Question 1

Calculate the molar solubility of thallium(I)chloride in 0.30 M NaCl at 25°C.Ksp for TlCl is 1.7 × 10-4.

Accepted Answer

A) 5.1 × 10-5 M 
B) 5.7 × 10-4 M 
C) 7.1 × 10-3 M 
D) 1.3 × 10-2 M 
A) 5.1 × 10-5 M 
B) 5.7 × 10-4 M 
C) 7.1 × 10-3 M 
D) 1.3 × 10-2 M B

Question 2

A buffer prepared by mixing 55.0 mL of 0.40 M HF with 55.0 mL of 0.40 M NaF will have a pH that is ________ 7.0.

Accepted Answer

less than

Question 3

What is the scandium ion concentration for a saturated solution of Sc(OH)3 if the Ksp for Sc(OH)3 is

Accepted Answer

A) 3.00 × 10-8 M 
B) 1.31 × 10-8 M 
C) 3.22 × 10-10 M 
D) 3.76 × 10-8 M 
A) 3.00 × 10-8 M 
B) 1.31 × 10-8 M 
C) 3.22 × 10-10 M 
D) 3.76 × 10-8 M B

Question 4

What is the pH of the resulting solution if 25 mL of 0.432 M methylamine,CH3NH2,is added to 15 mL of 0.234 M HCl? Assume that the volumes of the solutions are additive.Ka = 2.70 × 10-11 for CH3NH3+.

Accepted Answer

A) 3.11 
B) 3.74 
C) 10.26 
D) 10.89 
A) 3.11 
B) 3.74 
C) 10.26 
D) 10.89

Question 5

What is the pH of a buffer system made by dissolving 10.70 grams of NH4Cl and 20.00 mL of 12.0 M NH3 in enough water to make 1.000 L of solution? Kb = 1.8 × 10-5 for NH3.

Accepted Answer

A) 9.18 
B) 9.26 
C) 9.34 
D) 11.03 
A) 9.18 
B) 9.26 
C) 9.34 
D) 11.03

Question 6

The following pictures represent solutions that contain a weak acid HA (pKS1U1B1aS1U1B0 = 5.0)and its potassium salt KA.Unshaded spheres represent H atoms and shaded spheres represent AS1U1P1-S1S1P0 ions.(KS1U1P1+S1S1P0,HS1U1B13S1U1B0OS1U1P1+S1S1P0,OHS1U1P1-S1S1P0,and solvent HS1U1B12S1U1B0O molecules have been omitted for clarity. )  
-Which solution has the largest percent dissociation of HA?

Accepted Answer

A) (1) 
B) (2) 
C) (3) 
D) (4) 
A) (1) 
B) (2) 
C) (3) 
D) (4)

Question 7

State whether the solubility of Mg(OH)2 will increase or decrease upon the addition of aqueous solutions of a)HCl,b)LiOH,c)NH3.

Accepted Answer

a)increase

Question 8

The following pictures represent solutions that contain a weak acid HA and/or its potassium salt KA.Unshaded spheres represent H atoms and shaded spheres represent AS1U1P1-S1S1P0 ions.(KS1U1P1+S1S1P0,HS1U1B13S1U1B0OS1U1P1+S1S1P0,OHS1U1P1-S1S1P0,and solvent HS1U1B12S1U1B0O molecules have been omitted for clarity. )  
-Which solution has the highest pH?

Accepted Answer

A) (1) 
B) (2) 
C) (3) 
D) (4) 
A) (1) 
B) (2) 
C) (3) 
D) (4)

Question 9

The following pictures represent solutions at various stages in the titration of a weak diprotic acid HS1U1B12S1U1B0A with aqueous KOH.Unshaded spheres represent H atoms,black spheres represent oxygen atoms,and shaded spheres represent AS1U1P12-S1S1P0 ions.(KS1U1P1+S1S1P0,HS1U1B13S1U1B0OS1U1P1+S1S1P0 initially present,OHS1U1P1-S1S1P0 initially present and solvent water molecules have been omitted for clarity).  
-Which picture represents the system at the first equivalence point?

Accepted Answer

A) (1) 
B) (2) 
C) (3) 
D) (4) 
A) (1) 
B) (2) 
C) (3) 
D) (4)

Question 10

What is the pH at the equivalence point of a weak base-strong acid titration if 20.00 mL of NaOCl requires 28.30 mL of 0.50 M HCl? Ka = 3.0 × 10-8 for HOCl.

Accepted Answer

A) 0.30 
B) 3.18 
C) 3.76 
D) 4.03 
A) 0.30 
B) 3.18 
C) 3.76 
D) 4.03

Question 11

What is the [CH3CO2-]/[CH3CO2H] ratio necessary to make a buffer solution with a pH of 4.44? Ka = 1.8 × 10-5 for CH3CO2H.

Accepted Answer

A) 0.50:1 
B) 0.94:1 
C) 1.1:1 
D) 2.0:1 
A) 0.50:1 
B) 0.94:1 
C) 1.1:1 
D) 2.0:1

Question 12

Which is a net ionic equation for the neutralization reaction of a weak acid with a weak base?

Accepted Answer

A) H3O+(aq)+ OH-(aq)⇌ 2 H2O(l) 
B) HF(aq)+ NH3(aq)⇌ NH4+(aq)+ F-(aq) 
C) HCl(aq)+ OH-(aq)⇌ H2O(l)+ Cl-(aq) 
D) H3O+(aq)+ NH3(aq)⇌ NH4+(aq)+ H2O(l) 
A) H3O+(aq)+ OH-(aq)⇌ 2 H2O(l) 
B) HF(aq)+ NH3(aq)⇌ NH4+(aq)+ F-(aq) 
C) HCl(aq)+ OH-(aq)⇌ H2O(l)+ Cl-(aq) 
D) H3O+(aq)+ NH3(aq)⇌ NH4+(aq)+ H2O(l)

Question 13

Calculate the Ksp for silver sulfate if the solubility of Ag2SO4 in pure water is 4.5 g/L.

Accepted Answer

A) 3.0 × 10-6 
B) 1.2 × 10-5 
C) 2.1 × 10-4 
D) 4.2 × 10-4 
A) 3.0 × 10-6 
B) 1.2 × 10-5 
C) 2.1 × 10-4 
D) 4.2 × 10-4

Question 14

The balanced net ionic equation for the neutralization reaction involving equal molar amounts of HI  and KOH is ________.

Accepted Answer

H₃O⁺(aq)+ OH

Question 15

The half equivalence point in the titration of 0.100 M CH3NH2 (Kb = 3.7 × 10-4)with 0.250 M HCl occurs at pH = ________.

Accepted Answer

Question 16

What is the pH of the solution formed when 25 mL of 0.173 M NaOH is added to 35 mL of 0.342 M HCl?

Accepted Answer

The answer of What is the pH of the solution...

Question 17

The pH of a solution of ethylamine,C2H5NH2 (Kb = 6.4 × 10-4)and ethylammium bromide,C2H5NH3Br is 11.00.What is the molarity of C2H5NH3Br if the molarity of C2H5NH2 is 0.025 M?

Accepted Answer

Question 18

What is the pH of a solution prepared by mixing 25.00 mL of 0.10 M CH3CO2H with 25.00 mL of 0.040 M CH3CO2Na? Assume that the volume of the solutions are additive and that Ka = 1.8 × 10-5 for CH3CO2H.

Accepted Answer

A) 2.87 
B) 4.35 
C) 4.75 
D) 5.14 
A) 2.87 
B) 4.35 
C) 4.75 
D) 5.14

Question 19

What is the equation relating the equilibrium constant Kn for the neutralization of a weak acid with a weak base to the Ka of the acid,the Kb of the base and Kw?

Accepted Answer

A) Kn = 1/KaKbKw 
B) Kn =   
C) Kn =   
D) Kn =   
A) Kn = 1/KaKbKw 
B) Kn =   
C) Kn =   
D) Kn =

Question 20

The following pictures represent solutions that contain a weak acid HA and/or its potassium salt KA.Unshaded spheres represent H atoms and shaded spheres represent AS1U1P1-S1S1P0 ions.(KS1U1P1+S1S1P0,HS1U1B13S1U1B0OS1U1P1+S1S1P0,OHS1U1P1-S1S1P0,and solvent HS1U1B12S1U1B0O molecules have been omitted for clarity. )  
-Which of the solutions are buffer solutions?

Accepted Answer

A) (1)and (2) 
B) (1)and (3) 
C) (2)and (3) 
D) (2)and (4) 
A) (1)and (2) 
B) (1)and (3) 
C) (2)and (3) 
D) (2)and (4)

Exam 16: Applications of Aqueous Equilibria

Calculate the molar solubility of thallium(I)chloride in 0.30 M NaCl at 25°C.Ksp for TlCl is 1.7 × 10-4.

A buffer prepared by mixing 55.0 mL of 0.40 M HF with 55.0 mL of 0.40 M NaF will have a pH that is ________ 7.0.

What is the scandium ion concentration for a saturated solution of Sc(OH)3 if the Ksp for Sc(OH)3 is

What is the pH of the resulting solution if 25 mL of 0.432 M methylamine,CH3NH2,is added to 15 mL of 0.234 M HCl? Assume that the volumes of the solutions are additive.Ka = 2.70 × 10-11 for CH3NH3+.

What is the pH of a buffer system made by dissolving 10.70 grams of NH4Cl and 20.00 mL of 12.0 M NH3 in enough water to make 1.000 L of solution? Kb = 1.8 × 10-5 for NH3.

State whether the solubility of Mg(OH)2 will increase or decrease upon the addition of aqueous solutions of a)HCl,b)LiOH,c)NH3.

The following pictures represent solutions that contain a weak acid HA and/or its potassium salt KA.Unshaded spheres represent H atoms and shaded spheres represent A- ions.(K+,H3O+,OH-,and solvent H2O molecules have been omitted for clarity. ) -Which solution has the highest pH?

What is the pH at the equivalence point of a weak base-strong acid titration if 20.00 mL of NaOCl requires 28.30 mL of 0.50 M HCl? Ka = 3.0 × 10-8 for HOCl.

What is the [CH3CO2-]/[CH3CO2H] ratio necessary to make a buffer solution with a pH of 4.44? Ka = 1.8 × 10-5 for CH3CO2H.

Which is a net ionic equation for the neutralization reaction of a weak acid with a weak base?

Calculate the Ksp for silver sulfate if the solubility of Ag2SO4 in pure water is 4.5 g/L.

The balanced net ionic equation for the neutralization reaction involving equal molar amounts of HI and KOH is ________.

The half equivalence point in the titration of 0.100 M CH3NH2 (Kb = 3.7 × 10-4)with 0.250 M HCl occurs at pH = ________.

What is the pH of the solution formed when 25 mL of 0.173 M NaOH is added to 35 mL of 0.342 M HCl?

The pH of a solution of ethylamine,C2H5NH2 (Kb = 6.4 × 10-4)and ethylammium bromide,C2H5NH3Br is 11.00.What is the molarity of C2H5NH3Br if the molarity of C2H5NH2 is 0.025 M?

What is the pH of a solution prepared by mixing 25.00 mL of 0.10 M CH3CO2H with 25.00 mL of 0.040 M CH3CO2Na? Assume that the volume of the solutions are additive and that Ka = 1.8 × 10-5 for CH3CO2H.

What is the equation relating the equilibrium constant Kn for the neutralization of a weak acid with a weak base to the Ka of the acid,the Kb of the base and Kw?

The following pictures represent solutions that contain a weak acid HA and/or its potassium salt KA.Unshaded spheres represent H atoms and shaded spheres represent A- ions.(K+,H3O+,OH-,and solvent H2O molecules have been omitted for clarity. ) -Which of the solutions are buffer solutions?

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Calculate the molar solubility of thallium(I)chloride in 0.30 M NaCl at 25°C.K_sp for TlCl is 1.7 × 10^-4.

What is the scandium ion concentration for a saturated solution of Sc(OH)₃ if the K_sp for Sc(OH)₃ is

What is the pH of the resulting solution if 25 mL of 0.432 M methylamine,CH₃NH₂,is added to 15 mL of 0.234 M HCl? Assume that the volumes of the solutions are additive.K_a = 2.70 × 10^-11 for CH₃NH₃⁺.

What is the pH of a buffer system made by dissolving 10.70 grams of NH₄Cl and 20.00 mL of 12.0 M NH₃ in enough water to make 1.000 L of solution? K_b = 1.8 × 10^-5 for NH₃.

State whether the solubility of Mg(OH)₂ will increase or decrease upon the addition of aqueous solutions of a)HCl,b)LiOH,c)NH₃.

The following pictures represent solutions that contain a weak acid HA and/or its potassium salt KA.Unshaded spheres represent H atoms and shaded spheres represent A^- ions.(K⁺,H₃O⁺,OH^-,and solvent H₂O molecules have been omitted for clarity. ) -Which solution has the highest pH?

What is the pH at the equivalence point of a weak base-strong acid titration if 20.00 mL of NaOCl requires 28.30 mL of 0.50 M HCl? K_a = 3.0 × 10^-8 for HOCl.

What is the [CH₃CO₂^-]/[CH₃CO₂H] ratio necessary to make a buffer solution with a pH of 4.44? K_a = 1.8 × 10^-5 for CH₃CO₂H.

Calculate the K_sp for silver sulfate if the solubility of Ag₂SO₄ in pure water is 4.5 g/L.

The half equivalence point in the titration of 0.100 M CH₃NH₂ (K_b = 3.7 × 10^-4)with 0.250 M HCl occurs at pH = ________.

The pH of a solution of ethylamine,C₂H₅NH₂ (K_b = 6.4 × 10^-4)and ethylammium bromide,C₂H₅NH₃Br is 11.00.What is the molarity of C₂H₅NH₃Br if the molarity of C₂H₅NH₂is 0.025 M?

What is the pH of a solution prepared by mixing 25.00 mL of 0.10 M CH₃CO₂H with 25.00 mL of 0.040 M CH₃CO₂Na? Assume that the volume of the solutions are additive and that K_a = 1.8 × 10^-5 for CH₃CO₂H.

What is the equation relating the equilibrium constant K_n for the neutralization of a weak acid with a weak base to the K_a of the acid,the K_b of the base and K_w?

The following pictures represent solutions that contain a weak acid HA and/or its potassium salt KA.Unshaded spheres represent H atoms and shaded spheres represent A^- ions.(K⁺,H₃O⁺,OH^-,and solvent H₂O molecules have been omitted for clarity. ) -Which of the solutions are buffer solutions?