Question 1

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?

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Question 2

Give the name of the compound that is in antifreeze and is toxic to pets.

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Question 3

Sketch the titration curve for a monoprotic weak acid titrated with a strong base. Make sure to indicate the equivalence point (and whether it is acidic, basic, or neutral)and the buffer region.

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Question 4

Sketch the titration curve for a strong acid titrated with a strong base. Make sure to indicate the equivalence point (and whether the equivalence point is acidic, basic, or neutral)and the buffer region.

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Question 5

Match the following.

-pH > 7
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

Accepted Answer

pH = 7 is the expected pH at the equivalence point of a strong acid-strong base titration.

Question 6

In which of the following solutions would solid PbBr₂ be expected to be the least soluble at 25 °C? A)0.1 mol L^-1 HBr B)0.1 mol L^-1 NaBr C)0.1 mol L^-1 CaBr₂ D)0.1 mol L^-1 KNO₃

Accepted Answer

This question is asking about the solubility of solid PbBr₂ in different solutions. The solubility of a compound generally depends on the interaction between the compound and the solvent molecules. In this case, we can use the principle of common ion effect to predict the solubility of PbBr₂. The principle of common ion effect states that if a compound is dissolved in a solution that already contains one of its ions, the solubility of the compound will decrease. This is because the presence of the ion in solution reduces the concentration gradient and makes it harder for additional solute to dissolve. In the given options, only option C contains a common ion with PbBr₂. CaBr₂ in option C shares the Br- ion with PbBr₂. Therefore, according to the principle of common ion effect, PbBr₂ would be least soluble in option C compared to the other options that do not contain a common ion.

Question 7

Identify the compound that forms stalactites and stalagmites.

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Question 8

Define a buffer.

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Question 9

Match the following. -pH = pK_a2 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

Accepted Answer

At three-quarters of the way to the second equivalence point of a diprotic acid-strong base titration, the pH equals pKa2.

Question 10

Solid potassium chromate (K₂CrO₄)is slowly added to a solution containing 0.50 mol L^-1 AgNO₃ and 0.50 mol L^-1 Ba(NO₃)₂. What is the Ag⁺ concentration when BaCrO₄ just starts to precipitate? The K_sp for Ag₂CrO₄ and BaCrO₄ are 1.1 × 10^-12 and 1.2 × 10^-10, respectively. A)6.5 × 10^-5 mol L^-1 B)1.3 × 10^-4 mol L^-1 C)3.2 × 10^-4 mol L^-1 D)6.8 × 10^-2 mol L^-1

Accepted Answer

BaCrO₄ will precipitate first due to its higher Ksp. When BaCrO₄ starts to precipitate, [CrO₄²⁻] = Ksp / [Ba²⁺] = 1.2 × 10⁻¹⁰ / 0.50 = 2.4 × 10⁻¹⁰ mol L⁻¹. For Ag₂CrO₄, [Ag⁺]² = Ksp / [CrO₄²⁻] = 1.1 × 10⁻¹² / 2.4 × 10⁻¹⁰ = 4.58 × 10⁻³, so [Ag⁺] = √4.58 × 10⁻³ = 6.8 × 10⁻² mol L⁻¹.

Question 11

Sketch the titration curve for a diprotic acid. Make sure to label the equivalence point(s)and the relative amounts of base that were added to reach them.

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Question 12

Match the following.

-pH = 7
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

Accepted Answer

pH = 7 is the expected pH at the equivalence point of a strong acid-strong base titration.

Question 13

What is the molar solubility of AgCl in 0.40 mol L^-1 NH₃? K_sp for AgCl is 1.8 × 10^-10 and K_f for Ag(NH₃)₂⁺ is 1.7 × 10⁷. A)1.3 × 10^-5 mol L^-1 B)2.0 × 10^-5 mol L^-1 C)2.2 × 10^-2 mol L^-1 D)5.5 × 10^-2 mol L^-1

Accepted Answer

The molar solubility of AgCl in NH3 is increased due to the formation of the complex ion Ag(NH3)2+. The overall equilibrium constant for the dissolution and complexation is the product of Ksp and Kf. Solving for the solubility gives approximately 2.2 × 10^-2 mol L^-1.

Question 14

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

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Question 15

What is the molar solubility of AgCl in 0.10 mol L^-1 NaCN if the colourless complex ion Ag(CN)₂^- forms? K_sp for AgCl is 1.8 × 10^-10 and K_f for Ag(CN)₂^- is 1.0 × 10²¹. A)0.050 mol L^-1 B)0.10 mol L^-1 C)0.20 mol L^-1 D)0.40 mol L^-1

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Question 16

Match the following. -pH = pK_a 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

Accepted Answer

At the halfway point to the equivalence point in a weak acid-strong base titration, the concentrations of the weak acid and its conjugate base are equal, making pH = pKa.

Question 17

What is the molar solubility of barium fluoride (BaF₂)in water? The solubility-product constant for BaF₂ is 1.7 × 10^-6 at 25 °C. A)6.5 × 10^-4 mol L^-1 B)1.2 × 10^-2 mol L^-1 C)1.8 × 10^-3 mol L^-1 D)7.5 × 10^-3 mol L^-1 E)5.7 × 10^-7 mol L^-1

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Question 18

A solution of NaF is added dropwise to a solution that is 0.0144 mol L^-1 in Ba²⁺. When the concentration of F^- exceeds ________ mol L^-1, BaF₂ will precipitate. Neglect volume changes. For BaF₂, K_sp = 1.7 × 10^-6. A)5.9 × 10^-5 B)1.1 × 10^-2 C)2.4 × 10^-8 D)2.7 × 10^-3 E)1.2 × 10^-4

Accepted Answer

First, we need to write out the balanced equation for the reaction: Ba²⁺ + 2NaF^- → BaF₂ + Na2^- We can see that we are adding NaF to a solution containing Ba²⁺. The question asks us to find the concentration of F^- needed to precipitate BaF₂. This means that we need to find the concentration at which Qsp (the reaction quotient) equals Ksp, the solubility product constant for BaF₂. At this point, the solution is saturated with BaF₂ and any additional F^- will result in precipitation. The expression for Qsp is: Qsp = [BaF₂][Na2^-]^2 We can assume that the initial concentration of Ba²⁺ is much larger than the amount of NaF added, so we can neglect the change in its concentration. At the beginning of the reaction, there is no BaF₂ precipitate, so we can ignore its concentration in the Qsp expression. That leaves us with: Qsp = [Na2^-]^2[Ksp] Substituting in the values given in the question: Ksp = 1.7 × 10^-6 [NaF^-] = 0.0144 mol L^-1 [Na2^-] = 2 × [NaF^-] = 2 × 0.0144 mol L^-1 = 0.0288 mol L^-1 Plugging in these values: Qsp = (0.0288 mol L^-1)^2 × (1.7 × 10^-6) = 1.39 × 10^-9 Now we just need to find the concentration of NaF^- at which Qsp equals Ksp: Ksp = Qsp [Na2^-]^2[Ksp] = (0.0288 mol L^-1)^2 × (1.7 × 10^-6) [Na2^-]^2 = 1.39 × 10^-3 [Na2^-] = sqrt(1.39 × 10^-3) = 1.18 × 10^-7 Remember that [Na2^-] is twice [NaF^-], so: [NaF^-] = 0.59 × 10^-7 = 5.9 × 10^-6 Therefore, the answer is B) 1.1 × 10^-2.

Question 19

Match the following.

-pH < 7
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

Accepted Answer

pH = 7 is the expected pH at the equivalence point of a strong acid-strong base titration.

Question 20

What is the molar solubility of silver chloride (AgCl)in water? The solubility-product constant for AgCl is 1.8 × 10^-10 at 25 °C. A)9.0 × 10^-11 mol L^-1 B)3.6 × 10^-10 mol L^-1 C)9.74 mol L^-1 D)1.9 × 10^-5 mol L^-1 E)1.3 × 10^-5 mol L^-1

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Quiz 16: Aqueous Ionic Equilibrium

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?

Give the name of the compound that is in antifreeze and is toxic to pets.

Sketch the titration curve for a monoprotic weak acid titrated with a strong base. Make sure to indicate the equivalence point (and whether it is acidic, basic, or neutral)and the buffer region.

Sketch the titration curve for a strong acid titrated with a strong base. Make sure to indicate the equivalence point (and whether the equivalence point is acidic, basic, or neutral)and the buffer region.

Match the following. -pH > 7

In which of the following solutions would solid PbBr₂ be expected to be the least soluble at 25 °C?

Identify the compound that forms stalactites and stalagmites.

Define a buffer.

Match the following. -pH = pK_a2

Solid potassium chromate (K₂CrO₄) is slowly added to a solution containing 0.50 mol L^-1 AgNO₃ and 0.50 mol L^-1 Ba(NO₃) ₂. What is the Ag⁺ concentration when BaCrO₄ just starts to precipitate? The K_sp for Ag₂CrO₄ and BaCrO₄ are 1.1 × 10^-12 and 1.2 × 10^-10, respectively.

Sketch the titration curve for a diprotic acid. Make sure to label the equivalence point(s)and the relative amounts of base that were added to reach them.

Match the following. -pH = 7

What is the molar solubility of AgCl in 0.40 mol L^-1 NH₃? K_sp for AgCl is 1.8 × 10^-10 and K_f for Ag(NH₃) ₂⁺ is 1.7 × 10⁷.

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

What is the molar solubility of AgCl in 0.10 mol L^-1 NaCN if the colourless complex ion Ag(CN) ₂^- forms? K_sp for AgCl is 1.8 × 10^-10 and K_f for Ag(CN) ₂^- is 1.0 × 10²¹.

Match the following. -pH = pK_a

What is the molar solubility of barium fluoride (BaF₂) in water? The solubility-product constant for BaF₂ is 1.7 × 10^-6 at 25 °C.

A solution of NaF is added dropwise to a solution that is 0.0144 mol L^-1 in Ba²⁺. When the concentration of F^- exceeds ________ mol L^-1, BaF₂ will precipitate. Neglect volume changes. For BaF₂, K_sp = 1.7 × 10^-6.

Match the following. -pH < 7

What is the molar solubility of silver chloride (AgCl) in water? The solubility-product constant for AgCl is 1.8 × 10^-10 at 25 °C.

Quiz 16: Aqueous Ionic Equilibrium

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?

Give the name of the compound that is in antifreeze and is toxic to pets.

Sketch the titration curve for a monoprotic weak acid titrated with a strong base. Make sure to indicate the equivalence point (and whether it is acidic, basic, or neutral)and the buffer region.

Sketch the titration curve for a strong acid titrated with a strong base. Make sure to indicate the equivalence point (and whether the equivalence point is acidic, basic, or neutral)and the buffer region.

Match the following. -pH > 7

In which of the following solutions would solid PbBr2 be expected to be the least soluble at 25 °C?

Identify the compound that forms stalactites and stalagmites.

Define a buffer.

Match the following. -pH = pKa2

Solid potassium chromate (K2CrO4) is slowly added to a solution containing 0.50 mol L-1 AgNO3 and 0.50 mol L-1 Ba(NO3) 2. What is the Ag+ concentration when BaCrO4 just starts to precipitate? The Ksp for Ag2CrO4 and BaCrO4 are 1.1 × 10-12 and 1.2 × 10-10, respectively.

Sketch the titration curve for a diprotic acid. Make sure to label the equivalence point(s)and the relative amounts of base that were added to reach them.

Match the following. -pH = 7

What is the molar solubility of AgCl in 0.40 mol L-1 NH3? Ksp for AgCl is 1.8 × 10-10 and Kf for Ag(NH3) 2+ is 1.7 × 107.

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

What is the molar solubility of AgCl in 0.10 mol L-1 NaCN if the colourless complex ion Ag(CN) 2- forms? Ksp for AgCl is 1.8 × 10-10 and Kf for Ag(CN) 2- is 1.0 × 1021.

Match the following. -pH = pKa

What is the molar solubility of barium fluoride (BaF2) in water? The solubility-product constant for BaF2 is 1.7 × 10-6 at 25 °C.

A solution of NaF is added dropwise to a solution that is 0.0144 mol L-1 in Ba2+. When the concentration of F- exceeds ________ mol L-1, BaF2 will precipitate. Neglect volume changes. For BaF2, Ksp = 1.7 × 10-6.

Match the following. -pH < 7

What is the molar solubility of silver chloride (AgCl) in water? The solubility-product constant for AgCl is 1.8 × 10-10 at 25 °C.

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?

In which of the following solutions would solid PbBr₂ be expected to be the least soluble at 25 °C?

Match the following. -pH = pK_a2

Solid potassium chromate (K₂CrO₄) is slowly added to a solution containing 0.50 mol L^-1 AgNO₃ and 0.50 mol L^-1 Ba(NO₃) ₂. What is the Ag⁺ concentration when BaCrO₄ just starts to precipitate? The K_sp for Ag₂CrO₄ and BaCrO₄ are 1.1 × 10^-12 and 1.2 × 10^-10, respectively.

What is the molar solubility of AgCl in 0.40 mol L^-1 NH₃? K_sp for AgCl is 1.8 × 10^-10 and K_f for Ag(NH₃) ₂⁺ is 1.7 × 10⁷.

What is the molar solubility of AgCl in 0.10 mol L^-1 NaCN if the colourless complex ion Ag(CN) ₂^- forms? K_sp for AgCl is 1.8 × 10^-10 and K_f for Ag(CN) ₂^- is 1.0 × 10²¹.

Match the following. -pH = pK_a

What is the molar solubility of barium fluoride (BaF₂) in water? The solubility-product constant for BaF₂ is 1.7 × 10^-6 at 25 °C.

A solution of NaF is added dropwise to a solution that is 0.0144 mol L^-1 in Ba²⁺. When the concentration of F^- exceeds ________ mol L^-1, BaF₂ will precipitate. Neglect volume changes. For BaF₂, K_sp = 1.7 × 10^-6.

What is the molar solubility of silver chloride (AgCl) in water? The solubility-product constant for AgCl is 1.8 × 10^-10 at 25 °C.