Question 1

How many moles of CaF₂ will dissolve in 3.0 L of 0.041 M NaF solution? (K_sp for CaF₂ = 4.0 × 10^-11)

Accepted Answer

Using the equation for the solubility product, we can calculate the amount of CaF₂ that will dissolve in the NaF solution: K_sp = [Ca2+][F-]^2 4.0 × 10^-11 = [CaF₂][2(0.041 M)] [CaF₂] = (4.0 × 10^-11) / (0.082 M) [CaF₂] = 4.88 × 10^-10 mol/L Multiplying the concentration by the volume of the solution: [CaF₂] x 3.0 L = 1.46 × 10^-8 mol Therefore, the answer is C) 7.1 × 10^-8.

Question 2

What is the pH of a saturated solution of Zn(OH)₂? For Zn(OH)₂,K_sp = 2.1 × 10^-16.

Accepted Answer

The answer of What is the pH of a saturated...

Question 3

Which of the following will apply to a saturated solution of an ionic compound?

Accepted Answer

A saturated solution is one in which no more solute can dissolve in the solvent. This means that the concentration of the solute in the solution (Q_c) is at its maximum, and is equal to the solubility product constant (K_sp). Therefore, the correct choice is C, where the concentration of the solute in the solution is equal to the solubility product constant.

Question 4

For which of the following will precipitation be expected?

Accepted Answer

Precipitation is expected when the ion product (Q) of a solution exceeds the solubility product constant (Ksp) of the solute, indicating a supersaturated solution where excess solute will precipitate out.

Question 5

What is the concentration of silver(I)ion in a saturated solution of silver(I)carbonate containing 0.0046 M Na₂CO₃? For Ag₂CO₃,K_sp = 8.6 × 10^-12.

Accepted Answer

The answer of What is the concentration of silver(I)ion in...

Question 6

To 1.0 L of water,1.5 × 10^-6 mol of Pb(NO₃)₂,6.5 × 10^-6 mol of K₂CrO₄,and 1.0 mol of NaCl are added.What will happen? Salt K_sp PbCrO₄ 1)8 × 10^-14 PbCl₂ 1)6 × 10^-5

Accepted Answer

The concentration of Pb²⁺ and CrO₄^2- ions in the solution will exceed the K_sp of PbCrO₄, leading to its precipitation. PbCl₂ will not precipitate because the concentration of Cl^- ions is not high enough to exceed its K_sp.

Question 7

Rank the following salts in order of increasing molar solubility.

Accepted Answer

The answer of Rank the following salts in order of...

Question 8

The solubility of La(IO₃)₃ in a 0.71 M KIO₃ solution is 1.0 ×10^-7 mol/L.Calculate K_sp for La(IO₃)₃.

Accepted Answer

The expression for the solubility product constant (Ksp) of La(IO13)2 in a potassium iodate (KIO3) solution can be written as:

La(IO13)2(s) ⇌ La2+ + 2 IO13-

Ksp = [La2+][IO13-]^2

At equilibrium, the concentration of La(IO13)2(s) is equal to the solubility (S) of La(IO13)2 in the solution. Therefore, the concentration of La2+ and IO13- ions can be expressed in terms of S:

La(IO13)2(s) ⇌ La2+ + 2 IO13-

[S] = [La2+] = (1.0 × 10^-7 mol/L)

[IO13-] = 2[S] = 2(1.0 × 10^-7 mol/L) = 2.0 × 10^-7 mol/L

Substituting these values into the Ksp expression, we get:

Ksp = [La2+][IO13-]^2 = (1.0 × 10^-7 mol/L)(2.0 × 10^-7 mol/L)^2 = 4.0 × 10^-22

The answer in scientific notation is 3.6 × 10^-8, which corresponds to option (D).

Question 9

The insoluble salts AV,B₂W,C₂X₃,DY₂,and EZ₃,which were formed from the metal ions A⁺,B⁺,C³⁺,D²⁺,and E³⁺ and the nonmetals V^1-,W^2-,X^2-,Y^1-,and Z^1-,all have the same K_sp value.Which salt has the highest molar solubility?

Accepted Answer

The answer of The insoluble salts AV,B₂W,C₂X₃,DY₂,and EZ₃,which were formed...

Question 10

K_sp for PbF₂ is 4.0 ×10^-8.If a 0.032 M NaF solution is saturated with PbF₂,what is [Pb²⁺] in solution?

Accepted Answer

The answer of K_sp for PbF₂ is 4.0 ×10^-8.If a...

Question 11

What is the hydroxide-ion concentration of a saturated solution of Ni(OH)₂? For Ni(OH)₂,K_sp = 2.0 × 10^-15.

Accepted Answer

For Ni(OH)₂, Ksp = [Ni²⁺][OH⁻]². Let [Ni²⁺] = s and [OH⁻] = 2s. Ksp = s(2s)² = 4s³. Solving 4s³ = 2.0 × 10⁻¹⁵ gives s = 6.3 × 10⁻⁶ M, so [OH⁻] = 2s = 1.6 × 10⁻⁵ M.

Question 12

Suppose 50.00 mL of 2.0 × 10^-6 M Fe(NO₃)₃ is added to 50.00 mL of 2.0 ×10^-4 M KIO₃.Which of the following statements is true? For Fe(IO₃)₃,K_sp = 1.0 × 10^-14.

Accepted Answer

The answer of Suppose 50.00 mL of 2.0 × 10^-6...

Question 13

What is the molar solubility of MgF₂ in a 0.40 M NaF solution? For MgF₂,K_sp = 8.4 × 10^-8.

Accepted Answer

The answer of What is the molar solubility of MgF₂...

Question 14

Which of Figures I-IV represent(s)the result of mixing aqueous solutions of Na₂S and NiCl₂ in which the ion product Q_c > K_sp for the insoluble product? (C = cation,A = anion)

Accepted Answer

Only Figure III shows the formation of an insoluble product (precipitate), which occurs when the ion product (Q) exceeds the solubility product (Ksp). Figures I and II show no reaction or the formation of a clear solution, indicating the absence of a precipitate. Figure IV shows the formation of a colored complex, which is different from the formation of an insoluble product. Therefore, the correct answer is D) only III.

Question 15

Which Figures I-IV represent(s)the result of mixing aqueous solutions of NaOH and CuCl₂ in which the ion product Q_c > K_sp for the insoluble product? (C = cation,A = anion)

Accepted Answer

The answer of Which Figures I-IV represent(s)the result of mixing...

Question 16

The figure below represents the result of adding which of the following aqueous solutions to a filtered,saturated solution of AgCl?

Accepted Answer

The answer of The figure below represents the result of...

Question 17

In which of these solutions would silver(I)carbonate have the lowest molar solubility? For silver(I)carbonate,K_sp = 8.5 × 10^-12.

Accepted Answer

The presence of a common ion (Ag+) in 0.1 M AgNO3 will significantly reduce the solubility of silver(I)carbonate due to the common ion effect, making it the solution in which silver(I)carbonate has the lowest molar solubility.

Question 18

Which salt has the lowest molar solubility in pure water?

Accepted Answer

The solubility of a salt depends on its Ksp (solubility product constant), which is a measure of the concentration of ions in a saturated solution. Generally, the lower the Ksp, the lower the solubility of the salt. In the given options, PbCrO4 has the lowest Ksp value (1.8 x 10^-14). This means that PbCrO4 has the lowest molar solubility in pure water.

Question 19

In which of the following solutions would silver(I)phosphate,Ag₃PO₄,be least soluble?

Accepted Answer

Silver(I) phosphate, Ag3PO4, would be least soluble in a solution of 0.10 M AgNO3 because the common ion effect would cause it to precipitate more readily due to the presence of Ag+ ions from AgNO3.

Question 20

What is the molar solubility of MgF₂ in a 0.36 M Mg(NO₃)₂ solution? For MgF₂,K_sp = 8.4 × 10^-8.

Accepted Answer

First, write the balanced equation for the dissolution of MgFS1U1B12S1U1B0:

MgFS1U1B12S1U1B0(s) ⇌ MgS1U1B12S1U1B0+(aq) + FS1U1B1-(aq)

The equilibrium expression for this reaction can be written as:

KS1U1B1spS1U1B0 = [MgS1U1B12S1U1B0+][FS1U1B1-]

We are given that KS1U1B1spS1U1B0 = 8.4 × 10S1U1P1-8S1S1P0. Let x be the molar solubility of MgFS1U1B12S1U1B0 in the solution. Then, at equilibrium:

[MgS1U1B12S1U1B0+] = x
[FS1U1B1-] = x

We can then substitute these values into the equilibrium expression:

KS1U1B1spS1U1B0 = x^2

Solving for x, we get:

x = √(KS1U1B1spS1U1B0) = √(8.4 × 10S1U1P1-8S1S1P0) = 2.4 × 10S1U1P1-4S1S1P0 M

Therefore, the answer is B, 2.4 × 10S1U1P1-4S1S1P0 M.

Quiz 17: Solubility and Complex-Ion Equilibria

How many moles of CaF₂ will dissolve in 3.0 L of 0.041 M NaF solution? (K_sp for CaF₂ = 4.0 × 10^-11)

What is the pH of a saturated solution of Zn(OH) ₂? For Zn(OH) ₂,K_sp = 2.1 × 10^-16.

Which of the following will apply to a saturated solution of an ionic compound?

For which of the following will precipitation be expected?

What is the concentration of silver(I) ion in a saturated solution of silver(I) carbonate containing 0.0046 M Na₂CO₃? For Ag₂CO₃,K_sp = 8.6 × 10^-12.

To 1.0 L of water,1.5 × 10^-6 mol of Pb(NO₃) ₂,6.5 × 10^-6 mol of K₂CrO₄,and 1.0 mol of NaCl are added.What will happen? Salt K_sp PbCrO₄ 1) 8 × 10^-14 PbCl₂ 1) 6 × 10^-5

Rank the following salts in order of increasing molar solubility.

The solubility of La(IO₃) ₃ in a 0.71 M KIO₃ solution is 1.0 ×10^-7 mol/L.Calculate K_sp for La(IO₃) ₃.

The insoluble salts AV,B₂W,C₂X₃,DY₂,and EZ₃,which were formed from the metal ions A⁺,B⁺,C³⁺,D²⁺,and E³⁺ and the nonmetals V^1-,W^2-,X^2-,Y^1-,and Z^1-,all have the same K_sp value.Which salt has the highest molar solubility?

K_sp for PbF₂ is 4.0 ×10^-8.If a 0.032 M NaF solution is saturated with PbF₂,what is [Pb²⁺] in solution?

What is the hydroxide-ion concentration of a saturated solution of Ni(OH) ₂? For Ni(OH) ₂,K_sp = 2.0 × 10^-15.

Suppose 50.00 mL of 2.0 × 10^-6 M Fe(NO₃) ₃ is added to 50.00 mL of 2.0 ×10^-4 M KIO₃.Which of the following statements is true? For Fe(IO₃) ₃,K_sp = 1.0 × 10^-14.

What is the molar solubility of MgF₂ in a 0.40 M NaF solution? For MgF₂,K_sp = 8.4 × 10^-8.

Which of Figures I-IV represent(s) the result of mixing aqueous solutions of Na₂S and NiCl₂ in which the ion product Q_c > K_sp for the insoluble product? (C = cation,A = anion)

Which Figures I-IV represent(s) the result of mixing aqueous solutions of NaOH and CuCl₂ in which the ion product Q_c > K_sp for the insoluble product? (C = cation,A = anion)

The figure below represents the result of adding which of the following aqueous solutions to a filtered,saturated solution of AgCl?

In which of these solutions would silver(I) carbonate have the lowest molar solubility? For silver(I) carbonate,K_sp = 8.5 × 10^-12.

Which salt has the lowest molar solubility in pure water?

In which of the following solutions would silver(I) phosphate,Ag₃PO₄,be least soluble?

What is the molar solubility of MgF₂ in a 0.36 M Mg(NO₃) ₂ solution? For MgF₂,K_sp = 8.4 × 10^-8.

Quiz 17: Solubility and Complex-Ion Equilibria

How many moles of CaF2 will dissolve in 3.0 L of 0.041 M NaF solution? (Ksp for CaF2 = 4.0 × 10-11)

What is the pH of a saturated solution of Zn(OH) 2? For Zn(OH) 2,Ksp = 2.1 × 10-16.

Which of the following will apply to a saturated solution of an ionic compound?

For which of the following will precipitation be expected?

What is the concentration of silver(I) ion in a saturated solution of silver(I) carbonate containing 0.0046 M Na2CO3? For Ag2CO3,Ksp = 8.6 × 10-12.

To 1.0 L of water,1.5 × 10-6 mol of Pb(NO3) 2,6.5 × 10-6 mol of K2CrO4,and 1.0 mol of NaCl are added.What will happen? Salt Ksp PbCrO4 1) 8 × 10-14 PbCl2 1) 6 × 10-5

Rank the following salts in order of increasing molar solubility.

The solubility of La(IO3) 3 in a 0.71 M KIO3 solution is 1.0 ×10-7 mol/L.Calculate Ksp for La(IO3) 3.

The insoluble salts AV,B2W,C2X3,DY2,and EZ3,which were formed from the metal ions A+,B+,C3+,D2+,and E3+ and the nonmetals V1-,W2-,X2-,Y1-,and Z1-,all have the same Ksp value.Which salt has the highest molar solubility?

Ksp for PbF2 is 4.0 ×10-8.If a 0.032 M NaF solution is saturated with PbF2,what is [Pb2+] in solution?

What is the hydroxide-ion concentration of a saturated solution of Ni(OH) 2? For Ni(OH) 2,Ksp = 2.0 × 10-15.

Suppose 50.00 mL of 2.0 × 10-6 M Fe(NO3) 3 is added to 50.00 mL of 2.0 ×10-4 M KIO3.Which of the following statements is true? For Fe(IO3) 3,Ksp = 1.0 × 10-14.

What is the molar solubility of MgF2 in a 0.40 M NaF solution? For MgF2,Ksp = 8.4 × 10-8.

Which of Figures I-IV represent(s) the result of mixing aqueous solutions of Na2S and NiCl2 in which the ion product Qc > Ksp for the insoluble product? (C = cation,A = anion)

Which Figures I-IV represent(s) the result of mixing aqueous solutions of NaOH and CuCl2 in which the ion product Qc > Ksp for the insoluble product? (C = cation,A = anion)

The figure below represents the result of adding which of the following aqueous solutions to a filtered,saturated solution of AgCl?

In which of these solutions would silver(I) carbonate have the lowest molar solubility? For silver(I) carbonate,Ksp = 8.5 × 10-12.

Which salt has the lowest molar solubility in pure water?

In which of the following solutions would silver(I) phosphate,Ag3PO4,be least soluble?

What is the molar solubility of MgF2 in a 0.36 M Mg(NO3) 2 solution? For MgF2,Ksp = 8.4 × 10-8.

How many moles of CaF₂ will dissolve in 3.0 L of 0.041 M NaF solution? (K_sp for CaF₂ = 4.0 × 10^-11)

What is the pH of a saturated solution of Zn(OH) ₂? For Zn(OH) ₂,K_sp = 2.1 × 10^-16.

What is the concentration of silver(I) ion in a saturated solution of silver(I) carbonate containing 0.0046 M Na₂CO₃? For Ag₂CO₃,K_sp = 8.6 × 10^-12.

To 1.0 L of water,1.5 × 10^-6 mol of Pb(NO₃) ₂,6.5 × 10^-6 mol of K₂CrO₄,and 1.0 mol of NaCl are added.What will happen? Salt K_sp PbCrO₄ 1) 8 × 10^-14 PbCl₂ 1) 6 × 10^-5

The solubility of La(IO₃) ₃ in a 0.71 M KIO₃ solution is 1.0 ×10^-7 mol/L.Calculate K_sp for La(IO₃) ₃.

The insoluble salts AV,B₂W,C₂X₃,DY₂,and EZ₃,which were formed from the metal ions A⁺,B⁺,C³⁺,D²⁺,and E³⁺ and the nonmetals V^1-,W^2-,X^2-,Y^1-,and Z^1-,all have the same K_sp value.Which salt has the highest molar solubility?

K_sp for PbF₂ is 4.0 ×10^-8.If a 0.032 M NaF solution is saturated with PbF₂,what is [Pb²⁺] in solution?

What is the hydroxide-ion concentration of a saturated solution of Ni(OH) ₂? For Ni(OH) ₂,K_sp = 2.0 × 10^-15.

Suppose 50.00 mL of 2.0 × 10^-6 M Fe(NO₃) ₃ is added to 50.00 mL of 2.0 ×10^-4 M KIO₃.Which of the following statements is true? For Fe(IO₃) ₃,K_sp = 1.0 × 10^-14.

What is the molar solubility of MgF₂ in a 0.40 M NaF solution? For MgF₂,K_sp = 8.4 × 10^-8.

Which of Figures I-IV represent(s) the result of mixing aqueous solutions of Na₂S and NiCl₂ in which the ion product Q_c > K_sp for the insoluble product? (C = cation,A = anion)

Which Figures I-IV represent(s) the result of mixing aqueous solutions of NaOH and CuCl₂ in which the ion product Q_c > K_sp for the insoluble product? (C = cation,A = anion)

In which of these solutions would silver(I) carbonate have the lowest molar solubility? For silver(I) carbonate,K_sp = 8.5 × 10^-12.

In which of the following solutions would silver(I) phosphate,Ag₃PO₄,be least soluble?

What is the molar solubility of MgF₂ in a 0.36 M Mg(NO₃) ₂ solution? For MgF₂,K_sp = 8.4 × 10^-8.