)Al(OH)3
B)Ca(OH)2
C)Cr(OH)3
D)Zn(OH)2
E)Sn(OH)2
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26
Human blood is considered to be ________.
A)neutral
B)very basic
C)slightly basic
D)slightly acidic
E)very acidic
A)neutral
B)very basic
C)slightly basic
D)slightly acidic
E)very acidic
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27
The Ka of benzoic acid is 6.30 × 10-5.The pH of a buffer prepared by combining 50.0 mL of potassium benzoate and 50.0 mL of 1.00 M benzoic acid is ________.
A)1.705
B)0.851
C)3.406
D)4.201
E)2.383
potassium benzoate and 50.0 mL of 1.00 M benzoic acid is ________.A)1.705
B)0.851
C)3.406
D)4.201
E)2.383
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28
Which compound listed below has the smallest molar solubility in water?
A)ZnCO3
B)Cd(OH)2
C)CdCO3
D)AgI
E)CaF2
A)ZnCO3
B)Cd(OH)2
C)CdCO3
D)AgI
E)CaF2
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29
A result of the common-ion effect is ________.
A)that some ions, such as Na+ (aq), frequently appear in solutions but do not participate in solubility equilibria
B)that common ions, such as Na+ (aq), don't affect equilibrium constants
C)that the selective precipitation of a metal ion, such as Ag+, is promoted by the addition of an appropriate counterion (X-)that produces a compound (AgX)with a very low solubility
D)that ions such as K+ and Na+ are common ions, so that their values in equilibrium constant expressions are always 1.00
E)that common ions precipitate all counter-ions
A)that some ions, such as Na+ (aq), frequently appear in solutions but do not participate in solubility equilibria
B)that common ions, such as Na+ (aq), don't affect equilibrium constants
C)that the selective precipitation of a metal ion, such as Ag+, is promoted by the addition of an appropriate counterion (X-)that produces a compound (AgX)with a very low solubility
D)that ions such as K+ and Na+ are common ions, so that their values in equilibrium constant expressions are always 1.00
E)that common ions precipitate all counter-ions
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30
For which salt should the aqueous solubility be most sensitive to pH?
A)MgCl2
B)Mg(NO3)2
C)MgF2
D)MgBr2
E)MgI2
A)MgCl2
B)Mg(NO3)2
C)MgF2
D)MgBr2
E)MgI2
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31
Which one of the following is amphoteric?
A)H2SO4
B)H2O2
C)CO2
D)H2O
E)NaOH
A)H2SO4
B)H2O2
C)CO2
D)H2O
E)NaOH
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32
A 50.0 mL sample of a solution of a monoprotic acid is titrated with a 0.115 M NaOH solution.The titration curve above was obtained.The concentration of the monoprotic acid is about ________ mol/L.
A)0.120
B)25.0
C)0.240
D)0.0600
E)0.100
A)0.120
B)25.0
C)0.240
D)0.0600
E)0.100
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33
The molar solubility of ________ is not affected by the pH of the solution.
A)Na3PO4
B)NaF
C)KNO3
D)AlCl3
E)MnS
A)Na3PO4
B)NaF
C)KNO3
D)AlCl3
E)MnS
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34
Why does fluoride treatment render teeth more resistant to decay?
A)Fluoride kills the bacteria in the mouth that make the acids that decay teeth.
B)Fluoride stimulates production of tooth enamel to replace that lost to decay.
C)Fluoride reduces saliva production, keeping teeth drier and thus reducing decay.
D)Fluoride converts hydroxyapatite to fluoroapatite that is less reactive with acids.
E)Fluoride dissolves plaque, reducing its decaying contact with teeth.
A)Fluoride kills the bacteria in the mouth that make the acids that decay teeth.
B)Fluoride stimulates production of tooth enamel to replace that lost to decay.
C)Fluoride reduces saliva production, keeping teeth drier and thus reducing decay.
D)Fluoride converts hydroxyapatite to fluoroapatite that is less reactive with acids.
E)Fluoride dissolves plaque, reducing its decaying contact with teeth.
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35
A 25.0 mL sample of a solution of a monoprotic acid is titrated with a 0.115 M NaOH solution.The titration curve above was obtained.Which of the following indicators would be best for this titration?
A)methyl red
B)bromthymol blue
C)thymol blue
D)phenolpthalein
E)bromocresol purple
A)methyl red
B)bromthymol blue
C)thymol blue
D)phenolpthalein
E)bromocresol purple
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36
Calculate the pH of a solution prepared by dissolving of benzoic acid and of sodium benzoate in water sufficient to yield of solution.The Ka of benzoic acid is
A)2.516
B)3.892
C)4.502
D)10.158
E)4.195
of benzoic acid and of sodium benzoate in water sufficient to yield of solution.The Ka of benzoic acid is A)2.516
B)3.892
C)4.502
D)10.158
E)4.195
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37
Calculate the pH of a solution prepared by dissolving of acetic acid and of sodium acetate in water sufficient to yield of solution.The Ka of acetic acid is
A)2.516
B)3.892
C)4.502
D)10.158
E)5.056
of acetic acid and of sodium acetate in water sufficient to yield of solution.The Ka of acetic acid is A)2.516
B)3.892
C)4.502
D)10.158
E)5.056
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38
The pH of a solution prepared by dissolving 0.350 mol of acid in of of conjugate base is ________.The Kb for the conjugate base is (Assume the final volume is 1.00 L.)
A)11.23
B)1.66
C)11.14
D)2.77
E)none of the above
of of conjugate base is ________.The Kb for the conjugate base is (Assume the final volume is 1.00 L.)A)11.23
B)1.66
C)11.14
D)2.77
E)none of the above
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39
In which one of the following solutions is silver chloride the most soluble?
A)0.200 M HCl
B)0.750 M LiNO3
C)0.0150 M NH3
D)0.185 M KCl
E)pure H2O
A)0.200 M HCl
B)0.750 M LiNO3
C)0.0150 M NH3
D)0.185 M KCl
E)pure H2O
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40
Decreasing the pH of blood will cause hemoglobin to release ________.
A)CO2
B)N2
C)H2
D)O2
E)Fe
A)CO2
B)N2
C)H2
D)O2
E)Fe
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41
The pH of a solution prepared by mixing 50.0 mL of 0.125 M NaOH and 40.0 mL of 0.125 M HNO3 is ________.
A)13.29
B)7.00
C)8.11
D)11.00
E)12.14
A)13.29
B)7.00
C)8.11
D)11.00
E)12.14
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42
The Ksp for Cu(OH)2 is 4.8 × 10-20.Determine the molar solubility of Cu(OH)2 in a buffer solution with a pH of 10.1.
A)6.0 × 10-10
B)7.6
C)3.0 × 10-12
D)2.2 × 10-10
E)3.8 × 10-16
A)6.0 × 10-10
B)7.6
C)3.0 × 10-12
D)2.2 × 10-10
E)3.8 × 10-16
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43
The solubility of lead (II)chloride (PbCl2)is What is the Ksp of PbCl2?
A)5.0 × 10-4
B)4.1 × 10-6
C)3.1 × 10-7
D)1.6 × 10-5
E)1.6 × 10-2
What is the Ksp of PbCl2?A)5.0 × 10-4
B)4.1 × 10-6
C)3.1 × 10-7
D)1.6 × 10-5
E)1.6 × 10-2
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44
What is the solubility (in M)of PbCl2 in a solution of HCl? The Ksp of PbCl2 is
A)2.0 × 10-3
B)1.1 × 10-4
C)1.8 × 10-4
D)7.1 × 10-4
E)1.6 × 10-5
solution of HCl? The Ksp of PbCl2 is A)2.0 × 10-3
B)1.1 × 10-4
C)1.8 × 10-4
D)7.1 × 10-4
E)1.6 × 10-5
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45
The concentration of iodide ions in a saturated solution of silver iodide is ________ M.The solubility product constant of AgI is
A)3.8 × 10-11
B)3.0 × 10-10
C)9.1 × 10-9
D)3.5 × 10-9
E)1.4 × 10-8
A)3.8 × 10-11
B)3.0 × 10-10
C)9.1 × 10-9
D)3.5 × 10-9
E)1.4 × 10-8
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46
Calculate the pH of a solution that is 0.278 M in sodium formate ( )and in formic acid The of formic acid is 1.77 × .
A)3.843
B)3.647
C)13.90
D)10.16
E)4.954
)and in formic acid The of formic acid is 1.77 × .A)3.843
B)3.647
C)13.90
D)10.16
E)4.954
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47
The concentration of iodide ions in a saturated solution of lead (II)iodide is ________ M.The solubility product constant of PbI2 is
A)3.8 × 10-4
B)3.0 × 10-3
C)1.5 × 10-3
D)3.5 × 10-9
E)1.4 × 10-8
A)3.8 × 10-4
B)3.0 × 10-3
C)1.5 × 10-3
D)3.5 × 10-9
E)1.4 × 10-8
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48
Calculate the percent ionization of formic acid ( H)in a solution that is 0.322 M in formic acid and 0.178 M in sodium formate ( ).The of formic acid is 1.77 × .
A)35.6
B)0.1011
C)10.8
D)1.03 × 10-3
E)3.488
H)in a solution that is 0.322 M in formic acid and 0.178 M in sodium formate ( ).The of formic acid is 1.77 × .A)35.6
B)0.1011
C)10.8
D)1.03 × 10-3
E)3.488
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49
Calculate the maximum concentration (in M)of silver ions (Ag+)in a solution that contains of CO32-.The Ksp of Ag2CO3 is
A)1.8 × 10-5
B)1.4 × 10-6
C)2.8 × 10-6
D)3.2 × 10-10
E)8.1 × 10-12
of CO32-.The Ksp of Ag2CO3 is A)1.8 × 10-5
B)1.4 × 10-6
C)2.8 × 10-6
D)3.2 × 10-10
E)8.1 × 10-12
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50
What is the percent ionization of nitrous acid in a solution that is 0.222 M in nitrous acid (HNO2)and 0.278 M in potassium nitrite (KNO2)? The acid dissociation constant of nitrous acid is
A)55.6
B)15.5
C)2.78 ×
D)3.448
E)0.162
A)55.6
B)15.5
C)2.78 ×
D)3.448
E)0.162
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51
A 50.0 mL sample of an aqueous H2SO4 solution is titrated with a NaOH solution.The equivalence point is reached with of the base.The concentration of H2SO4 is ________ M.
A)0.234
B)0.469
C)0.150
D)0.300
E)0.938
NaOH solution.The equivalence point is reached with of the base.The concentration of H2SO4 is ________ M.A)0.234
B)0.469
C)0.150
D)0.300
E)0.938
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52
The pH of a solution prepared by mixing 50.0 mL of 0.125 M KOH and 50.0 mL of 0.125 M HCl is ________.
A)6.29
B)7.00
C)8.11
D)5.78
E)0.00
A)6.29
B)7.00
C)8.11
D)5.78
E)0.00
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53
The concentration of fluoride ions in a saturated solution of barium fluoride is ________ M.The solubility product constant of BaF2 is
A)3.8 × 10-4
B)3.0 × 10-3
C)1.5 × 10-2
D)7.5 × 10-3
E)1.4 × 10-4
A)3.8 × 10-4
B)3.0 × 10-3
C)1.5 × 10-2
D)7.5 × 10-3
E)1.4 × 10-4
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54
What is the percent ionization of nitrous acid in a solution that is 0.189 M in nitrous acid? The acid dissociation constant of nitrous acid is
A)0.0450
B)8.51 × 10-5
C)0.594
D)4.20
E)4.88
A)0.0450
B)8.51 × 10-5
C)0.594
D)4.20
E)4.88
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55
Calculate the percent ionization of formic acid ( H)in a solution that is 0.152 M in formic acid.The of formic acid is 1.77 × .
A)2.74 ×
B)0.0180
C)3.44
D)0.581
E)8.44
H)in a solution that is 0.152 M in formic acid.The of formic acid is 1.77 × .A)2.74 ×
B)0.0180
C)3.44
D)0.581
E)8.44
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56
The solubility of manganese (II)hydroxide (Mn(OH)2)is What is the Ksp of Mn(OH)2?
A)1.1 × 10-14
B)4.3 × 10-14
C)2.1 × 10-14
D)4.8 × 10-10
E)2.2 × 10-5
What is the Ksp of Mn(OH)2?A)1.1 × 10-14
B)4.3 × 10-14
C)2.1 × 10-14
D)4.8 × 10-10
E)2.2 × 10-5
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57
The pH of a solution prepared by mixing 40.0 mL of 0.125 M Mg(OH)2 and 150.0 mL of 0.125 M HCl is ________.
A)6.29
B)4.11
C)1.14
D)5.78
E)1.34
A)6.29
B)4.11
C)1.14
D)5.78
E)1.34
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58
Determine the Ksp for magnesium hydroxide (Mg(OH)2)where the solubility of Mg(OH)2 is .
A)2.7 × 10-12
B)1.1 × 10-11
C)2.0 × 10-8
D)3.9 × 10-8
E)1.4 × 10-4
.A)2.7 × 10-12
B)1.1 × 10-11
C)2.0 × 10-8
D)3.9 × 10-8
E)1.4 × 10-4
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59
Calculate the pH of a solution that is 0.322 M in nitrous acid ( )and 0.178 M in potassium nitrite (KNO2).The acid dissociation constant of nitrous acid is 4.50 × .
A)3.093
B)3.607
C)14.26
D)10.91
E)4.589
)and 0.178 M in potassium nitrite (KNO2).The acid dissociation constant of nitrous acid is 4.50 × .A)3.093
B)3.607
C)14.26
D)10.91
E)4.589
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60
Calculate the maximum concentration (in M)of calcium ions (Ca2+)in a solution that contains of CO32-.The Ksp of CaCO3 is
A)5.8 × 10-5
B)6.8 × 10-9
C)3.4 × 10-9
D)6.2 × 10-8
E)1.9 × 10-10
of CO32-.The Ksp of CaCO3 is A)5.8 × 10-5
B)6.8 × 10-9
C)3.4 × 10-9
D)6.2 × 10-8
E)1.9 × 10-10
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61
What is the pH of a buffer solution that is 0.266 M in lactic acid and 0.111 M in sodium lactate? The of lactic acid is 1.4 × .
A)14.38
B)10.53
C)5.38
D)3.47
E)4.23
of lactic acid is 1.4 × .A)14.38
B)10.53
C)5.38
D)3.47
E)4.23
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62
Which solution would have the greatest buffering capacity?
A)0.574 M HF and 0.312 M NaF
B)0.287 M HF and 0.156 M NaF
C)0.189 M HF and 0.103 M NaF
D)1.15 M HF and 0.624 M NaF
E)They are all buffer solutions and would all have the same capacity.
A)0.574 M HF and 0.312 M NaF
B)0.287 M HF and 0.156 M NaF
C)0.189 M HF and 0.103 M NaF
D)1.15 M HF and 0.624 M NaF
E)They are all buffer solutions and would all have the same capacity.
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63
The of some weak acid HA is 1.76 × .The pH of a buffer prepared by combining 15.0 mL of A- and 50.0 mL of 1.00 M HA is ________.
A)1.705
B)4.232
C)0.851
D)2.383
E)3.406
of some weak acid HA is 1.76 × .The pH of a buffer prepared by combining 15.0 mL of A- and 50.0 mL of 1.00 M HA is ________.A)1.705
B)4.232
C)0.851
D)2.383
E)3.406
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64
A solution is prepared by dissolving 0.23 mol of hypochlorous acid and 0.27 mol of sodium hypochlorite in water sufficient to yield 1.00 L of solution.The addition of 0.05 mol of HCl to this buffer solution causes the pH to drop slightly.The pH does not decrease drastically because the HCl reacts with the ________ present in the buffer solution.The of hypochlorous acid is 1.36 × 10-3.
A) O
B)
C)hypochlorite ion
D)hypochlorous acid
E)This is a buffer solution: the pH does not change upon addition of acid or base.
of hypochlorous acid is 1.36 × 10-3.A)
OB)
C)hypochlorite ion
D)hypochlorous acid
E)This is a buffer solution: the pH does not change upon addition of acid or base.
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65
The of ammonia is 1.76 × .What is the pH of a buffer which is prepared by combining 50.0 mL of 1.00 M ammonia and 45.0 mL of 1.00 M ammonium nitrate?
A)9.372
B)4.632
C)4.742
D)9.291
E)none of the above
of ammonia is 1.76 × .What is the pH of a buffer which is prepared by combining 50.0 mL of 1.00 M ammonia and 45.0 mL of 1.00 M ammonium nitrate?A)9.372
B)4.632
C)4.742
D)9.291
E)none of the above
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66
A buffer solution with a pH of 4.31 is prepared with and The Ka of H is
A)0.37
B)0.74
C)4.2 × 10-6
D)8.8 × 10-10
E)0.18
and The Ka of H is A)0.37
B)0.74
C)4.2 × 10-6
D)8.8 × 10-10
E)0.18
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67
0.78 M Na and are required to prepare a buffer solution with a pH of 4.40 .The of H is
A)3.5
B)4.1 × 104
C)1.7
D)0.86
E)0.35
and are required to prepare a buffer solution with a pH of 4.40 .The of H is A)3.5
B)4.1 × 104
C)1.7
D)0.86
E)0.35
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68
What is the pH of a solution which is prepared by dissolving 0.850 mol of N and of in water sufficient to yield 1.00 L of solution? The of ammonia is
A)9.700
B)5.204
C)8.781
D)8.796
E)4.300
and of in water sufficient to yield 1.00 L of solution? The of ammonia is A)9.700
B)5.204
C)8.781
D)8.796
E)4.300
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69
Consider a solution containing 0.100 M fluoride ions and 0.126 M hydrogen fluoride.The concentration of fluoride ions after the addition of 9.00 mL of 0.0100 M HCl to 25.0 mL of this solution is ________ M.
A)0.0735
B)0.0762
C)0.0980
D)0.0709
E)0.00253
A)0.0735
B)0.0762
C)0.0980
D)0.0709
E)0.00253
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70
A buffer solution contains 0.100 M fluoride ions and 0.126 M hydrogen fluoride.What is the concentration (M)of hydrogen fluoride after addition of 9.00 mL of 0.0100 M HCl to 25.0 mL of this solution?
A)0.0900
B)0.122
C)0.130
D)0.0953
E)0.00976
A)0.0900
B)0.122
C)0.130
D)0.0953
E)0.00976
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71
Calculate the pH of a solution prepared by dissolving 0.270 mol of weak acid HA and 0.260 mol of its conjugate base in water sufficient to yield 1.00 L of solution.The of HA is
A)2.099
B)3.736
C)10.264
D)3.952
E)2.307
of HA is A)2.099
B)3.736
C)10.264
D)3.952
E)2.307
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72
acid and formate are required to prepare a buffer solution with a pH of 4.78 .The of formic acid is A)0.17
B)0.083
C)3.3 × 103
D)0.041
E)9.8
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73
A 25.0 mL sample of 0.150 M acetic acid is titrated with a 0.150 M NaOH solution.What is the pH at the equivalence point? The of acetic acid is 4.50 × 10-4.
A)11.74
B)9.26
C)4.74
D)7.00
E)8.81
of acetic acid is 4.50 × 10-4.A)11.74
B)9.26
C)4.74
D)7.00
E)8.81
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74
What is the pH of a solution that contains 0.800 M weak acid ( = 1.76 × )and 0.172 M of its conjugate base?
A)8.578
B)5.422
C)8.370
D)4.087
E)9.913
= 1.76 × )and 0.172 M of its conjugate base?A)8.578
B)5.422
C)8.370
D)4.087
E)9.913
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75
How many milliliters of 0.0839 M NaOH are required to titrate 25.0 mL of to the equivalence point?
A)29.5
B)0.332
C)4.57
D)0.208
E)21.2
to the equivalence point?A)29.5
B)0.332
C)4.57
D)0.208
E)21.2
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76
The addition of hydrofluoric acid and ________ to water produces a buffer solution.
A)NaF
B)HF
C)NaN
D)NaBr
E)KI
A)NaF
B)HF
C)NaN
D)NaBr
E)KI
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77
A solution is prepared by dissolving 0.23 mol of benzoic acid and 0.27 mol of sodium benzoate in water sufficient to yield 1.00 L of solution.The addition of 0.05 mol of NaOH to this buffer solution causes the pH to increase slightly.The pH does not increase drastically because the NaOH reacts with the ________ present in the buffer solution.The of benzoic acid is 6.3 × 10-5.
A) O
B)
C)benzoate
D)benzoic acid
E)This is a buffer solution: the pH does not change upon addition of acid or base.
of benzoic acid is 6.3 × 10-5.A)
OB)
C)benzoate
D)benzoic acid
E)This is a buffer solution: the pH does not change upon addition of acid or base.
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78
What is the pH of a buffer solution that is 0.172 M in hypochlorous acid (HClO)and 0.131 M in sodium hypochlorite? The of hypochlorous acid is 3.8 × .
A)14.12
B)6.70
C)9.07
D)7.54
E)7.30
of hypochlorous acid is 3.8 × .A)14.12
B)6.70
C)9.07
D)7.54
E)7.30
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79
Calculate the pH of a solution prepared by dissolving 0.250 mol of benzoic acid ( H)and of sodium benzoate (Na )in water sufficient to yield 1.00 L of solution.The of benzoic acid is
A)4.409
B)3.965
C)10.035
D)9.591
E)5.190
H)and of sodium benzoate (Na )in water sufficient to yield 1.00 L of solution.The of benzoic acid is A)4.409
B)3.965
C)10.035
D)9.591
E)5.190
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80
A buffer solution with a pH of 4.63 is prepared with acid and formate. The of formic acid is
A)1.1
B)2.1
C)5.4 × 10-6
D)3.0 × 10-8
E)0.54
acid and formate. The of formic acid is A)1.1
B)2.1
C)5.4 × 10-6
D)3.0 × 10-8
E)0.54
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