Calculate the molar solubility of AgBr in a 0.25M solution of NH3(aq)(Ksp (AgBr)= 7.7 x 10-13 ; Kf (Ag(NH3)2+)= 1.5 x 107.

A) 8.8 x 10-7 M B) 3.4 x 10-3 M C) 8.4 x 10-4 M D) 2.5 x 10-1 M E) 9.7 x 102 M A) 8.8 x 10-7 M B) 3.4 x 10-3 M C) 8.4 x 10-4 M D) 2.5 x 10-1 M E) 9.7 x 102 M

Exam 16: Acid-Base Equilibria and Solubility Equilibria

At 25 °C, the base ionization constant for NH₃ is 1.8 × 10^-5.If 0.0800 mole of solid magnesium chloride is dissolved in a solution prepared by adding 0.0500 mol of solid ammonium chloride to 100.ml of 0.150 M ammonia, will a precipitate of magnesium hydroxide form? (Assume the volume of the solution is unchanged.The solubility product constant for magnesium hydroxide is 1.5 × 10^-11.)

(Short Answer)

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Question 61

What is the optimum pH of a sodium formate/formic acid buffer? (For formic acid, K_a = 1.7 × 10^-4)

(Short Answer)

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Question 62

Will a precipitate of AgCl form when 0.050 mol NaCl(s)and 0.050 mol AgNO₃(s)are dissolved in 500.mL of 3.0 M NH₃? [K_fforAg(NH₃)₂⁺is 1.5 × 10⁷; K_sp(AgCl)= 1.6 × 10^-10]

(Short Answer)

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Question 63

The pH at the equivalence point of a titration may differ from 7.0 due to

(Multiple Choice)

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Question 64

Methyl red is a common acid-base indicator.It has a K_a equal to 6.3 × 10^-6.Its un-ionized form is red and its anionic form is yellow.What color would a methyl red solution have at pH = 7.8?

(Multiple Choice)

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Question 65

An environmental chemist obtained a 200.mL sample of lake water believed to be contaminated with a single monoprotic strong acid.Titrating this sample with a 0.0050 M NaOH(aq)required 7.3 mL of the NaOH solution to reach the endpoint.What is the pH of the lake?

(Short Answer)

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Question 66

Write an equation showing the net reaction that occurs when a strong base is added to a CO₃^2-/HCO₃^- buffer solution (for carbonic acid, K_a1 = 4.2 × 10^-7, K_a2 = 2.4 × 10^-8):

(Essay)

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Question 67

A solution is prepared by mixing 500.mL of 0.10 M NaOCl and 500.mL of 0.20 M HOCl.What is the pH of this solution? [K_a(HOCl)= 3.2 × 10^-8]

(Multiple Choice)

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Question 68

To 1.00 L of a 0.100 M aqueous solution of benzoic acid (C₆H₅COOH)is added 1.00 mL of 12.0 M HCl.What is the percentage ionization of the benzoic acid in the resulting solution? [K_a(C₆H₅COOH)= 6.5 × 10^-5]

(Multiple Choice)

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Question 69

A sample of rainwater collected near a lead smelter is analyzed for acid content.Experiments show that a 100.mL sample of the rainwater is neutralized by 22.4 milliters of 0.0122 M NaOH.Assuming that the acid present is sulfurous acid, which resulted from the reaction of SO₂ with water, what is the molarity of acid in the rainwater?

(Short Answer)

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Question 70

An environmental chemist obtained a 200.mL sample of lake water believed to be contaminated with a single monoprotic strong acid.Titrating this sample with a 0.0050 M NaOH(aq)required 7.3 mL of the NaOH solution to reach the endpoint.What is the concentration of H⁺ in the lake?

(Short Answer)

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Question 71

Consider a buffer solution prepared from HOCl and NaOCl.Which is the net ionic equation for the reaction that occurs when NaOH is added to this buffer?

(Multiple Choice)

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Question 72

The K_sp of CaF₂ is 4 × 10^-11.What is the maximum concentration of Ca²⁺ possible in a 0.10 M NaF solution?

(Short Answer)

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Question 73

A saturated sodium carbonate solution at 100°C contains 45.5 g of dissolved sodium carbonate per 100.mL of solution.The solubility product constant for sodium carbonate at this temperature is

(Multiple Choice)

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Question 74

Calculate the percent ionization of formic acid in a solution that is 0.010 M HCOOH and 0.005 M HCOONa and compare your answer to the percent ionization you would calculate if the sodium formate were not present.Explain the difference, if any.(K_a = 1.7 × 10^-4)

(Essay)

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Question 75

Calculate the pH of the solution resulting from the addition of 10.0 mL of 0.10 M NaOH to 50.0 mL of 0.10 M HCN (K_a = 4.9 × 10^-10)solution.

(Multiple Choice)

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Question 76

Calculate the pH at the equivalence point for the titration of 0.22 M HCN with 0.22 M NaOH.(K_a = 4.9 × 10^-10 for HCN)

(Short Answer)

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Question 77

Calculate the equilibrium constant K_c for the following overall reaction: AgCl(s)+ 2CN^-(aq) Ag(CN)₂^-(aq)+ Cl^-(aq) For AgCl, K_sp = 1.6 × 10^-10; for Ag(CN)₂^-, K_f = 1.0 × 10²¹.

(Short Answer)

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Question 78

Calculate the molar solubility of AgBr in a 0.25M solution of NH₃(aq)(K_sp (AgBr)= 7.7 x 10^-13 ; K_f (Ag(NH₃)₂⁺)= 1.5 x 10⁷.

(Multiple Choice)

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Question 79

A saturated sodium carbonate solution at 0°C contains 7.1 g of dissolved sodium carbonate per 100.mL of solution.The solubility product constant for sodium carbonate at this temperature is

(Multiple Choice)

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Question 80

Showing 61 - 80 of 131

Exam 16: Acid-Base Equilibria and Solubility Equilibria

What is the optimum pH of a sodium formate/formic acid buffer? (For formic acid, Ka = 1.7 × 10-4)

Will a precipitate of AgCl form when 0.050 mol NaCl(s)and 0.050 mol AgNO3(s)are dissolved in 500.mL of 3.0 M NH3? [Kf for Ag(NH3)2+ is 1.5 × 107; Ksp(AgCl)= 1.6 × 10-10]

The pH at the equivalence point of a titration may differ from 7.0 due to

Methyl red is a common acid-base indicator.It has a Ka equal to 6.3 × 10-6.Its un-ionized form is red and its anionic form is yellow.What color would a methyl red solution have at pH = 7.8?

An environmental chemist obtained a 200.mL sample of lake water believed to be contaminated with a single monoprotic strong acid.Titrating this sample with a 0.0050 M NaOH(aq)required 7.3 mL of the NaOH solution to reach the endpoint.What is the pH of the lake?

Write an equation showing the net reaction that occurs when a strong base is added to a CO32-/HCO3- buffer solution (for carbonic acid, Ka1 = 4.2 × 10-7, Ka2 = 2.4 × 10-8):

A solution is prepared by mixing 500.mL of 0.10 M NaOCl and 500.mL of 0.20 M HOCl.What is the pH of this solution? [Ka(HOCl)= 3.2 × 10-8]

To 1.00 L of a 0.100 M aqueous solution of benzoic acid (C6H5COOH)is added 1.00 mL of 12.0 M HCl.What is the percentage ionization of the benzoic acid in the resulting solution? [Ka(C6H5COOH)= 6.5 × 10-5]

An environmental chemist obtained a 200.mL sample of lake water believed to be contaminated with a single monoprotic strong acid.Titrating this sample with a 0.0050 M NaOH(aq)required 7.3 mL of the NaOH solution to reach the endpoint.What is the concentration of H+ in the lake?

Consider a buffer solution prepared from HOCl and NaOCl.Which is the net ionic equation for the reaction that occurs when NaOH is added to this buffer?

The Ksp of CaF2 is 4 × 10-11.What is the maximum concentration of Ca2+ possible in a 0.10 M NaF solution?

A saturated sodium carbonate solution at 100°C contains 45.5 g of dissolved sodium carbonate per 100.mL of solution.The solubility product constant for sodium carbonate at this temperature is

Calculate the percent ionization of formic acid in a solution that is 0.010 M HCOOH and 0.005 M HCOONa and compare your answer to the percent ionization you would calculate if the sodium formate were not present.Explain the difference, if any.(Ka = 1.7 × 10-4)

Calculate the pH of the solution resulting from the addition of 10.0 mL of 0.10 M NaOH to 50.0 mL of 0.10 M HCN (Ka = 4.9 × 10-10)solution.

Calculate the pH at the equivalence point for the titration of 0.22 M HCN with 0.22 M NaOH.(Ka = 4.9 × 10-10 for HCN)

Calculate the equilibrium constant Kc for the following overall reaction: AgCl(s)+ 2CN-(aq) Ag(CN)2-(aq)+ Cl-(aq) For AgCl, Ksp = 1.6 × 10-10; for Ag(CN)2-, Kf = 1.0 × 1021.

Calculate the molar solubility of AgBr in a 0.25M solution of NH3(aq)(Ksp (AgBr)= 7.7 x 10-13 ; Kf (Ag(NH3)2+)= 1.5 x 107.

A saturated sodium carbonate solution at 0°C contains 7.1 g of dissolved sodium carbonate per 100.mL of solution.The solubility product constant for sodium carbonate at this temperature is

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What is the optimum pH of a sodium formate/formic acid buffer? (For formic acid, K_a = 1.7 × 10^-4)

Will a precipitate of AgCl form when 0.050 mol NaCl(s)and 0.050 mol AgNO₃(s)are dissolved in 500.mL of 3.0 M NH₃? [K_fforAg(NH₃)₂⁺is 1.5 × 10⁷; K_sp(AgCl)= 1.6 × 10^-10]

Methyl red is a common acid-base indicator.It has a K_a equal to 6.3 × 10^-6.Its un-ionized form is red and its anionic form is yellow.What color would a methyl red solution have at pH = 7.8?

Write an equation showing the net reaction that occurs when a strong base is added to a CO₃^2-/HCO₃^- buffer solution (for carbonic acid, K_a1 = 4.2 × 10^-7, K_a2 = 2.4 × 10^-8):

A solution is prepared by mixing 500.mL of 0.10 M NaOCl and 500.mL of 0.20 M HOCl.What is the pH of this solution? [K_a(HOCl)= 3.2 × 10^-8]

To 1.00 L of a 0.100 M aqueous solution of benzoic acid (C₆H₅COOH)is added 1.00 mL of 12.0 M HCl.What is the percentage ionization of the benzoic acid in the resulting solution? [K_a(C₆H₅COOH)= 6.5 × 10^-5]

An environmental chemist obtained a 200.mL sample of lake water believed to be contaminated with a single monoprotic strong acid.Titrating this sample with a 0.0050 M NaOH(aq)required 7.3 mL of the NaOH solution to reach the endpoint.What is the concentration of H⁺ in the lake?

The K_sp of CaF₂ is 4 × 10^-11.What is the maximum concentration of Ca²⁺ possible in a 0.10 M NaF solution?

Calculate the percent ionization of formic acid in a solution that is 0.010 M HCOOH and 0.005 M HCOONa and compare your answer to the percent ionization you would calculate if the sodium formate were not present.Explain the difference, if any.(K_a = 1.7 × 10^-4)

Calculate the pH of the solution resulting from the addition of 10.0 mL of 0.10 M NaOH to 50.0 mL of 0.10 M HCN (K_a = 4.9 × 10^-10)solution.

Calculate the pH at the equivalence point for the titration of 0.22 M HCN with 0.22 M NaOH.(K_a = 4.9 × 10^-10 for HCN)

Calculate the equilibrium constant K_c for the following overall reaction: AgCl(s)+ 2CN^-(aq) Ag(CN)₂^-(aq)+ Cl^-(aq) For AgCl, K_sp = 1.6 × 10^-10; for Ag(CN)₂^-, K_f = 1.0 × 10²¹.

Calculate the molar solubility of AgBr in a 0.25M solution of NH₃(aq)(K_sp (AgBr)= 7.7 x 10^-13 ; K_f (Ag(NH₃)₂⁺)= 1.5 x 10⁷.