Question 1

When 100 mL each of 2.0 × 10^-6 M Ag+ and 2.0 × 10^-3 M Br- are mixed, what is the remaining Ag+ ion concentration and is precipitation complete? The solubility product constant of AgBr is 5.0 × 10^-13.

Accepted Answer

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Question 2

What is the free Ag⁺ concentration of 0.020 M Ag⁺ solution mixed with an equal volume of 2.0 M NH₃? Kf for [Ag(NH₃)₂]⁺ is 1.6 × 10⁷.

Accepted Answer

First, let's write the balanced equilibrium equation for the complex formation: Ag⁺ + [NH₃] -> [Ag(NH₃)₂]⁺ The equilibrium constant expression is: K = [Ag(NH₃)₂]⁺ / ([Ag⁺] * [NH₃]) We are given that Kf = 1.6 × 10⁷. We can use an ICE table to solve for the concentration of free Ag⁺ after mixing: Initial: 0.020 M 2.0 M Ag⁺ NH₃ Change: -x -x -x -x Equilibrium: 0.020 - x 2.0 - x We can assume that x is very small compared to the initial concentrations, so we can approximate 0.020 - x as 0.020 and 2.0 - x as 2.0. Substituting the equilibrium concentrations into the equilibrium constant expression, we get: 1.6 × 10⁷ = [Ag(NH₃)₂]⁺ / (0.020 * 2.0) Solving for [Ag(NH₃)₂]⁺, we get: [Ag(NH₃)₂]⁺ = 0.020 * 2.0 * 1.6 × 10⁷ = 6.4 × 10^-8 Therefore, the concentration of free Ag⁺ is: [Ag⁺] = 0.020 - [Ag(NH₃)₂]⁺ = 0.020 - 6.4 × 10^-8 = 6.5 × 10^-10 Therefore, the correct answer is D: 6.5 × 10^-10.

Question 3

When equal volumes of the indicated solutions are mixed, precipitation should occur only for: barium fluoride 1.0 × 10^-6 calcium carbonate 2.8 × 10^-9 Calcium fluoride 5.3 × 10^-9 Magnesium fluoride 3.7 × 10^-9 Silver carbonate 8.5 × 10-12

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The answer of When equal volumes of the indicated solutions...

Question 4

If iron(III) acetate is added to be 1 × 10^-10 M in a solution that is 0.10 M NH₃, what is Qsp and will Fe(OH)₃ precipitate? The Ksp of Fe(OH)₃ is 4 × 10^-38 and Kb for NH₃ is 1.8 × 10^-5.

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The answer of If iron(III) acetate is added to be...

Question 5

In which of the following one molar solutions would you expect cadmium sulfide, CdS, to be the most soluble?

Accepted Answer

Cadmium sulfide (CdS) is more soluble in acidic solutions. HCl provides an acidic environment, which increases the solubility of CdS by shifting the equilibrium towards dissolution.

Question 6

When 100 mL each of 2.0 × 10^-4 M Ca²⁺ and 2.0 × 10^-2M F- are mixed, what is the remaining Ca²⁺ ion concentration and is precipitation complete? The solubility product constant of CaF₂ is 5.3 × 10^-9.

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The answer of When 100 mL each of 2.0 ×...

Question 7

What is the approximate concentration of free Fe³⁺ ion in a solution prepared by mixing equal volumes of 0.06 M Fe³⁺ and 4.0 M F- solutions? [The net formation constant for FeF₅(H₂O)₂^- is 2.0 × 10¹⁵.]

Accepted Answer

The formation of FeF5(H2O)2- complex ion decreases the free Fe3+ ion concentration. The equilibrium constant expression for the formation of the complex ion is:Kf = [FeF5(H2O)2-] / [Fe3+][F-]5Substituting the given values into the expression, we get:2.0 × 10^15 = [FeF5(H2O)2-] / [Fe3+][4.0]^5Assuming that the initial concentration of Fe3+ is 0.03 M (since equal volumes of 0.06 M Fe3+ and 4.0 M F- solutions are mixed), we can solve for the concentration of free Fe3+ ion:[Fe3+] = [FeF5(H2O)2-] / (2.0 × 10^15 * [4.0]^5)[Fe3+] = 6.9 × 10^-19 M

Question 8

To a saturated solution of barium carbonate is added just enough sodium sulfate to achieve a maximum sulfate concentration without precipitation of barium sulfate. If no complexes form and the "salt effect" is negligible, what is the concentration of the sulfate ion in this solution? [Ksp for barium carbonate is 1.6 × 10^-9; Ksp for barium sulfate is 7.9 × 10^-11]

Accepted Answer

The answer of To a saturated solution of barium carbonate...

Question 9

Consider an aqueous solution which is 0.020 M in Pb2+ and 0.20 M in Ag+. Concentrated potassium iodide solution (so that volume changes may be neglected) is added gradually with good stirring to this solution. Eventually the iodide ion concentration should increase enough to cause precipitation of the second ion. What will be the concentration of the ion that precipitates first when the second ion just begins to precipitate?

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Question 10

If chromium(III) chloride is added to be 1 × 10^-12 M in a solution that is 0.10 M NH₃, what is Qsp and will Cr(OH)₃ precipitate? The Ksp of Cr(OH)₃ is 6.3 × 10^-31 and Kb for NH₃ is 1.8 × 10^-5.

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Question 11

The solubility product constant of Mg(OH)₂ is 9.0 × 10^-12. If a solution is 0.010 M with respect to Mg²⁺ ion, the amount of [OH-] required to start the precipitation of Mg(OH)₂ is:

Accepted Answer

The answer of The solubility product constant of Mg(OH)₂ is...

Question 12

When 100 mL each of 2.0 × 10^-4 M Ag⁺ and 2.0 × 10-1 M CO₃^2- are mixed, what is the remaining Ag⁺ ion concentration and is precipitation complete? The solubility product constant of Ag₂CO₃ is 8.5 × 10^-12.

Accepted Answer

The answer of When 100 mL each of 2.0 ×...

Question 13

When 100 mL each of 2.0 × 10^-5 M Ca²⁺ and 2.0 × 10^-3M CO₃^2- are mixed, what is the remaining Ca²⁺ ion concentration and is precipitation complete? The solubility product constant of CaCO₃ is 2.8 × 10^-9.

Accepted Answer

The ion product Q = [Ca²⁺][CO₃^2-] = (1.0 × 10^-5)(1.0 × 10^-3) = 1.0 × 10^-8, which is greater than K_sp (2.8 × 10^-9), so precipitation occurs. The remaining [Ca²⁺] is calculated using the K_sp value, resulting in 2.8 × 10^-6 M, but precipitation is not complete.

Question 14

What is the concentration of free Zn²⁺ if 0.020 M Zn²+ solution is mixed with an equal volume of 2.0 M NH₃? Kf for [Zn(NH₃)₄]²⁺ is 4.1 × 10⁸.

Accepted Answer

First, we need to write the balanced equation for the reaction between ZnS and NHS:

ZnS + 2NHS → [Zn(NHS)2] + H2S

The equilibrium constant for this reaction can be written as:

Kf = [Zn(NHS)2][H2S] / [ZnS][NHS]^2

We are given that Kf = 4.1 × 10^-18 and [ZnS] = 0.020 M. We also know that the volume of the NHS solution added is equal to the volume of the ZnS solution, so the final concentration of NHS is 1.0 M.

Let x be the concentration of free ZnS in the solution after the reaction reaches equilibrium.

At equilibrium, the concentration of [Zn(NHS)2] and [H2S] are both equal to x, while the concentration of [NHS] is 1.0 - x.

Substituting these values into the equilibrium constant expression and solving for x, we get:

4.1 × 10^-18 = x^2 / (0.020 - x)^2

x = 2.88 × 10^-11 M

Therefore, the concentration of free ZnS in the solution is 2.88 × 10^-11 M. The closest choice is B, which is the correct answer.

Question 15

A homeowner in Boston becomes concerned that there may be appreciable amounts of lead in her drinking water due to 150-year old water pipes in her house. Consequently, she takes a sample of her drinking water in to be analyzed. The laboratory technician, who is new on the job, has been told to analyze by precipitating the lead ion as the iodide (Ksp = 7.1 × 10^-9 for PbI2) by slowly adding small portions of 1.00 M NaI solution. If we assume that the concentration of lead in the solution is 1.00 mg/liter or approximately 4.8 × 10-6 M (this would be 1.0 part per million) is it possible to detect the lead in the drinking water by adding a total of no more than 10.0 mL of NaI solution to a 100 mL sample of drinking water? You must of course consider dilution effects. What is Q?

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The answer of A homeowner in Boston becomes concerned that...

Question 16

When equal volumes of the indicated solutions are mixed, precipitation should occur only for: barium fluoride 1.0 × 10^-6 calcium carbonate 2.8 × 10^-9 Calcium fluoride 5.3 × 10^-9 Magnesium fluoride 3.7 × 10^-8 Silver carbonate 8.5 × 10^-12

Accepted Answer

The answer of When equal volumes of the indicated solutions...

Question 17

A solution contains [Ba²⁺] = 5.0 × 10^-5 M, [Ag⁺] = 3.0 × 10^-5 M, and [Zn²⁺] = 2.0 × 10^-7 M. Sodium oxalate is slowly added so that [C₂O₄^2-] increases. What is the concentration of the first cation to precipitate when the second cation just begins to precipitate?

Accepted Answer

The first cation to precipitate will be the one with the lowest Ksp value. We can calculate the Ksp values using the given concentrations:

Ksp BaSO4 = [BaS1U1P12+S1S1P0][CS1U1B12S1U1B0OS1U1B14S1U1B0S1U1P12-S1S1P0] = (5.0 × 10^-5)(x)

Ksp Ag2Ox = [AgS1U1P1+S1S1P0][CS1U1B12S1U1B0OS1U1B14S1U1B0S1S1P0]^2 = (3.0 × 10^-5)(x^2)

Ksp ZnC2O4 = [ZnS1U1P12+S1S1P0][CS1U1B12S1U1B0OS1U1B14S1U1B0S1U1P12-S1S1P0] = (2.0 × 10^-7)(x)

where x is the concentration of sodium oxalate.

At the point where the second cation just begins to precipitate, the concentration of the ion with the higher Ksp value will reach its solubility product. So we can set the Ksp expression for Ag2Ox equal to its Ksp value and solve for x:

Ksp Ag2Ox = (3.0 × 10^-5)(x^2) = 5.5 × 10^-13

x = 2.2 × 10^-6 M

Now we can calculate the ion concentrations at this point:

[BaS1U1P12+S1S1P0] = (5.0 × 10^-5)(2.2 × 10^-6) / (1.5 × 10^-12) = 7.3 × 10^-3 M

[AgS1U1P1+S1S1P0] = 3.0 × 10^-5 M

[ZnS1U1P12+S1S1P0] = (2.0 × 10^-7)(2.2 × 10^-6) / (1.5 × 10^-12) = 2.9 × 10^-2 M

Therefore, the first cation to precipitate is Ba2+ and its concentration at this point is 7.3 × 10^-3 M, which is closest to choice B: 2.2 × 10^-6.

Question 18

To a concentrated buffer of pH 9.0 was added an equal volume of a solution that was 0.20 M in each of the ions Ca²⁺, Cd²⁺, and Cu²⁺. The expected precipitate would consist of: salt: calcium hydroxide cadmium hydroxide copper(II) hydroxide Ksp: 4.0 × 10^-6 2.0 × 10^-14 1.8 × 10^-19

Accepted Answer

The answer of To a concentrated buffer of pH 9.0...

Question 19

In which of the following solutions will the concentration of dissolved silver species be the highest if solid AgNO₃ is stirred with 1.00 L of solution?

Accepted Answer

Ammonia (NH₃) forms a complex ion with silver ions, increasing the solubility of AgNO₃ in the solution.

Question 20

What is the free Cu²⁺ concentration if 0.020 M Cu²⁺ solution is mixed with an equal volume of 4.0 M NH₃? Kf for [Cu(NH₃)₄]²⁺ is 1.1 × 10¹³.

Accepted Answer

The answer of What is the free Cu²⁺ concentration if...

Quiz 18: Solubility and Complex-Ion Equilibria

When 100 mL each of 2.0 × 10^-6 M Ag+ and 2.0 × 10^-3 M Br- are mixed, what is the remaining Ag+ ion concentration and is precipitation complete? The solubility product constant of AgBr is 5.0 × 10^-13.

What is the free Ag⁺ concentration of 0.020 M Ag⁺ solution mixed with an equal volume of 2.0 M NH₃? Kf for [Ag(NH₃) ₂]⁺ is 1.6 × 10⁷.

When equal volumes of the indicated solutions are mixed, precipitation should occur only for: barium fluoride 1.0 × 10^-6 calcium carbonate 2.8 × 10^-9 Calcium fluoride 5.3 × 10^-9 Magnesium fluoride 3.7 × 10^-9 Silver carbonate 8.5 × 10-12

If iron(III) acetate is added to be 1 × 10^-10 M in a solution that is 0.10 M NH₃, what is Qsp and will Fe(OH) ₃ precipitate? The Ksp of Fe(OH) ₃ is 4 × 10^-38 and Kb for NH₃ is 1.8 × 10^-5.

In which of the following one molar solutions would you expect cadmium sulfide, CdS, to be the most soluble?

When 100 mL each of 2.0 × 10^-4 M Ca²⁺ and 2.0 × 10^-2M F- are mixed, what is the remaining Ca²⁺ ion concentration and is precipitation complete? The solubility product constant of CaF₂ is 5.3 × 10^-9.

What is the approximate concentration of free Fe³⁺ ion in a solution prepared by mixing equal volumes of 0.06 M Fe³⁺ and 4.0 M F- solutions? [The net formation constant for FeF₅(H₂O) ₂^- is 2.0 × 10¹⁵.]

If chromium(III) chloride is added to be 1 × 10^-12 M in a solution that is 0.10 M NH₃, what is Qsp and will Cr(OH) ₃ precipitate? The Ksp of Cr(OH) ₃ is 6.3 × 10^-31 and Kb for NH₃ is 1.8 × 10^-5.

The solubility product constant of Mg(OH) ₂ is 9.0 × 10^-12. If a solution is 0.010 M with respect to Mg²⁺ ion, the amount of [OH-] required to start the precipitation of Mg(OH) ₂ is:

When 100 mL each of 2.0 × 10^-4 M Ag⁺ and 2.0 × 10-1 M CO₃^2- are mixed, what is the remaining Ag⁺ ion concentration and is precipitation complete? The solubility product constant of Ag₂CO₃ is 8.5 × 10^-12.

When 100 mL each of 2.0 × 10^-5 M Ca²⁺ and 2.0 × 10^-3M CO₃^2- are mixed, what is the remaining Ca²⁺ ion concentration and is precipitation complete? The solubility product constant of CaCO₃ is 2.8 × 10^-9.

What is the concentration of free Zn²⁺ if 0.020 M Zn²+ solution is mixed with an equal volume of 2.0 M NH₃? Kf for [Zn(NH₃) ₄]²⁺ is 4.1 × 10⁸.

When equal volumes of the indicated solutions are mixed, precipitation should occur only for: barium fluoride 1.0 × 10^-6 calcium carbonate 2.8 × 10^-9 Calcium fluoride 5.3 × 10^-9 Magnesium fluoride 3.7 × 10^-8 Silver carbonate 8.5 × 10^-12

A solution contains [Ba²⁺] = 5.0 × 10^-5 M, [Ag⁺] = 3.0 × 10^-5 M, and [Zn²⁺] = 2.0 × 10^-7 M. Sodium oxalate is slowly added so that [C₂O₄^2-] increases. What is the concentration of the first cation to precipitate when the second cation just begins to precipitate?

To a concentrated buffer of pH 9.0 was added an equal volume of a solution that was 0.20 M in each of the ions Ca²⁺, Cd²⁺, and Cu²⁺. The expected precipitate would consist of: salt: calcium hydroxide cadmium hydroxide copper(II) hydroxide Ksp: 4.0 × 10^-6 2.0 × 10^-14 1.8 × 10^-19

In which of the following solutions will the concentration of dissolved silver species be the highest if solid AgNO₃ is stirred with 1.00 L of solution?

What is the free Cu²⁺ concentration if 0.020 M Cu²⁺ solution is mixed with an equal volume of 4.0 M NH₃? Kf for [Cu(NH₃) ₄]²⁺ is 1.1 × 10¹³.

Quiz 18: Solubility and Complex-Ion Equilibria

When 100 mL each of 2.0 × 10-6 M Ag+ and 2.0 × 10-3 M Br- are mixed, what is the remaining Ag+ ion concentration and is precipitation complete? The solubility product constant of AgBr is 5.0 × 10-13.

What is the free Ag+ concentration of 0.020 M Ag+ solution mixed with an equal volume of 2.0 M NH3? Kf for [Ag(NH3) 2]+ is 1.6 × 107.

When equal volumes of the indicated solutions are mixed, precipitation should occur only for: barium fluoride 1.0 × 10-6 calcium carbonate 2.8 × 10-9 Calcium fluoride 5.3 × 10-9 Magnesium fluoride 3.7 × 10-9 Silver carbonate 8.5 × 10-12

If iron(III) acetate is added to be 1 × 10-10 M in a solution that is 0.10 M NH3, what is Qsp and will Fe(OH) 3 precipitate? The Ksp of Fe(OH) 3 is 4 × 10-38 and Kb for NH3 is 1.8 × 10-5.

In which of the following one molar solutions would you expect cadmium sulfide, CdS, to be the most soluble?

When 100 mL each of 2.0 × 10-4 M Ca2+ and 2.0 × 10-2 M F- are mixed, what is the remaining Ca2+ ion concentration and is precipitation complete? The solubility product constant of CaF2 is 5.3 × 10-9.

What is the approximate concentration of free Fe3+ ion in a solution prepared by mixing equal volumes of 0.06 M Fe3+ and 4.0 M F- solutions? [The net formation constant for FeF5(H2O) 2- is 2.0 × 1015.]

If chromium(III) chloride is added to be 1 × 10-12 M in a solution that is 0.10 M NH3, what is Qsp and will Cr(OH) 3 precipitate? The Ksp of Cr(OH) 3 is 6.3 × 10-31 and Kb for NH3 is 1.8 × 10-5.

The solubility product constant of Mg(OH) 2 is 9.0 × 10-12. If a solution is 0.010 M with respect to Mg2+ ion, the amount of [OH-] required to start the precipitation of Mg(OH) 2 is:

When 100 mL each of 2.0 × 10-4 M Ag+ and 2.0 × 10-1 M CO32- are mixed, what is the remaining Ag+ ion concentration and is precipitation complete? The solubility product constant of Ag2CO3 is 8.5 × 10-12.

When 100 mL each of 2.0 × 10-5 M Ca2+ and 2.0 × 10-3 M CO32- are mixed, what is the remaining Ca2+ ion concentration and is precipitation complete? The solubility product constant of CaCO3 is 2.8 × 10-9.

What is the concentration of free Zn2+ if 0.020 M Zn2+ solution is mixed with an equal volume of 2.0 M NH3? Kf for [Zn(NH3) 4]2+ is 4.1 × 108.

When equal volumes of the indicated solutions are mixed, precipitation should occur only for: barium fluoride 1.0 × 10-6 calcium carbonate 2.8 × 10-9 Calcium fluoride 5.3 × 10-9 Magnesium fluoride 3.7 × 10-8 Silver carbonate 8.5 × 10-12

A solution contains [Ba2+] = 5.0 × 10-5 M, [Ag+] = 3.0 × 10-5 M, and [Zn2+] = 2.0 × 10-7 M. Sodium oxalate is slowly added so that [C2O42-] increases. What is the concentration of the first cation to precipitate when the second cation just begins to precipitate?

To a concentrated buffer of pH 9.0 was added an equal volume of a solution that was 0.20 M in each of the ions Ca2+, Cd2+, and Cu2+. The expected precipitate would consist of: salt: calcium hydroxide cadmium hydroxide copper(II) hydroxide Ksp: 4.0 × 10-6 2.0 × 10-14 1.8 × 10-19

In which of the following solutions will the concentration of dissolved silver species be the highest if solid AgNO3 is stirred with 1.00 L of solution?

What is the free Cu2+ concentration if 0.020 M Cu2+ solution is mixed with an equal volume of 4.0 M NH3? Kf for [Cu(NH3) 4]2+ is 1.1 × 1013.

When 100 mL each of 2.0 × 10^-6 M Ag+ and 2.0 × 10^-3 M Br- are mixed, what is the remaining Ag+ ion concentration and is precipitation complete? The solubility product constant of AgBr is 5.0 × 10^-13.

What is the free Ag⁺ concentration of 0.020 M Ag⁺ solution mixed with an equal volume of 2.0 M NH₃? Kf for [Ag(NH₃) ₂]⁺ is 1.6 × 10⁷.

When equal volumes of the indicated solutions are mixed, precipitation should occur only for: barium fluoride 1.0 × 10^-6 calcium carbonate 2.8 × 10^-9 Calcium fluoride 5.3 × 10^-9 Magnesium fluoride 3.7 × 10^-9 Silver carbonate 8.5 × 10-12

If iron(III) acetate is added to be 1 × 10^-10 M in a solution that is 0.10 M NH₃, what is Qsp and will Fe(OH) ₃ precipitate? The Ksp of Fe(OH) ₃ is 4 × 10^-38 and Kb for NH₃ is 1.8 × 10^-5.

When 100 mL each of 2.0 × 10^-4 M Ca²⁺ and 2.0 × 10^-2M F- are mixed, what is the remaining Ca²⁺ ion concentration and is precipitation complete? The solubility product constant of CaF₂ is 5.3 × 10^-9.

What is the approximate concentration of free Fe³⁺ ion in a solution prepared by mixing equal volumes of 0.06 M Fe³⁺ and 4.0 M F- solutions? [The net formation constant for FeF₅(H₂O) ₂^- is 2.0 × 10¹⁵.]

If chromium(III) chloride is added to be 1 × 10^-12 M in a solution that is 0.10 M NH₃, what is Qsp and will Cr(OH) ₃ precipitate? The Ksp of Cr(OH) ₃ is 6.3 × 10^-31 and Kb for NH₃ is 1.8 × 10^-5.

The solubility product constant of Mg(OH) ₂ is 9.0 × 10^-12. If a solution is 0.010 M with respect to Mg²⁺ ion, the amount of [OH-] required to start the precipitation of Mg(OH) ₂ is:

When 100 mL each of 2.0 × 10^-4 M Ag⁺ and 2.0 × 10-1 M CO₃^2- are mixed, what is the remaining Ag⁺ ion concentration and is precipitation complete? The solubility product constant of Ag₂CO₃ is 8.5 × 10^-12.

When 100 mL each of 2.0 × 10^-5 M Ca²⁺ and 2.0 × 10^-3M CO₃^2- are mixed, what is the remaining Ca²⁺ ion concentration and is precipitation complete? The solubility product constant of CaCO₃ is 2.8 × 10^-9.

What is the concentration of free Zn²⁺ if 0.020 M Zn²+ solution is mixed with an equal volume of 2.0 M NH₃? Kf for [Zn(NH₃) ₄]²⁺ is 4.1 × 10⁸.

When equal volumes of the indicated solutions are mixed, precipitation should occur only for: barium fluoride 1.0 × 10^-6 calcium carbonate 2.8 × 10^-9 Calcium fluoride 5.3 × 10^-9 Magnesium fluoride 3.7 × 10^-8 Silver carbonate 8.5 × 10^-12

A solution contains [Ba²⁺] = 5.0 × 10^-5 M, [Ag⁺] = 3.0 × 10^-5 M, and [Zn²⁺] = 2.0 × 10^-7 M. Sodium oxalate is slowly added so that [C₂O₄^2-] increases. What is the concentration of the first cation to precipitate when the second cation just begins to precipitate?

To a concentrated buffer of pH 9.0 was added an equal volume of a solution that was 0.20 M in each of the ions Ca²⁺, Cd²⁺, and Cu²⁺. The expected precipitate would consist of: salt: calcium hydroxide cadmium hydroxide copper(II) hydroxide Ksp: 4.0 × 10^-6 2.0 × 10^-14 1.8 × 10^-19

In which of the following solutions will the concentration of dissolved silver species be the highest if solid AgNO₃ is stirred with 1.00 L of solution?

What is the free Cu²⁺ concentration if 0.020 M Cu²⁺ solution is mixed with an equal volume of 4.0 M NH₃? Kf for [Cu(NH₃) ₄]²⁺ is 1.1 × 10¹³.