Question 1

A 100.0 mL sample of 0.18 mol L-1 HClO4 is titrated with 0.27 mol L-1 NaOH.Determine the pH of the solution after the addition of 30.0 mL of NaOH.

Accepted Answer

A) 0.86 
B) 1.21 
C) 2.00 
D) 1.12 
E) 2.86 
A) 0.86 
B) 1.21 
C) 2.00 
D) 1.12 
E) 2.86

Question 2

A 100.0 mL sample of 0.18 mol L-1 HClO4 is titrated with 0.27 mol L-1 NaOH.Determine the pH of the solution after the addition of 100.0 mL of NaOH.

Accepted Answer

A) 13.1 
B) 12.7 
C) 1.3 
D) 0.9 
E) 12.9 
A) 13.1 
B) 12.7 
C) 1.3 
D) 0.9 
E) 12.9

Question 3

Describe the information necessary (and why)to choose a good indicator for a weak acid-strong base titration.

Accepted Answer

In order to choose an appropriate indica

Question 4

Calculate the solubility (in g L-1)of silver carbonate in water at 25 °C if the Ksp for $\mathrm { Ag } _ { 2 } \mathrm { CO } _ { 3 }$ is 8.4 × $10 ^ { - 12 }$ .

Accepted Answer

A) 8.0 × 10-4 g L-1 
B) 3.5 × 10-2 g L-1 
C) 4.4 × 10-2 g L-1 
D) 5.6 × 10-2 g L-1 
A) 8.0 × 10-4 g L-1 
B) 3.5 × 10-2 g L-1 
C) 4.4 × 10-2 g L-1 
D) 5.6 × 10-2 g L-1

Question 5

Determine the molar solubility of CuCl in a solution containing 0.050 mol L-1 KCl.Ksp (CuCl)= 1.0 × 10-6.

Accepted Answer

A) 1.0 × 10-12 mol L-1 
B) 5.0 × 10-7 mol L-1 
C) 2.0 × 10-5 mol L-1 
D) 1.0 × 10-3 mol L-1 
E) 0.050 mol L-1 
A) 1.0 × 10-12 mol L-1 
B) 5.0 × 10-7 mol L-1 
C) 2.0 × 10-5 mol L-1 
D) 1.0 × 10-3 mol L-1 
E) 0.050 mol L-1

Question 6

A 100.0 mL sample of 0.18 mol L-1 HClO4 is titrated with 0.27 mol L-1 NaOH.Determine the pH of the solution before the addition of any NaOH.

Accepted Answer

A) 1.74 
B) 1.05 
C) 0.74 
D) 0.57 
E) 1.57 
A) 1.74 
B) 1.05 
C) 0.74 
D) 0.57 
E) 1.57

Question 7

A 25.0 mL sample of 0.150 mol L-1 formic acid is titrated with a 0.150 mol L-1 NaOH solution.What is the pH at the equivalence point? The $K _ { a }$ of formic acid is 1.8 × 10-4.

Accepted Answer

A) 11.38 
B) 10.26 
C) 5.69 
D) 8.31 
E) 7.00 
A) 11.38 
B) 10.26 
C) 5.69 
D) 8.31 
E) 7.00

Question 8

A sample contains Ba3(PO4)2, CdS,AgCl,NH4Cl,and ZnS.Identify the precipitate formed after the addition of 6 mol L-1 HCl followed by the addition of H2S and 0.2 mol L-1 HCl.

Accepted Answer

A) Ba3(PO4)2 
B) CdS 
C) AgCl 
D) NH4Cl 
E) ZnS 
A) Ba3(PO4)2 
B) CdS 
C) AgCl 
D) NH4Cl 
E) ZnS

Question 9

Determine the molar solubility of MgCO3 in pure water.Ksp (MgCO3)= 6.82 × 10-6.

Accepted Answer

A) 6.82 × 10-6 mol L-1 
B) 3.41 × 10-6 mol L-1 
C) 4.65 × 10-3 mol L-1 
D) 2.61 × 10-3 mol L-1 
E) 3.25 × 10-4 mol L-1 
A) 6.82 × 10-6 mol L-1 
B) 3.41 × 10-6 mol L-1 
C) 4.65 × 10-3 mol L-1 
D) 2.61 × 10-3 mol L-1 
E) 3.25 × 10-4 mol L-1

Question 10

Define a buffer.

Accepted Answer

Buffers contain significant am

Question 11

What volume of 5.00 × 10-3 mol L-1 HNO3 is needed to titrate 80.00 mL of 5.00 × 10-3 mol L-1 Ca(OH)2 to the equivalence point?

Accepted Answer

A) 10.0 mL 
B) 40.0 mL 
C) 80.0 mL 
D) 160.mL 
A) 10.0 mL 
B) 40.0 mL 
C) 80.0 mL 
D) 160.mL

Question 12

A solution of NaF is added dropwise to a solution that is 0.0188 mol L-1 in $\mathrm { Ba } ^ { 2 + }$ .When the concentration of $\mathrm { F } ^ { - }$ exceeds ________ mol L-1, $\mathrm { BaF } _ { 2 }$ will precipitate.Neglect volume changes.For $\mathrm { BaF } _ { 2 }$ , $K _ { \mathrm { sp } } = 1.7 \times 10 ^ { - 6 }$

Accepted Answer

A) 9.0 × 10-5 
B) 3.2 × 10-8 
C) 4.5 × 10-5 
D) 2.4 × 10-3 
E) 9.5 × 10-3 
A) 9.0 × 10-5 
B) 3.2 × 10-8 
C) 4.5 × 10-5 
D) 2.4 × 10-3 
E) 9.5 × 10-3

Question 13

Identify the expression for the solubility product constant for PbCl2.

Accepted Answer

A)  $\frac { \left[ \mathrm { Pb } ^ { 2 } + \right] \left[ \mathrm { Cl } ^ { - } \right] ^ { 2 } } { \left[ \mathrm { PbCl } _ { 2 } \right] }$ 
B)    
C) [Pb2+][Cl-]2 
D)  $\frac { \left[ \mathrm { Pb } ^ { 2 } + \right] ^ { 2 } \left[ \mathrm { Cl } ^ { - } \right] } { \left[ \mathrm { PbCl } _ { 2 } \right] }$ 
E) [Pb2+]2[Cl-] 
A)  $\frac { \left[ \mathrm { Pb } ^ { 2 } + \right] \left[ \mathrm { Cl } ^ { - } \right] ^ { 2 } } { \left[ \mathrm { PbCl } _ { 2 } \right] }$ 
B)    
C) [Pb2+][Cl-]2 
D)  $\frac { \left[ \mathrm { Pb } ^ { 2 } + \right] ^ { 2 } \left[ \mathrm { Cl } ^ { - } \right] } { \left[ \mathrm { PbCl } _ { 2 } \right] }$ 
E) [Pb2+]2[Cl-]

Question 14

Identify the expression for the solubility product constant for Cr2(CO3)3.

Accepted Answer

A) [Cr3+]2[CO32-]3 
B)  $\frac { \left[ \mathrm { Cr } ^ { 3 + } \right] ^ { 2 } \left[ \mathrm { CO } _ { 3 } ^ { 2 - } \right] ^ { 3 } } { \left[ \mathrm { Cr } _ { 2 } \left( \mathrm { CO } _ { 3 } \right) _ { 3 } \right] }$ 
C)  $\frac { \left[ \mathrm { Cr } _ { 2 } \left( \mathrm { CO } _ { 3 } \right) 3 \right] } { \left[ \mathrm { Cr } ^ { 3 + } \right] ^ { 2 } \left[ \mathrm { CO } _ { 3 } { } ^ { 2 - } \right] ^ { 3 } }$ 
D)  $\frac { \left[ \mathrm { Cr } ^ { 3 + } \right] ^ { 3 } \left[ \mathrm { CO } _ { 3 } ^ { 2 - } \right] ^ { 2 } } { \left[ \mathrm { Cr } _ { 2 } \left( \mathrm { CO } _ { 3 } \right) _ { 3 } \right] }$ 
E) [Cr3+]3[CO32-]2 
A) [Cr3+]2[CO32-]3 
B)  $\frac { \left[ \mathrm { Cr } ^ { 3 + } \right] ^ { 2 } \left[ \mathrm { CO } _ { 3 } ^ { 2 - } \right] ^ { 3 } } { \left[ \mathrm { Cr } _ { 2 } \left( \mathrm { CO } _ { 3 } \right) _ { 3 } \right] }$ 
C)  $\frac { \left[ \mathrm { Cr } _ { 2 } \left( \mathrm { CO } _ { 3 } \right) 3 \right] } { \left[ \mathrm { Cr } ^ { 3 + } \right] ^ { 2 } \left[ \mathrm { CO } _ { 3 } { } ^ { 2 - } \right] ^ { 3 } }$ 
D)  $\frac { \left[ \mathrm { Cr } ^ { 3 + } \right] ^ { 3 } \left[ \mathrm { CO } _ { 3 } ^ { 2 - } \right] ^ { 2 } } { \left[ \mathrm { Cr } _ { 2 } \left( \mathrm { CO } _ { 3 } \right) _ { 3 } \right] }$ 
E) [Cr3+]3[CO32-]2

Question 15

The molar solubility of CuI is 2.26 × 10-6 mol L-1 in pure water.Calculate the Ksp for CuI.

Accepted Answer

A) 5.11 × 10-12 
B) 4.52 × 10-6 
C) 1.50 × 10-3 
D) 4.62 × 10-17 
E) 1.02 × 10-11 
A) 5.11 × 10-12 
B) 4.52 × 10-6 
C) 1.50 × 10-3 
D) 4.62 × 10-17 
E) 1.02 × 10-11

Question 16

What is the pH of a solution made by mixing 30.00 mL of 0.10 mol L-1 acetic acid (CH3COOH)with 50.00 mL of 0.100 mol L-1 KOH? Assume that the volumes of the solutions are additive.Ka = 1.8 × 10-5 for $\mathrm { CH } _ { 3 } \mathrm { COOH }$

Accepted Answer

A) 8.26 
B) 9.26 
C) 11.13 
D) 12.40 
A) 8.26 
B) 9.26 
C) 11.13 
D) 12.40

Question 17

An acid solution is 0.100 mol L-1 in HCl and 0.200 mol L-1 $\mathrm { H } _ { 2 }$ $\mathrm { SO } _ { 4 }$ .What volume of a 0.150 mol L-1 KOH solution would completely neutralize 500.0 mL of this solution?

Accepted Answer

A) 0.700 L 
B) 1.98 L 
C) 1.67 L 
D) 1.02 L 
E) 0.250 L 
A) 0.700 L 
B) 1.98 L 
C) 1.67 L 
D) 1.02 L 
E) 0.250 L

Question 18

Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 mol L-1 NH4Cl with 200.0 mL of 0.12 mol L-1 NH3.The Kb for NH3 is 1.8 × 10-5.

Accepted Answer

A) 9.06 
B) 9.45 
C) 4.55 
D) 4.74 
E) 9.26 
A) 9.06 
B) 9.45 
C) 4.55 
D) 4.74 
E) 9.26

Question 19

Predict the number of equivalence point(s)in the titration for a diprotic acid with a strong base.

Accepted Answer

The answer of Predict the number of equivalence point(s)in the...

Exam 16: Aqueous Ionic Equilibrium

A 100.0 mL sample of 0.18 mol L-1 HClO4 is titrated with 0.27 mol L-1 NaOH.Determine the pH of the solution after the addition of 30.0 mL of NaOH.

A 100.0 mL sample of 0.18 mol L-1 HClO4 is titrated with 0.27 mol L-1 NaOH.Determine the pH of the solution after the addition of 100.0 mL of NaOH.

Describe the information necessary (and why)to choose a good indicator for a weak acid-strong base titration.

Calculate the solubility (in g L-1)of silver carbonate in water at 25 °C if the Ksp for Ag2CO3\mathrm { Ag } _ { 2 } \mathrm { CO } _ { 3 }Ag2​CO3​ is 8.4 × 10−1210 ^ { - 12 }10−12 .

Determine the molar solubility of CuCl in a solution containing 0.050 mol L-1 KCl.Ksp (CuCl)= 1.0 × 10-6.

A 100.0 mL sample of 0.18 mol L-1 HClO4 is titrated with 0.27 mol L-1 NaOH.Determine the pH of the solution before the addition of any NaOH.

A 25.0 mL sample of 0.150 mol L-1 formic acid is titrated with a 0.150 mol L-1 NaOH solution.What is the pH at the equivalence point? The KaK _ { a }Ka​ of formic acid is 1.8 × 10-4.

A sample contains Ba3(PO4)2, CdS,AgCl,NH4Cl,and ZnS.Identify the precipitate formed after the addition of 6 mol L-1 HCl followed by the addition of H2S and 0.2 mol L-1 HCl.

Determine the molar solubility of MgCO3 in pure water.Ksp (MgCO3)= 6.82 × 10-6.

Define a buffer.

What volume of 5.00 × 10-3 mol L-1 HNO3 is needed to titrate 80.00 mL of 5.00 × 10-3 mol L-1 Ca(OH)2 to the equivalence point?

Identify the expression for the solubility product constant for PbCl2.

Identify the expression for the solubility product constant for Cr2(CO3)3.

The molar solubility of CuI is 2.26 × 10-6 mol L-1 in pure water.Calculate the Ksp for CuI.

What is the pH of a solution made by mixing 30.00 mL of 0.10 mol L-1 acetic acid (CH3COOH)with 50.00 mL of 0.100 mol L-1 KOH? Assume that the volumes of the solutions are additive.Ka = 1.8 × 10-5 for CH3COOH\mathrm { CH } _ { 3 } \mathrm { COOH }CH3​COOH

An acid solution is 0.100 mol L-1 in HCl and 0.200 mol L-1 H2\mathrm { H } _ { 2 }H2​ SO4\mathrm { SO } _ { 4 }SO4​ .What volume of a 0.150 mol L-1 KOH solution would completely neutralize 500.0 mL of this solution?

Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 mol L-1 NH4Cl with 200.0 mL of 0.12 mol L-1 NH3.The Kb for NH3 is 1.8 × 10-5.

Predict the number of equivalence point(s)in the titration for a diprotic acid with a strong base.

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A 100.0 mL sample of 0.18 mol L^-1 HClO₄ is titrated with 0.27 mol L^-1 NaOH.Determine the pH of the solution after the addition of 30.0 mL of NaOH.

A 100.0 mL sample of 0.18 mol L^-1 HClO₄ is titrated with 0.27 mol L^-1 NaOH.Determine the pH of the solution after the addition of 100.0 mL of NaOH.

Calculate the solubility (in g L^-1)of silver carbonate in water at 25 °C if the K_sp for $\mathrm { Ag } _ { 2 } \mathrm { CO } _ { 3 }$ is 8.4 × $10 ^ { - 12 }$ .

Determine the molar solubility of CuCl in a solution containing 0.050 mol L^-1 KCl.K_sp (CuCl)= 1.0 × 10^-6.

A 100.0 mL sample of 0.18 mol L^-1 HClO₄ is titrated with 0.27 mol L^-1 NaOH.Determine the pH of the solution before the addition of any NaOH.

A 25.0 mL sample of 0.150 mol L^-1 formic acid is titrated with a 0.150 mol L^-1 NaOH solution.What is the pH at the equivalence point? The $K _ { a }$ of formic acid is 1.8 × 10^-4.

A sample contains Ba₃(PO₄)₂,CdS,AgCl,NH₄Cl,and ZnS.Identify the precipitate formed after the addition of 6 mol L^-1 HCl followed by the addition of H₂S and 0.2 mol L^-1 HCl.

Determine the molar solubility of MgCO₃in pure water.K_sp (MgCO₃)= 6.82 × 10^-6.

What volume of 5.00 × 10^-3 mol L^-1 HNO₃ is needed to titrate 80.00 mL of 5.00 × 10^-3 mol L^-1 Ca(OH)₂ to the equivalence point?

Identify the expression for the solubility product constant for PbCl₂.

Identify the expression for the solubility product constant for Cr₂(CO₃)₃.

The molar solubility of CuI is 2.26 × 10^-6 mol L^-1 in pure water.Calculate the K_sp for CuI.

What is the pH of a solution made by mixing 30.00 mL of 0.10 mol L^-1 acetic acid (CH₃COOH)with 50.00 mL of 0.100 mol L^-1 KOH? Assume that the volumes of the solutions are additive.K_a = 1.8 × 10^-5for $\mathrm { CH } _ { 3 } \mathrm { COOH }$

An acid solution is 0.100 mol L^-1 in HCl and 0.200 mol L^-1 $\mathrm { H } _ { 2 }$ $\mathrm { SO } _ { 4 }$ .What volume of a 0.150 mol L^-1 KOH solution would completely neutralize 500.0 mL of this solution?

Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 mol L^-1 NH₄Cl with 200.0 mL of 0.12 mol L^-1 NH₃.The K_b for NH₃ is 1.8 × 10^-5.