Question 1

Which of the following compounds will be more soluble in acidic solution than in pure water?

Accepted Answer

A) PbCl2 
B) FeS 
C) Ca(ClO4)2 
D) CuI 
E) AgBr 
A) PbCl2 
B) FeS 
C) Ca(ClO4)2 
D) CuI 
E) AgBr

Question 2

Define a buffer.

Accepted Answer

Buffers contain significant am

Question 3

Consider the Ksp values for two compounds: MZ, Ksp = 1.5 × 10-20 and MZ2, Ksp = 1.5 × 10-20. Why don't these compounds have the same molar solubility?

Accepted Answer

These two compounds have the same solubi

Question 4

What is the pH of a buffer system prepared by dissolving 10.70 grams of NH4Cl and 25.00 mL of 12 mol L-1 NH3 in enough water to make 1.000 L of solution? Kb = 1.80 × 10-5 for NH3.

Accepted Answer

A) 9.08 
B) 9.26 
C) 9.43 
D) 11.32 
A) 9.08 
B) 9.26 
C) 9.43 
D) 11.32

Question 5

Match the following.

-pH < 7

Accepted Answer

A) equivalence point of a weak base-strong acid titration 
B) equivalence point of a weak acid-strong base titration 
C) three-quarters of the way to second equivalence point of a diprotic acid-strong base titration 
D) halfway to equivalence point of a weak acid-strong base titration 
E) equivalence point of a strong acid-strong base titration 
A) equivalence point of a weak base-strong acid titration 
B) equivalence point of a weak acid-strong base titration 
C) three-quarters of the way to second equivalence point of a diprotic acid-strong base titration 
D) halfway to equivalence point of a weak acid-strong base titration 
E) equivalence point of a strong acid-strong base titration

Question 6

Calculate the pH of a solution formed by mixing 200.0 mL of 0.30 mol L-1 HClO with 300.0 mL of 0.20 mol L-1 KClO. The Ka for HClO is 2.9 × 10-8.

Accepted Answer

A) 5.99 
B) 8.01 
C) 7.54 
D) 7.06 
E) 6.46 
A) 5.99 
B) 8.01 
C) 7.54 
D) 7.06 
E) 6.46

Question 7

Calculate the Ksp for silver sulfite if the solubility of Ag2SO3 in pure water is 4.6 × 10-3 g L-1.

Accepted Answer

A) 3.8 × 10-15 
B) 1.5 × 10-14 
C) 2.4 × 10-10 
D) 4.8 × 10-10 
A) 3.8 × 10-15 
B) 1.5 × 10-14 
C) 2.4 × 10-10 
D) 4.8 × 10-10

Question 8

When titrating a strong monoprotic acid with KOH at 25 °C, the

Accepted Answer

A) pH will be less than 7 at the equivalence point. 
B) pH will be greater than 7 at the equivalence point. 
C) titration will require more moles of base than acid to reach the equivalence point. 
D) pH will be equal to 7 at the equivalence point. 
E) titration will require more moles of acid than base to reach the equivalence point. 
A) pH will be less than 7 at the equivalence point. 
B) pH will be greater than 7 at the equivalence point. 
C) titration will require more moles of base than acid to reach the equivalence point. 
D) pH will be equal to 7 at the equivalence point. 
E) titration will require more moles of acid than base to reach the equivalence point.

Question 9

Determine the molar solubility of AgI in pure water. Ksp (AgI)= 8.51 × 10-17.

Accepted Answer

A) 9.22 × 10-9 mol L-1 
B) 4.26 × 10-17 mol L-1 
C) 8.51 × 10-17 mol L-1 
D) 2.77 × 10-6 mol L-1 
E) 4.40 × 10-6 mol L-1 
A) 9.22 × 10-9 mol L-1 
B) 4.26 × 10-17 mol L-1 
C) 8.51 × 10-17 mol L-1 
D) 2.77 × 10-6 mol L-1 
E) 4.40 × 10-6 mol L-1

Question 10

A 25.0 mL sample of 0.150 mol L-1 hydrofluoric acid is titrated with a 0.150 mol L-1 NaOH solution. What is the pH at the equivalence point? The Ka of hydrofluoric acid is 3.5 × 10-4.

Accepted Answer

A) 10.17 
B) 10.83 
C) 3.17 
D) 7.00 
E) 8.17 
A) 10.17 
B) 10.83 
C) 3.17 
D) 7.00 
E) 8.17

Question 11

Identify the indicator that has two endpoints.

Accepted Answer

A) phenol red 
B) thymol blue 
C) crystal violet 
D) phenolphthalein 
E) alizarin yellow R 
A) phenol red 
B) thymol blue 
C) crystal violet 
D) phenolphthalein 
E) alizarin yellow R

Question 12

How many millilitres of 0.120 mol L-1 NaOH are required to titrate 50.0 mL of 0.0998 mol L-1 butanoic acid to the equivalence point? Butanoic acid is monoprotic. The Ka of butanoic acid is 1.5 × 10-5.

Accepted Answer

A) 4.90 
B) 50.0 
C) 41.6 
D) 60.1 
E) 4.65 
A) 4.90 
B) 50.0 
C) 41.6 
D) 60.1 
E) 4.65

Question 13

Match the following.

-pH = pKa

Accepted Answer

A) equivalence point of a weak base-strong acid titration 
B) equivalence point of a weak acid-strong base titration 
C) three-quarters of the way to second equivalence point of a diprotic acid-strong base titration 
D) halfway to equivalence point of a weak acid-strong base titration 
E) equivalence point of a strong acid-strong base titration 
A) equivalence point of a weak base-strong acid titration 
B) equivalence point of a weak acid-strong base titration 
C) three-quarters of the way to second equivalence point of a diprotic acid-strong base titration 
D) halfway to equivalence point of a weak acid-strong base titration 
E) equivalence point of a strong acid-strong base titration

Question 14

A 100.0 mL sample of 0.20 mol L-1 HF is titrated with 0.10 mol L-1 KOH. Determine the pH of the solution after the addition of 300.0 mL of KOH. The Ka of HF is 3.5 × 10-4.

Accepted Answer

A) 12.40 
B) 9.33 
C) 5.06 
D) 8.94 
E) 12.00 
A) 12.40 
B) 9.33 
C) 5.06 
D) 8.94 
E) 12.00

Question 15

A 1.00 L buffer solution is 0.250 mol L-1 in HF and 0.250 mol L-1 in NaF. Calculate the pH of the solution after the addition of 100.0 mL of 1.00 mol L-1 HCl. The Ka for HF is 3.5 × 10-4.

Accepted Answer

A) 3.09 
B) 4.11 
C) 3.82 
D) 3.46 
E) 2.78 
A) 3.09 
B) 4.11 
C) 3.82 
D) 3.46 
E) 2.78

Question 16

The molar solubility of ZnS is 1.6 × 10-12 mol L-1 in pure water. Calculate the Ksp for ZnS.

Accepted Answer

A) 8.0 × 10-13 
B) 3.2 × 10-12 
C) 1.6 × 10-35 
D) 2.6 × 10-24 
E) 6.8 × 10-5 
A) 8.0 × 10-13 
B) 3.2 × 10-12 
C) 1.6 × 10-35 
D) 2.6 × 10-24 
E) 6.8 × 10-5

Question 17

Match the following.

-pH = pKa2

Accepted Answer

A) equivalence point of a weak base-strong acid titration 
B) equivalence point of a weak acid-strong base titration 
C) three-quarters of the way to second equivalence point of a diprotic acid-strong base titration 
D) halfway to equivalence point of a weak acid-strong base titration 
E) equivalence point of a strong acid-strong base titration 
A) equivalence point of a weak base-strong acid titration 
B) equivalence point of a weak acid-strong base titration 
C) three-quarters of the way to second equivalence point of a diprotic acid-strong base titration 
D) halfway to equivalence point of a weak acid-strong base titration 
E) equivalence point of a strong acid-strong base titration

Question 18

A 100.0 mL sample of 0.20 mol L-1 HF is titrated with 0.10 mol L-1 KOH. Determine the pH of the solution before the addition of any KOH. The Ka of HF is 3.5 × 10-4.

Accepted Answer

A) 4.15 
B) 0.70 
C) 2.08 
D) 3.46 
E) 1.00 
A) 4.15 
B) 0.70 
C) 2.08 
D) 3.46 
E) 1.00

Question 19

Which of the following is TRUE?

Accepted Answer

A) The equivalence point is where the amount of acid equals the amount of base during any acid-base titration. 
B) At the equivalence point, the pH is always 7. 
C) An indicator is not pH sensitive. 
D) A titration curve is a plot of pH vs. the [base]/[acid] ratio. 
E) A titration curve is a plot of pH versus titration time. 
A) The equivalence point is where the amount of acid equals the amount of base during any acid-base titration. 
B) At the equivalence point, the pH is always 7. 
C) An indicator is not pH sensitive. 
D) A titration curve is a plot of pH vs. the [base]/[acid] ratio. 
E) A titration curve is a plot of pH versus titration time.

Question 20

Identify the most commonly used indicator among the following five:

Accepted Answer

A) alizarin 
B) thymol blue 
C) crystal violet 
D) phenolphthalein 
E) alizarin yellow R 
A) alizarin 
B) thymol blue 
C) crystal violet 
D) phenolphthalein 
E) alizarin yellow R

Exam 16: Aqueous Ionic Equilibrium

Which of the following compounds will be more soluble in acidic solution than in pure water?

Define a buffer.

Consider the Ksp values for two compounds: MZ, Ksp = 1.5 × 10-20 and MZ2, Ksp = 1.5 × 10-20. Why don't these compounds have the same molar solubility?

What is the pH of a buffer system prepared by dissolving 10.70 grams of NH4Cl and 25.00 mL of 12 mol L-1 NH3 in enough water to make 1.000 L of solution? Kb = 1.80 × 10-5 for NH3.

Match the following. -pH < 7

Calculate the pH of a solution formed by mixing 200.0 mL of 0.30 mol L-1 HClO with 300.0 mL of 0.20 mol L-1 KClO. The Ka for HClO is 2.9 × 10-8.

Calculate the Ksp for silver sulfite if the solubility of Ag2SO3 in pure water is 4.6 × 10-3 g L-1.

When titrating a strong monoprotic acid with KOH at 25 °C, the

Determine the molar solubility of AgI in pure water. Ksp (AgI)= 8.51 × 10-17.

A 25.0 mL sample of 0.150 mol L-1 hydrofluoric acid is titrated with a 0.150 mol L-1 NaOH solution. What is the pH at the equivalence point? The Ka of hydrofluoric acid is 3.5 × 10-4.

Identify the indicator that has two endpoints.

How many millilitres of 0.120 mol L-1 NaOH are required to titrate 50.0 mL of 0.0998 mol L-1 butanoic acid to the equivalence point? Butanoic acid is monoprotic. The Ka of butanoic acid is 1.5 × 10-5.

Match the following. -pH = pKa

A 100.0 mL sample of 0.20 mol L-1 HF is titrated with 0.10 mol L-1 KOH. Determine the pH of the solution after the addition of 300.0 mL of KOH. The Ka of HF is 3.5 × 10-4.

A 1.00 L buffer solution is 0.250 mol L-1 in HF and 0.250 mol L-1 in NaF. Calculate the pH of the solution after the addition of 100.0 mL of 1.00 mol L-1 HCl. The Ka for HF is 3.5 × 10-4.

The molar solubility of ZnS is 1.6 × 10-12 mol L-1 in pure water. Calculate the Ksp for ZnS.

Match the following. -pH = pKa2

A 100.0 mL sample of 0.20 mol L-1 HF is titrated with 0.10 mol L-1 KOH. Determine the pH of the solution before the addition of any KOH. The Ka of HF is 3.5 × 10-4.

Which of the following is TRUE?

Identify the most commonly used indicator among the following five:

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Chemical Reactions and Stoichiometry

Gases

Thermochemistry

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Filters

Consider the K_sp values for two compounds: MZ, K_sp = 1.5 × 10^-20 and MZ₂, K_sp = 1.5 × 10^-20. Why don't these compounds have the same molar solubility?

What is the pH of a buffer system prepared by dissolving 10.70 grams of NH₄Cl and 25.00 mL of 12 mol L^-1 NH₃ in enough water to make 1.000 L of solution? K_b = 1.80 × 10^-5for NH₃.

Calculate the pH of a solution formed by mixing 200.0 mL of 0.30 mol L^-1 HClO with 300.0 mL of 0.20 mol L^-1 KClO. The K_a for HClO is 2.9 × 10^-8.

Calculate the K_sp for silver sulfite if the solubility of Ag₂SO₃ in pure water is 4.6 × 10^-3g L^-1.

Determine the molar solubility of AgI in pure water. K_sp (AgI)= 8.51 × 10^-17.

A 25.0 mL sample of 0.150 mol L^-1 hydrofluoric acid is titrated with a 0.150 mol L^-1 NaOH solution. What is the pH at the equivalence point? The K_a of hydrofluoric acid is 3.5 × 10^-4.

How many millilitres of 0.120 mol L^-1 NaOH are required to titrate 50.0 mL of 0.0998 mol L^-1 butanoic acid to the equivalence point? Butanoic acid is monoprotic. The K_a of butanoic acid is 1.5 × 10^-5.

Match the following. -pH = pK_a

A 100.0 mL sample of 0.20 mol L^-1 HF is titrated with 0.10 mol L^-1 KOH. Determine the pH of the solution after the addition of 300.0 mL of KOH. The K_a of HF is 3.5 × 10^-4.

A 1.00 L buffer solution is 0.250 mol L^-1 in HF and 0.250 mol L^-1 in NaF. Calculate the pH of the solution after the addition of 100.0 mL of 1.00 mol L^-1 HCl. The K_a for HF is 3.5 × 10^-4.

The molar solubility of ZnS is 1.6 × 10^-12 mol L^-1 in pure water. Calculate the K_sp for ZnS.

Match the following. -pH = pK_a2

A 100.0 mL sample of 0.20 mol L^-1 HF is titrated with 0.10 mol L^-1 KOH. Determine the pH of the solution before the addition of any KOH. The K_a of HF is 3.5 × 10^-4.