What is the molar solubility of lead(II)chromate in 0.055 M Na2S2O3? For PbCrO4,Ksp = 2.0 $\times$ 10-16;for Pb(S2O3)34-,Kf = 2.2 $\times$ 106.

A) M B) M C) M D) M E) M A) M B) M C) M D) M E) M

The Ksp for BaF2 is 2.4 $\times$10-5.When 10 mL of 0.01 M NaF is mixed with 10 mL of 0.01 M BaNO3,will a precipitate form?

A) No,because Q is 1 $\times$ 10-12 and since it is less than Ksp no precipitate will form. B) Yes,because Q is 1 $\times$ 10-12 and since it is less than Ksp a precipitate will form. C) No,because Q is 1.25 $\times$10-7 and since it is less than Ksp no precipitate will form. D) Yes,because Q is 1.25 $\times$ 10-7 and since it is less than Ksp a precipitate will form. E) None of the above. A) No,because Q is 1 $\times$ 10-12 and since it is less than Ksp no precipitate will form. B) Yes,because Q is 1 $\times$ 10-12 and since it is less than Ksp a precipitate will form. C) No,because Q is 1.25 $\times$10-7 and since it is less than Ksp no precipitate will form. D) Yes,because Q is 1.25 $\times$ 10-7 and since it is less than Ksp a precipitate will form. E) None of the above.

The following questions refer to the following system: 500.0 mL of 0.020 M Mn(NOS1U1B13S1U1B0)S1U1B12S1U1B0 are mixed with 1.0 L of 1.0 M NaS1U1B12S1U1B0CS1U1B12S1U1B0OS1U1B14S1U1B0.The oxalate ion,CS1U1B12S1U1B0OS1U1B14S1U1B0,acts as a ligand to form a complex ion with the MnS1U1P12+S1S1P0 ion with a coordination number of two. MnS1U1P12+S1S1P0 + CS1U1B12S1U1B0OS1U1B14S1U1B0S1U1P12S1S1P0S1U1P1-S1S1P0 S1U1P1 S1S1P0 MnCS1U1B12S1U1B0OS1U1B14S1U1B0 KS1U1B11S1U1B0 = 7.9 $\times$ 10S1U1P13S1S1P0 [Mn(CS1U1B12S1U1B0OS1U1B14S1U1B0)S1U1B12S1U1B0]S1U1P12S1S1P0S1U1P1-S1S1P0 S1U1P1 S1S1P0 MnCS1U1B12S1U1B0OS1U1B14 S1U1B0+ CS1U1B12S1U1B0OS1U1B14S1U1B0S1U1P12S1S1P0S1U1P1-S1S1P0 KS1U1B12S1U1B0 = 1.26 $\times$ 10S1U1P1-S1S1P0S1U1P12S1S1P0 -Find the equilibrium concentration of Mn(C2O4)in the system.

A) 9.2 $\times$ 10-5 M B) 0.01 M C) 2.5 $\times$ 10-8 M D) 1.3 $\times$ 10-4 M E) 6.7 $\times$10-3 M A) 9.2 $\times$ 10-5 M B) 0.01 M C) 2.5 $\times$ 10-8 M D) 1.3 $\times$ 10-4 M E) 6.7 $\times$10-3 M

The following questions refer to the following system: 500.0 mL of 0.020 M Mn(NOS1U1B13S1U1B0)S1U1B12S1U1B0 are mixed with 1.0 L of 1.0 M NaS1U1B12S1U1B0CS1U1B12S1U1B0OS1U1B14S1U1B0.The oxalate ion,CS1U1B12S1U1B0OS1U1B14S1U1B0,acts as a ligand to form a complex ion with the MnS1U1P12+S1S1P0 ion with a coordination number of two. MnS1U1P12+S1S1P0 + CS1U1B12S1U1B0OS1U1B14S1U1B0S1U1P12S1S1P0S1U1P1-S1S1P0 S1U1P1 S1S1P0 MnCS1U1B12S1U1B0OS1U1B14S1U1B0 KS1U1B11S1U1B0 = 7.9 $\times$ 10S1U1P13S1S1P0 [Mn(CS1U1B12S1U1B0OS1U1B14S1U1B0)S1U1B12S1U1B0]S1U1P12S1S1P0S1U1P1-S1S1P0 S1U1P1 S1S1P0 MnCS1U1B12S1U1B0OS1U1B14 S1U1B0+ CS1U1B12S1U1B0OS1U1B14S1U1B0S1U1P12S1S1P0S1U1P1-S1S1P0 KS1U1B12S1U1B0 = 1.26 $\times$ 10S1U1P1-S1S1P0S1U1P12S1S1P0 -Find the equilibrium concentration of the [Mn(C2O4)2]2- ion.

A) 9.2 $\times$10-5 M B) 0.01 M C) 2.5 $\times$10-8 M D) 1.3 $\times$ 10-4 M E) 6.7 $\times$ 10-3 M A) 9.2 $\times$10-5 M B) 0.01 M C) 2.5 $\times$10-8 M D) 1.3 $\times$ 10-4 M E) 6.7 $\times$ 10-3 M

The Ksp for PbF2 is 4.0 $\times$10-8.If a 0.040 M NaF solution is saturated with PbF2,what is the [Pb2+] in the solution?

A) M B) M C) M D) M E) M A) M B) M C) M D) M E) M

If 30 mL of 5.0 $\times$10-4 M Ca(NO3)2 are added to 70 mL of 2.0 $\times$ 10-4 M NaF,will a precipitate occur? (Ksp of CaF2 = 4.0 $\times$ 10-11)

A) No,because the ion product is greater than Ksp. B) Yes,because the ion product is less than Ksp. C) No,because the ion product is less than Ksp. D) Not enough information is given. E) Yes,because the ion product is greater than Ksp. A) No,because the ion product is greater than Ksp. B) Yes,because the ion product is less than Ksp. C) No,because the ion product is less than Ksp. D) Not enough information is given. E) Yes,because the ion product is greater than Ksp.

The following questions refer to the following system: 500.0 mL of 0.020 M Mn(NOS1U1B13S1U1B0)S1U1B12S1U1B0 are mixed with 1.0 L of 1.0 M NaS1U1B12S1U1B0CS1U1B12S1U1B0OS1U1B14S1U1B0.The oxalate ion,CS1U1B12S1U1B0OS1U1B14S1U1B0,acts as a ligand to form a complex ion with the MnS1U1P12+S1S1P0 ion with a coordination number of two. MnS1U1P12+S1S1P0 + CS1U1B12S1U1B0OS1U1B14S1U1B0S1U1P12S1S1P0S1U1P1-S1S1P0 S1U1P1 S1S1P0 MnCS1U1B12S1U1B0OS1U1B14S1U1B0 KS1U1B11S1U1B0 = 7.9 $\times$ 10S1U1P13S1S1P0 [Mn(CS1U1B12S1U1B0OS1U1B14S1U1B0)S1U1B12S1U1B0]S1U1P12S1S1P0S1U1P1-S1S1P0 S1U1P1 S1S1P0 MnCS1U1B12S1U1B0OS1U1B14 S1U1B0+ CS1U1B12S1U1B0OS1U1B14S1U1B0S1U1P12S1S1P0S1U1P1-S1S1P0 KS1U1B12S1U1B0 = 1.26 $\times$ 10S1U1P1-S1S1P0S1U1P12S1S1P0 -Find the equilibrium concentration of the Mn2+ ion.

A) 9.2 $\times$10-5 M B) 0.01 M C) 2.5 $\times$ 10-8 M D) 1.3 $\times$10-4 M E) 6.7 $\times$ 10-3 M A) 9.2 $\times$10-5 M B) 0.01 M C) 2.5 $\times$ 10-8 M D) 1.3 $\times$10-4 M E) 6.7 $\times$ 10-3 M

Calculate the solubility of Cu(OH)2 in a solution buffered at pH = 7.59.(Ksp = 1.6 $\times$ 10-19)

A) M B) M C) M D) M E) none of these A) M B) M C) M D) M E) none of these

The in a saturated solution of is 5.93 $\times$ 10-3 M.Calculate the Ksp for .

A) B) C) D) E) none of these A) B) C) D) E) none of these

A 0.012-mol sample of Na2SO4 is added to 400 mL of each of two solutions.One solution contains 1.5 $\times$ 10-3 M BaCl2;the other contains 1.5 $\times$ 10-3 M CaCl2.Given that Ksp for BaSO4 = 1.5 $\times$ 10-9 and Ksp for CaSO4 = 6.1 $\times$10-5:

A) BaSO4 would precipitate but CaSO4 would not. B) CaSO4 would precipitate but BaSO4 would not. C) Both BaSO4 and CaSO4 would precipitate. D) Neither BaSO4 nor CaSO4 would precipitate. E) Not enough information is given to determine if precipitation would occur. A) BaSO4 would precipitate but CaSO4 would not. B) CaSO4 would precipitate but BaSO4 would not. C) Both BaSO4 and CaSO4 would precipitate. D) Neither BaSO4 nor CaSO4 would precipitate. E) Not enough information is given to determine if precipitation would occur.

What is the maximum concentration of carbonate ions that will precipitate BaCO3 but not MgCO3 from a solution that is M each in Mg2+ and Ba2+? For MgCO3,Ksp = 1.0 $\times$10-15 and for BaCO3,Ksp = 2.6 $\times$10-9.

A) M B) M C) M D) M E) None of these;MgCO3 will always precipitate before BaCO3. A) M B) M C) M D) M E) None of these;MgCO3 will always precipitate before BaCO3.

A solution is 0.010 M in each of Pb(NO3)2,Mn(NO3)2,and Zn(NO3)2.Solid NaOH is added until the pH of the solution is 8.50.Which of the following statements is true?

A) No precipitate will form. B) Only Pb(OH)2 will precipitate. C) Only Mn(OH)2 will precipitate. D) Only Zn(OH)2 and Pb(OH)2 will precipitate. E) All three hydroxides will precipitate. A) No precipitate will form. B) Only Pb(OH)2 will precipitate. C) Only Mn(OH)2 will precipitate. D) Only Zn(OH)2 and Pb(OH)2 will precipitate. E) All three hydroxides will precipitate.

Consider a solution made by mixing 500.0 mL of 4.0 M NHS1U1B13S1U1B0 and 500.0 mL of 0.40 M AgNOS1U1B13S1U1B0.AgS1U1P1+S1S1P0 reacts with NHS1U1B13S1U1B0 to form AgNHS1U1B13S1U1B0S1U1P1+S1S1P0 and Ag(NHS1U1B13S1U1B0)S1U1B12S1U1B0S1U1P1+S1S1P0: AgS1U1P1+S1S1P0 + NHS1U1B13S1U1B0 S1U1B1 S1U1B0 AgNHS1U1B13S1U1B0S1U1P1+S1S1P0 KS1U1B11S1U1B0 = 2.1 $\times$ 10S1U1P13S1S1P0 AgNHS1U1B13S1U1B0S1U1P1+S1S1P0 + NHS1U1B13S1U1B0 S1U1B1 S1U1B0 Ag(NHS1U1B13S1U1B0)S1U1B12S1U1B0S1U1P1+S1S1P0 KS1U1B12S1U1B0 = 8.2 $\times$10S1U1P13S1S1P0 -The concentration of Ag(NH3)2+ at equilibrium is:

A) 2.0 M B) 0.40 M C) 0.20 M D) 1.0 $\times$ 10-3 M E) none of these A) 2.0 M B) 0.40 M C) 0.20 M D) 1.0 $\times$ 10-3 M E) none of these

Exam 16: Solubility and Complex Ion Equilibria

You have two salts,AgX and AgY,with very similar K_sp values.You know that K_a for HX is much greater than K_a for HY.Which salt is more soluble in acidic solution?

(Multiple Choice)

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Question 61

What is the molar solubility of lead(II)chromate in 0.055 M Na₂S₂O₃? For PbCrO₄,K_sp = 2.0 $\times$ 10^-¹⁶;for Pb(S₂O₃)₃⁴^-,K_f = 2.2 $\times$ 10⁶.

(Multiple Choice)

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Question 62

The K_sp for BaF₂ is 2.4 $\times$ 10^-⁵.When 10 mL of 0.01 M NaF is mixed with 10 mL of 0.01 M BaNO₃,will a precipitate form?

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Question 63

The following questions refer to the following system: 500.0 mL of 0.020 M Mn(NO₃)₂ are mixed with 1.0 L of 1.0 M Na₂C₂O₄.The oxalate ion,C₂O₄,acts as a ligand to form a complex ion with the Mn²⁺ ion with a coordination number of two. Mn²⁺ + C₂O₄²^- $The following questions refer to the following system: 500.0 mL of 0.020 M Mn(NO3)2 are mixed with 1.0 L of 1.0 M Na2C2O4.The oxalate ion,C2O4,acts as a ligand to form a complex ion with the Mn2+ ion with a coordination number of two. Mn2+ + C2O42- MnC2O4 K1 = 7.9 \times 103 [Mn(C2O4)2]2- MnC2O4 + C2O42- K2 = 1.26 \times 10-2 -Find the equilibrium concentration of Mn(C2O4)in the system.$ MnC₂O₄ K₁ = 7.9 $\times$ 10³ [Mn(C₂O₄)₂]²^- $The following questions refer to the following system: 500.0 mL of 0.020 M Mn(NO3)2 are mixed with 1.0 L of 1.0 M Na2C2O4.The oxalate ion,C2O4,acts as a ligand to form a complex ion with the Mn2+ ion with a coordination number of two. Mn2+ + C2O42- MnC2O4 K1 = 7.9 \times 103 [Mn(C2O4)2]2- MnC2O4 + C2O42- K2 = 1.26 \times 10-2 -Find the equilibrium concentration of Mn(C2O4)in the system.$ MnC₂O₄+ C₂O₄²^- K₂ = 1.26 $\times$ 10^-² -Find the equilibrium concentration of Mn(C₂O₄)in the system.

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Question 64

The following questions refer to the following system: 500.0 mL of 0.020 M Mn(NO₃)₂ are mixed with 1.0 L of 1.0 M Na₂C₂O₄.The oxalate ion,C₂O₄,acts as a ligand to form a complex ion with the Mn²⁺ ion with a coordination number of two. Mn²⁺ + C₂O₄²^- $The following questions refer to the following system: 500.0 mL of 0.020 M Mn(NO3)2 are mixed with 1.0 L of 1.0 M Na2C2O4.The oxalate ion,C2O4,acts as a ligand to form a complex ion with the Mn2+ ion with a coordination number of two. Mn2+ + C2O42- MnC2O4 K1 = 7.9 \times 103 [Mn(C2O4)2]2- MnC2O4 + C2O42- K2 = 1.26 \times 10-2 -Find the equilibrium concentration of the [Mn(C2O4)2]2- ion.$ MnC₂O₄ K₁ = 7.9 $\times$ 10³ [Mn(C₂O₄)₂]²^- $The following questions refer to the following system: 500.0 mL of 0.020 M Mn(NO3)2 are mixed with 1.0 L of 1.0 M Na2C2O4.The oxalate ion,C2O4,acts as a ligand to form a complex ion with the Mn2+ ion with a coordination number of two. Mn2+ + C2O42- MnC2O4 K1 = 7.9 \times 103 [Mn(C2O4)2]2- MnC2O4 + C2O42- K2 = 1.26 \times 10-2 -Find the equilibrium concentration of the [Mn(C2O4)2]2- ion.$ MnC₂O₄+ C₂O₄²^- K₂ = 1.26 $\times$ 10^-² -Find the equilibrium concentration of the [Mn(C₂O₄)₂]²^- ion.

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Question 65

The K_sp for PbF₂ is 4.0 $\times$ 10^-⁸.If a 0.040 M NaF solution is saturated with PbF₂,what is the [Pb²⁺] in the solution?

(Multiple Choice)

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Question 66

What is the best way to ensure complete precipitation of SnS from a saturated H₂S solution?

(Multiple Choice)

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Question 67

How many moles of Fe(OH)₂ [K_sp = 1.8 $\times$ 10^-¹⁵] will dissolve in 1.0 liter of water buffered at pH = 10.37?

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Question 68

If 30 mL of 5.0 $\times$ 10^-⁴ M Ca(NO₃)₂ are added to 70 mL of 2.0 $\times$ 10^-⁴ M NaF,will a precipitate occur? (K_sp of CaF₂ = 4.0 $\times$ 10^-¹¹)

(Multiple Choice)

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Question 69

The following questions refer to the following system: 500.0 mL of 0.020 M Mn(NO₃)₂ are mixed with 1.0 L of 1.0 M Na₂C₂O₄.The oxalate ion,C₂O₄,acts as a ligand to form a complex ion with the Mn²⁺ ion with a coordination number of two. Mn²⁺ + C₂O₄²^- $The following questions refer to the following system: 500.0 mL of 0.020 M Mn(NO3)2 are mixed with 1.0 L of 1.0 M Na2C2O4.The oxalate ion,C2O4,acts as a ligand to form a complex ion with the Mn2+ ion with a coordination number of two. Mn2+ + C2O42- MnC2O4 K1 = 7.9 \times 103 [Mn(C2O4)2]2- MnC2O4 + C2O42- K2 = 1.26 \times 10-2 -Find the equilibrium concentration of the Mn2+ ion.$ MnC₂O₄ K₁ = 7.9 $\times$ 10³ [Mn(C₂O₄)₂]²^- $The following questions refer to the following system: 500.0 mL of 0.020 M Mn(NO3)2 are mixed with 1.0 L of 1.0 M Na2C2O4.The oxalate ion,C2O4,acts as a ligand to form a complex ion with the Mn2+ ion with a coordination number of two. Mn2+ + C2O42- MnC2O4 K1 = 7.9 \times 103 [Mn(C2O4)2]2- MnC2O4 + C2O42- K2 = 1.26 \times 10-2 -Find the equilibrium concentration of the Mn2+ ion.$ MnC₂O₄+ C₂O₄²^- K₂ = 1.26 $\times$ 10^-² -Find the equilibrium concentration of the Mn²⁺ ion.

(Multiple Choice)

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Question 70

Calculate the solubility of Cu(OH)₂ in a solution buffered at pH = 7.59.(K_sp = 1.6 $\times$ 10^-¹⁹)

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Question 71

The $The in a saturated solution of is 5.93 \times 10-3 M.Calculate the Ksp for .$ in a saturated solution of $The in a saturated solution of is 5.93 \times 10-3 M.Calculate the Ksp for .$ is 5.93 $\times$ 10^-³ M.Calculate the K_sp for $The in a saturated solution of is 5.93 \times 10-3 M.Calculate the Ksp for .$ .

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Question 72

A 0.012-mol sample of Na₂SO₄ is added to 400 mL of each of two solutions.One solution contains 1.5 $\times$ 10^-³ M BaCl₂;the other contains 1.5 $\times$ 10^-³ M CaCl₂.Given that K_sp for BaSO₄ = 1.5 $\times$ 10^-⁹ and K_sp for CaSO₄ = 6.1 $\times$ 10^-⁵:

(Multiple Choice)

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Question 73

It is observed that 7.50 mmol of BaF₂ will dissolve in 1.0 L of water.Use these data to calculate the value of K_sp for barium fluoride.

(Multiple Choice)

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Question 74

Will precipitation occur?

(Multiple Choice)

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Question 75

In the qualitative analysis scheme for metal ions,how are the Analytical Group III cations separated from the cations of Analytical Groups IV and V?

(Multiple Choice)

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Question 76

What is the maximum concentration of carbonate ions that will precipitate BaCO₃ but not MgCO₃ from a solution that is $What is the maximum concentration of carbonate ions that will precipitate BaCO3 but not MgCO3 from a solution that is M each in Mg2+ and Ba2+? For MgCO3,Ksp = 1.0 \times 10-15 and for BaCO3,Ksp = 2.6 \times 10-9.$ M each in Mg²⁺ and Ba²⁺? For MgCO₃,K_sp = 1.0 $\times$ 10^-¹⁵ and for BaCO₃,K_sp = 2.6 $\times$ 10^-⁹.

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Question 77

The concentration of OH^- in a saturated solution of Mg(OH)₂ is 3.63 $\times$ 10^-⁴ M.The K_sp of Mg(OH)₂ is

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Question 78

A solution is 0.010 M in each of Pb(NO₃)₂,Mn(NO₃)₂,and Zn(NO₃)₂.Solid NaOH is added until the pH of the solution is 8.50.Which of the following statements is true?

(Multiple Choice)

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Question 79

Consider a solution made by mixing 500.0 mL of 4.0 M NH₃ and 500.0 mL of 0.40 M AgNO₃.Ag⁺ reacts with NH₃ to form AgNH₃⁺ and Ag(NH₃)₂⁺: Ag⁺ + NH₃ $Consider a solution made by mixing 500.0 mL of 4.0 M NH3 and 500.0 mL of 0.40 M AgNO3.Ag+ reacts with NH3 to form AgNH3+ and Ag(NH3)2+: Ag+ + NH3 AgNH3+ K1 = 2.1 \times 103 AgNH3+ + NH3 Ag(NH3)2+ K2 = 8.2 \times 103 -The concentration of Ag(NH3)2+ at equilibrium is:$ AgNH₃⁺ K₁ = 2.1 $\times$ 10³ AgNH₃⁺ + NH₃ $Consider a solution made by mixing 500.0 mL of 4.0 M NH3 and 500.0 mL of 0.40 M AgNO3.Ag+ reacts with NH3 to form AgNH3+ and Ag(NH3)2+: Ag+ + NH3 AgNH3+ K1 = 2.1 \times 103 AgNH3+ + NH3 Ag(NH3)2+ K2 = 8.2 \times 103 -The concentration of Ag(NH3)2+ at equilibrium is:$ Ag(NH₃)₂⁺ K₂ = 8.2 $\times$ 10³ -The concentration of Ag(NH₃)₂⁺ at equilibrium is:

(Multiple Choice)

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Question 80

Showing 61 - 80 of 93

You have two salts,AgX and AgY,with very similar K_sp values.You know that K_a for HX is much greater than K_a for HY.Which salt is more soluble in acidic solution?

What is the molar solubility of lead(II)chromate in 0.055 M Na₂S₂O₃? For PbCrO₄,K_sp = 2.0 $\times$ 10^-¹⁶;for Pb(S₂O₃)₃⁴^-,K_f = 2.2 $\times$ 10⁶.

The K_sp for BaF₂ is 2.4 $\times$ 10^-⁵.When 10 mL of 0.01 M NaF is mixed with 10 mL of 0.01 M BaNO₃,will a precipitate form?

The K_sp for PbF₂ is 4.0 $\times$ 10^-⁸.If a 0.040 M NaF solution is saturated with PbF₂,what is the [Pb²⁺] in the solution?

What is the best way to ensure complete precipitation of SnS from a saturated H₂S solution?

How many moles of Fe(OH)₂ [K_sp = 1.8 $\times$ 10^-¹⁵] will dissolve in 1.0 liter of water buffered at pH = 10.37?

If 30 mL of 5.0 $\times$ 10^-⁴ M Ca(NO₃)₂ are added to 70 mL of 2.0 $\times$ 10^-⁴ M NaF,will a precipitate occur? (K_sp of CaF₂ = 4.0 $\times$ 10^-¹¹)

Calculate the solubility of Cu(OH)₂ in a solution buffered at pH = 7.59.(K_sp = 1.6 $\times$ 10^-¹⁹)

A 0.012-mol sample of Na₂SO₄ is added to 400 mL of each of two solutions.One solution contains 1.5 $\times$ 10^-³ M BaCl₂;the other contains 1.5 $\times$ 10^-³ M CaCl₂.Given that K_sp for BaSO₄ = 1.5 $\times$ 10^-⁹ and K_sp for CaSO₄ = 6.1 $\times$ 10^-⁵:

It is observed that 7.50 mmol of BaF₂ will dissolve in 1.0 L of water.Use these data to calculate the value of K_sp for barium fluoride.

Will precipitation occur?

In the qualitative analysis scheme for metal ions,how are the Analytical Group III cations separated from the cations of Analytical Groups IV and V?

The concentration of OH^- in a saturated solution of Mg(OH)₂ is 3.63 $\times$ 10^-⁴ M.The K_sp of Mg(OH)₂ is

A solution is 0.010 M in each of Pb(NO₃)₂,Mn(NO₃)₂,and Zn(NO₃)₂.Solid NaOH is added until the pH of the solution is 8.50.Which of the following statements is true?

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Exam 16: Solubility and Complex Ion Equilibria

You have two salts,AgX and AgY,with very similar Ksp values.You know that Ka for HX is much greater than Ka for HY.Which salt is more soluble in acidic solution?

What is the molar solubility of lead(II)chromate in 0.055 M Na2S2O3? For PbCrO4,Ksp = 2.0 ×\times× 10-16;for Pb(S2O3)34-,Kf = 2.2 ×\times× 106.

The Ksp for BaF2 is 2.4 ×\times× 10-5.When 10 mL of 0.01 M NaF is mixed with 10 mL of 0.01 M BaNO3,will a precipitate form?

The Ksp for PbF2 is 4.0 ×\times× 10-8.If a 0.040 M NaF solution is saturated with PbF2,what is the [Pb2+] in the solution?

What is the best way to ensure complete precipitation of SnS from a saturated H2S solution?

How many moles of Fe(OH)2 [Ksp = 1.8 ×\times× 10-15] will dissolve in 1.0 liter of water buffered at pH = 10.37?

If 30 mL of 5.0 ×\times× 10-4 M Ca(NO3)2 are added to 70 mL of 2.0 ×\times× 10-4 M NaF,will a precipitate occur? (Ksp of CaF2 = 4.0 ×\times× 10-11)

Calculate the solubility of Cu(OH)2 in a solution buffered at pH = 7.59.(Ksp = 1.6 ×\times× 10-19)

The in a saturated solution of is 5.93 ×\times× 10-3 M.Calculate the Ksp for .

A 0.012-mol sample of Na2SO4 is added to 400 mL of each of two solutions.One solution contains 1.5 ×\times× 10-3 M BaCl2;the other contains 1.5 ×\times× 10-3 M CaCl2.Given that Ksp for BaSO4 = 1.5 ×\times× 10-9 and Ksp for CaSO4 = 6.1 ×\times× 10-5:

It is observed that 7.50 mmol of BaF2 will dissolve in 1.0 L of water.Use these data to calculate the value of Ksp for barium fluoride.

Will precipitation occur?

In the qualitative analysis scheme for metal ions,how are the Analytical Group III cations separated from the cations of Analytical Groups IV and V?

What is the maximum concentration of carbonate ions that will precipitate BaCO3 but not MgCO3 from a solution that is M each in Mg2+ and Ba2+? For MgCO3,Ksp = 1.0 ×\times× 10-15 and for BaCO3,Ksp = 2.6 ×\times× 10-9.

The concentration of OH- in a saturated solution of Mg(OH)2 is 3.63 ×\times× 10-4 M.The Ksp of Mg(OH)2 is

A solution is 0.010 M in each of Pb(NO3)2,Mn(NO3)2,and Zn(NO3)2.Solid NaOH is added until the pH of the solution is 8.50.Which of the following statements is true?

Consider a solution made by mixing 500.0 mL of 4.0 M NH3 and 500.0 mL of 0.40 M AgNO3.Ag+ reacts with NH3 to form AgNH3+ and Ag(NH3)2+: Ag+ + NH3 AgNH3+ K1 = 2.1 ×\times× 103 AgNH3+ + NH3 Ag(NH3)2+ K2 = 8.2 ×\times× 103 -The concentration of Ag(NH3)2+ at equilibrium is:

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You have two salts,AgX and AgY,with very similar K_sp values.You know that K_a for HX is much greater than K_a for HY.Which salt is more soluble in acidic solution?

What is the molar solubility of lead(II)chromate in 0.055 M Na₂S₂O₃? For PbCrO₄,K_sp = 2.0 $\times$ 10^-¹⁶;for Pb(S₂O₃)₃⁴^-,K_f = 2.2 $\times$ 10⁶.

The K_sp for BaF₂ is 2.4 $\times$ 10^-⁵.When 10 mL of 0.01 M NaF is mixed with 10 mL of 0.01 M BaNO₃,will a precipitate form?

The K_sp for PbF₂ is 4.0 $\times$ 10^-⁸.If a 0.040 M NaF solution is saturated with PbF₂,what is the [Pb²⁺] in the solution?

What is the best way to ensure complete precipitation of SnS from a saturated H₂S solution?

How many moles of Fe(OH)₂ [K_sp = 1.8 $\times$ 10^-¹⁵] will dissolve in 1.0 liter of water buffered at pH = 10.37?

If 30 mL of 5.0 $\times$ 10^-⁴ M Ca(NO₃)₂ are added to 70 mL of 2.0 $\times$ 10^-⁴ M NaF,will a precipitate occur? (K_sp of CaF₂ = 4.0 $\times$ 10^-¹¹)

Calculate the solubility of Cu(OH)₂ in a solution buffered at pH = 7.59.(K_sp = 1.6 $\times$ 10^-¹⁹)

A 0.012-mol sample of Na₂SO₄ is added to 400 mL of each of two solutions.One solution contains 1.5 $\times$ 10^-³ M BaCl₂;the other contains 1.5 $\times$ 10^-³ M CaCl₂.Given that K_sp for BaSO₄ = 1.5 $\times$ 10^-⁹ and K_sp for CaSO₄ = 6.1 $\times$ 10^-⁵:

It is observed that 7.50 mmol of BaF₂ will dissolve in 1.0 L of water.Use these data to calculate the value of K_sp for barium fluoride.

The concentration of OH^- in a saturated solution of Mg(OH)₂ is 3.63 $\times$ 10^-⁴ M.The K_sp of Mg(OH)₂ is

A solution is 0.010 M in each of Pb(NO₃)₂,Mn(NO₃)₂,and Zn(NO₃)₂.Solid NaOH is added until the pH of the solution is 8.50.Which of the following statements is true?