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

A) A precipitate of KCl will form. B) A precipitate of PbCrO4 will form. C) A precipitate of PbCl2 will form. D) No precipitate will form. E) Both a precipitate of PbCl2 and a precipitate of PbCrO4 will form. A) A precipitate of KCl will form. B) A precipitate of PbCrO4 will form. C) A precipitate of PbCl2 will form. D) No precipitate will form. E) Both a precipitate of PbCl2 and a precipitate of PbCrO4 will form. B

What will happen if 50.0 mL of 0.032 M Na2S2O3,50.0 mL of 0.010 M AgNO3,and 50.0 mL of 0.047 M KCl are mixed together? For AgCl,Ksp = 1.8 × 10-10; for Ag(S2O3)23-,Kf = 2.9 × 1013.

A) A precipitate of Ag2S2O3 will form. B) A precipitate of KNO3 will form. C) No precipitate will form because silver(I)ion exists predominantly as Ag+. D) No precipitate will form because silver(I)ion exists predominantly in the complex Ag(S2O3)23-. E) A precipitate of AgCl will form. A) A precipitate of Ag2S2O3 will form. B) A precipitate of KNO3 will form. C) No precipitate will form because silver(I)ion exists predominantly as Ag+. D) No precipitate will form because silver(I)ion exists predominantly in the complex Ag(S2O3)23-. E) A precipitate of AgCl will form.

A solution contains 0.018 mol each of I-,Br-,and Cl-.When the solution is mixed with 200 mL of 0.24 M AgNO3,how much AgCl(s)precipitates out? Ksp AgI = 1)5 × 10-16 Ksp AgBr = 5)0 × 10-13 Ksp AgCl = 1)6 × 10-10

A) 5.0 g B) 3.3 g C) 2.6 g D) 0.0 g E) 1.7 g A) 5.0 g B) 3.3 g C) 2.6 g D) 0.0 g E) 1.7 g

What is the minimum concentration of Pb2+ required to begin precipitating Pb(OH)2(s)in a solution of pH 10.78? For Pb(OH)2,Ksp = 1.4 × 10-20.

A) 3.0 × 10-4 M B) 8.4 × 10-10 M C) 2.3 × 10-17 M D) 3.9 × 10-14 M E) 1.2 × 10-22 M A) 3.0 × 10-4 M B) 8.4 × 10-10 M C) 2.3 × 10-17 M D) 3.9 × 10-14 M E) 1.2 × 10-22 M

What is the concentration of Cd2+ in a 0.012 M Cd(NO3)2 solution that is also 1.0 M NH3? For Cd(NH3)42+,Kf = 1.0 × 107.

A) 3.5 × 102 M B) 1.3 × 10-9 M C) 1.5 × 10-9 M D) 3.2 × 103 M E) 1.2 × 10-2 M A) 3.5 × 102 M B) 1.3 × 10-9 M C) 1.5 × 10-9 M D) 3.2 × 103 M E) 1.2 × 10-2 M

If 500 mL of 1.3 × 10-6 M AgNO3 is mixed with 500 mL of 1.3 × 10-6 M NaBr,what will occur? For AgBr,Ksp = 5 × 10-13.

A) Silver(I)bromide will precipitate. B) The concentration of Ag+ will be 1.3 × 10-6 M. C) 6.5 × 10-7 mol of AgBr will form. D) No precipitation will occur. E) Sodium bromide will precipitate. A) Silver(I)bromide will precipitate. B) The concentration of Ag+ will be 1.3 × 10-6 M. C) 6.5 × 10-7 mol of AgBr will form. D) No precipitation will occur. E) Sodium bromide will precipitate.

Exam 17: Solubility and Complex-Ion Equilibria

Figures I-IV represent ionic compounds formed upon the mixing of an aqueous solution containing cation C with an aqueous solution containing anion A.Identify the figure(s)that represent(s)products for which K_sp = 108s⁵,where s is the molar solubility of the ionic compound.

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(Multiple Choice)

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Question 1

Correct Answer:

Verified

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

Free

(Multiple Choice)

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Question 2

Correct Answer:

Verified

For which of the following salts would the addition of nitric acid increase its solubility?

Free

(Multiple Choice)

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Question 3

Correct Answer:

Verified

The figure below represents the results of adding a strong acid to a saturated solution of an ionic compound.Which of the following could be the ionic compound?

(Multiple Choice)

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Question 4

Which of the following substances will increase the molar solubility of nickel(II)phosphate in a saturated solution?

(Multiple Choice)

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Question 5

What is the solubility (in g/L)of silver(I)chloride at 25°C? The solubility product constant for silver(I)chloride is 1.8 × 10^-10 at 25°C.

(Multiple Choice)

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Question 6

For which pair of cations would the addition of dilute hydrobromic acid precipitate one but not the other?

(Multiple Choice)

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Question 7

What will happen if 50.0 mL of 0.032 M Na₂S₂O₃,50.0 mL of 0.010 M AgNO₃,and 50.0 mL of 0.047 M KCl are mixed together? For AgCl,K_sp = 1.8 × 10^-10; for Ag(S₂O₃)₂^3-,K_f = 2.9 × 10¹³.

(Multiple Choice)

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Question 8

A solution contains 0.018 mol each of I^-,Br^-,and Cl^-.When the solution is mixed with 200 mL of 0.24 M AgNO₃,how much AgCl(s)precipitates out? K_sp AgI = 1)5 × 10^-16 K_sp AgBr = 5)0 × 10^-13 K_sp AgCl = 1)6 × 10^-10

(Multiple Choice)

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Question 9

What is the minimum concentration of Pb²⁺ required to begin precipitating Pb(OH)₂(s)in a solution of pH 10.78? For Pb(OH)₂,K_sp = 1.4 × 10^-20.

(Multiple Choice)

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Question 10

What is the solubility (in g/L)of aluminum hydroxide at 25°C? The solubility product constant for aluminum hydroxide is 4.6× 10^-33 at 25°C.

(Multiple Choice)

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Question 11

A 5.0 × 10^-4 M solution of MnSO₄ is gradually made more basic by adding NaOH.At what pH will manganese(II)hydroxide begin to precipitate? For Mn(OH)₂,K_sp = 2.0 × 10^-13.

(Multiple Choice)

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Question 12

What is the concentration of Cd²⁺ in a 0.012 M Cd(NO₃)2 solution that is also 1.0 M NH₃? For Cd(NH₃)₄²⁺,K_f = 1.0 × 10⁷.

(Multiple Choice)

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Question 13

A saturated solution of which of the following salts will have the greatest molar concentration of silver ion?

(Multiple Choice)

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Question 14

If 500 mL of 1.3 × 10^-6 M AgNO₃ is mixed with 500 mL of 1.3 × 10^-6 M NaBr,what will occur? For AgBr,K_sp = 5 × 10^-13.

(Multiple Choice)

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Question 15

What is the correct mathematical expression for finding the molar solubility (s)of Sn(OH)₂?

(Multiple Choice)

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Question 16

Figures I-IV represent ionic compounds formed upon the mixing of an aqueous solution containing cation C with an aqueous solution containing anion A.Identify the figure(s)that represent(s)products for which K_sp = s²,where s is the molar solubility of the ionic compound.

(Multiple Choice)

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Question 17

Which of the following insoluble salts will dissolve upon reaction with excess ammonia?

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Question 18

What is the molar solubility of nickel(II)sulfide in 0.091 M KCN? For NiS,K_sp = 3.0 × 10^-19; for Ni(CN)₄^2-,K_f = 1.0 × 10³¹.

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Question 19

Cation C and anion A form an ionic compound for which K_sp = 4s³,where s is the molar solubility of the ionic compound.Which of Figures I-III represent(s)possible results of the mixing of an aqueous solution containing cation C with an aqueous solution containing anion A?

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Question 20

Showing 1 - 20 of 115

Exam 17: Solubility and Complex-Ion Equilibria

Figures I-IV represent ionic compounds formed upon the mixing of an aqueous solution containing cation C with an aqueous solution containing anion A.Identify the figure(s)that represent(s)products for which Ksp = 108s5,where s is the molar solubility of the ionic compound.

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

For which of the following salts would the addition of nitric acid increase its solubility?

The figure below represents the results of adding a strong acid to a saturated solution of an ionic compound.Which of the following could be the ionic compound?

Which of the following substances will increase the molar solubility of nickel(II)phosphate in a saturated solution?

What is the solubility (in g/L)of silver(I)chloride at 25°C? The solubility product constant for silver(I)chloride is 1.8 × 10-10 at 25°C.

For which pair of cations would the addition of dilute hydrobromic acid precipitate one but not the other?

What will happen if 50.0 mL of 0.032 M Na2S2O3,50.0 mL of 0.010 M AgNO3,and 50.0 mL of 0.047 M KCl are mixed together? For AgCl,Ksp = 1.8 × 10-10; for Ag(S2O3)23-,Kf = 2.9 × 1013.

A solution contains 0.018 mol each of I-,Br-,and Cl-.When the solution is mixed with 200 mL of 0.24 M AgNO3,how much AgCl(s)precipitates out? Ksp AgI = 1)5 × 10-16 Ksp AgBr = 5)0 × 10-13 Ksp AgCl = 1)6 × 10-10

What is the minimum concentration of Pb2+ required to begin precipitating Pb(OH)2(s)in a solution of pH 10.78? For Pb(OH)2,Ksp = 1.4 × 10-20.

What is the solubility (in g/L)of aluminum hydroxide at 25°C? The solubility product constant for aluminum hydroxide is 4.6× 10-33 at 25°C.

A 5.0 × 10-4 M solution of MnSO4 is gradually made more basic by adding NaOH.At what pH will manganese(II)hydroxide begin to precipitate? For Mn(OH)2,Ksp = 2.0 × 10-13.

What is the concentration of Cd2+ in a 0.012 M Cd(NO3)2 solution that is also 1.0 M NH3? For Cd(NH3)42+,Kf = 1.0 × 107.

A saturated solution of which of the following salts will have the greatest molar concentration of silver ion?

If 500 mL of 1.3 × 10-6 M AgNO3 is mixed with 500 mL of 1.3 × 10-6 M NaBr,what will occur? For AgBr,Ksp = 5 × 10-13.

What is the correct mathematical expression for finding the molar solubility (s)of Sn(OH)2?

Figures I-IV represent ionic compounds formed upon the mixing of an aqueous solution containing cation C with an aqueous solution containing anion A.Identify the figure(s)that represent(s)products for which Ksp = s2,where s is the molar solubility of the ionic compound.

Which of the following insoluble salts will dissolve upon reaction with excess ammonia?

What is the molar solubility of nickel(II)sulfide in 0.091 M KCN? For NiS,Ksp = 3.0 × 10-19; for Ni(CN)42-,Kf = 1.0 × 1031.

Cation C and anion A form an ionic compound for which Ksp = 4s3,where s is the molar solubility of the ionic compound.Which of Figures I-III represent(s)possible results of the mixing of an aqueous solution containing cation C with an aqueous solution containing anion A?

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Figures I-IV represent ionic compounds formed upon the mixing of an aqueous solution containing cation C with an aqueous solution containing anion A.Identify the figure(s)that represent(s)products for which K_sp = 108s⁵,where s is the molar solubility of the ionic compound.

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

What is the solubility (in g/L)of silver(I)chloride at 25°C? The solubility product constant for silver(I)chloride is 1.8 × 10^-10 at 25°C.

What will happen if 50.0 mL of 0.032 M Na₂S₂O₃,50.0 mL of 0.010 M AgNO₃,and 50.0 mL of 0.047 M KCl are mixed together? For AgCl,K_sp = 1.8 × 10^-10; for Ag(S₂O₃)₂^3-,K_f = 2.9 × 10¹³.

A solution contains 0.018 mol each of I^-,Br^-,and Cl^-.When the solution is mixed with 200 mL of 0.24 M AgNO₃,how much AgCl(s)precipitates out? K_sp AgI = 1)5 × 10^-16 K_sp AgBr = 5)0 × 10^-13 K_sp AgCl = 1)6 × 10^-10

What is the minimum concentration of Pb²⁺ required to begin precipitating Pb(OH)₂(s)in a solution of pH 10.78? For Pb(OH)₂,K_sp = 1.4 × 10^-20.

What is the solubility (in g/L)of aluminum hydroxide at 25°C? The solubility product constant for aluminum hydroxide is 4.6× 10^-33 at 25°C.

A 5.0 × 10^-4 M solution of MnSO₄ is gradually made more basic by adding NaOH.At what pH will manganese(II)hydroxide begin to precipitate? For Mn(OH)₂,K_sp = 2.0 × 10^-13.

What is the concentration of Cd²⁺ in a 0.012 M Cd(NO₃)2 solution that is also 1.0 M NH₃? For Cd(NH₃)₄²⁺,K_f = 1.0 × 10⁷.

If 500 mL of 1.3 × 10^-6 M AgNO₃ is mixed with 500 mL of 1.3 × 10^-6 M NaBr,what will occur? For AgBr,K_sp = 5 × 10^-13.

What is the correct mathematical expression for finding the molar solubility (s)of Sn(OH)₂?

Figures I-IV represent ionic compounds formed upon the mixing of an aqueous solution containing cation C with an aqueous solution containing anion A.Identify the figure(s)that represent(s)products for which K_sp = s²,where s is the molar solubility of the ionic compound.

What is the molar solubility of nickel(II)sulfide in 0.091 M KCN? For NiS,K_sp = 3.0 × 10^-19; for Ni(CN)₄^2-,K_f = 1.0 × 10³¹.

Cation C and anion A form an ionic compound for which K_sp = 4s³,where s is the molar solubility of the ionic compound.Which of Figures I-III represent(s)possible results of the mixing of an aqueous solution containing cation C with an aqueous solution containing anion A?