Question 1

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

Accepted Answer

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Question 2

The solubility of Ba(NO₃)₂ is 130.5 g/L at 0ºC. How many moles of dissolved salt are present in 4.0 L of a saturated solution of Ba(NO₃)₂ at 0ºC?

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The answer of The solubility of Ba(NO₃)₂ is 130.5 g/L...

Question 3

NaCl is added slowly to a solution that is 0.010 M each in Cu⁺, Ag⁺, and Au⁺.The K_sp's for CuCl, AgCl, and AuCl are 1.9 * 10^-7, 1.8 * 10^-10, and 2.0 * 10^-13, respectively.Which compound will precipitate first?

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The answer of NaCl is added slowly to a solution...

Question 4

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?

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The answer of An environmental chemist obtained a 200.mL sample...

Question 5

Will Fe(OH)₃ precipitate from a buffer solution that is 0.60 M CH₃COOH and 0.10 M CH₃COONa, if the solution is also made to be 0.001 M in Fe³⁺? For Fe(OH)₃, K_sp = 6.8 * 10^-36.

Accepted Answer

The answer of Will Fe(OH)₃ precipitate from a buffer solution...

Question 6

Bromothymol blue is a common acid-base indicator. It has a K_a equal to 1.6 * 10^-7. Its un-ionized form is yellow and its conjugate base is blue. What color would a solution have at pH = 5.8?

Accepted Answer

The answer of Bromothymol blue is a common acid-base indicator....

Question 7

Solid sodium iodide is slowly added to a solution that is 0.0050 M Pb²⁺ and 0.0050 M Ag⁺.[K_sp (PbI₂)= 1.4 * 10^-8; K_sp (AgI)= 8.3 * 10^-17] What percent of Ag⁺ remains in solution at this point?

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The answer of Solid sodium iodide is slowly added to...

Question 8

Solid sodium iodide is slowly added to a solution that is 0.0050 M Pb²⁺ and 0.0050 M Ag⁺.[K_sp (PbI₂)= 1.4 * 10^-8; K_sp (AgI)= 8.3 * 10^-17] What compound will precipitate first?

Accepted Answer

The answer of Solid sodium iodide is slowly added to...

Question 9

Solid sodium iodide is slowly added to a solution that is 0.0050 M Pb²⁺ and 0.0050 M Ag⁺.[K_sp (PbI₂)= 1.4 * 10^-8; K_sp (AgI)= 8.3 * 10^-17] Calculate the Ag⁺ concentration when PbI₂ just begins to precipitate.

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The answer of Solid sodium iodide is slowly added to...

Question 10

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.If the size of the lake can be approximated as 1.1 km long by 2.3 km wide, and has an average depth of 10.m, estimate how many moles of the strong acid are present in the lake?

Accepted Answer

The answer of An environmental chemist obtained a 200.mL sample...

Question 11

Ammonium chloride solutions are slightly acidic, so they are better solvents than water for insoluble substances such as Ca(OH)₂. Identify two reactions that, added together, give the overall reaction below, and determine K_c for the overall reaction. Ca(OH)₂(s)+ 2NH₄⁺(aq) Ca²⁺(aq)+ 2NH₃(aq)+ 2H₂O Given: K_sp for Ca(OH)₂ is 4.0 * 10^-8; K_b for NH₃ is 1.8 * 10^-5.

Accepted Answer

The answer of Ammonium chloride solutions are slightly acidic, so...

Question 12

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?

Accepted Answer

The answer of An environmental chemist obtained a 200.mL sample...

Question 13

Calculate the equilibrium constant K_c for the net reaction shown below. AgI(s)+ 2NH₃(aq) Ag(NH₃)₂⁺(aq)+ I^-(aq) For AgI, K_sp = 8.3 * 10^-17; for Ag(NH₃)₂⁺, K_f = 1.5 * 10⁷.

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Question 14

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]

Accepted Answer

The answer of Will a precipitate of AgCl form when...

Question 15

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.

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The answer of Calculate the equilibrium constant K_c for the...

Question 16

A 50.0 mL sample of 2.0 * 10^-4 M CuNO₃ is added to 50.0 mL of 4.0 M NaCN. The formation constant of the complex ion Cu(CN)₃^2- is 1.0 * 10⁹. What is the copper(I)ion concentration in this system at equilibrium?

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Question 17

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?

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Question 18

The concentration of Mg²⁺ in seawater is 5.0 * 10^-2M. What hydroxide concentration is needed to remove 90% of the Mg²⁺ by precipitation? (For Mg(OH)₂, K_sp = 1.2 * 10^-11.)

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Question 19

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)

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Question 20

Describe how to prepare 500.mL of a cyanic acid (HCNO)/sodium cyanate (NaCNO)buffer having a pH of 4.80. [K_a(HCNO)= 2.0 * 10^-4]

Accepted Answer

The answer of Describe how to prepare 500.mL of a...

Quiz 16: Acid-Base Equilibria and Solubility Equilibria

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

The solubility of Ba(NO3)2 is 130.5 g/L at 0ºC. How many moles of dissolved salt are present in 4.0 L of a saturated solution of Ba(NO3)2 at 0ºC?

NaCl is added slowly to a solution that is 0.010 M each in Cu+, Ag+, and Au+.The Ksp's for CuCl, AgCl, and AuCl are 1.9 * 10-7, 1.8 * 10-10, and 2.0 * 10-13, respectively.Which compound will precipitate first?

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?

Will Fe(OH)3 precipitate from a buffer solution that is 0.60 M CH3COOH and 0.10 M CH3COONa, if the solution is also made to be 0.001 M in Fe3+? For Fe(OH)3, Ksp = 6.8 * 10-36.

Bromothymol blue is a common acid-base indicator. It has a Ka equal to 1.6 * 10-7. Its un-ionized form is yellow and its conjugate base is blue. What color would a solution have at pH = 5.8?

Solid sodium iodide is slowly added to a solution that is 0.0050 M Pb2+ and 0.0050 M Ag+.[Ksp (PbI2)= 1.4 * 10-8; Ksp (AgI)= 8.3 * 10-17] What percent of Ag+ remains in solution at this point?

Solid sodium iodide is slowly added to a solution that is 0.0050 M Pb2+ and 0.0050 M Ag+.[Ksp (PbI2)= 1.4 * 10-8; Ksp (AgI)= 8.3 * 10-17] What compound will precipitate first?

Solid sodium iodide is slowly added to a solution that is 0.0050 M Pb2+ and 0.0050 M Ag+.[Ksp (PbI2)= 1.4 * 10-8; Ksp (AgI)= 8.3 * 10-17] Calculate the Ag+ concentration when PbI2 just begins to precipitate.

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?

Calculate the equilibrium constant Kc for the net reaction shown below. AgI(s)+ 2NH3(aq) Ag(NH3)2+(aq)+ I-(aq) For AgI, Ksp = 8.3 * 10-17; for Ag(NH3)2+, Kf = 1.5 * 107.

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]

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.

A 50.0 mL sample of 2.0 * 10-4 M CuNO3 is added to 50.0 mL of 4.0 M NaCN. The formation constant of the complex ion Cu(CN)32- is 1.0 * 109. What is the copper(I)ion concentration in this system at equilibrium?

The concentration of Mg2+ in seawater is 5.0 * 10-2 M. What hydroxide concentration is needed to remove 90% of the Mg2+ by precipitation? (For Mg(OH)2, Ksp = 1.2 * 10-11.)

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)

Describe how to prepare 500.mL of a cyanic acid (HCNO)/sodium cyanate (NaCNO)buffer having a pH of 4.80. [Ka(HCNO)= 2.0 * 10-4]

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

The solubility of Ba(NO₃)₂ is 130.5 g/L at 0ºC. How many moles of dissolved salt are present in 4.0 L of a saturated solution of Ba(NO₃)₂ at 0ºC?

NaCl is added slowly to a solution that is 0.010 M each in Cu⁺, Ag⁺, and Au⁺.The K_sp's for CuCl, AgCl, and AuCl are 1.9 * 10^-7, 1.8 * 10^-10, and 2.0 * 10^-13, respectively.Which compound will precipitate first?

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?

Will Fe(OH)₃ precipitate from a buffer solution that is 0.60 M CH₃COOH and 0.10 M CH₃COONa, if the solution is also made to be 0.001 M in Fe³⁺? For Fe(OH)₃, K_sp = 6.8 * 10^-36.

Bromothymol blue is a common acid-base indicator. It has a K_a equal to 1.6 * 10^-7. Its un-ionized form is yellow and its conjugate base is blue. What color would a solution have at pH = 5.8?

Solid sodium iodide is slowly added to a solution that is 0.0050 M Pb²⁺ and 0.0050 M Ag⁺.[K_sp (PbI₂)= 1.4 * 10^-8; K_sp (AgI)= 8.3 * 10^-17] What percent of Ag⁺ remains in solution at this point?

Solid sodium iodide is slowly added to a solution that is 0.0050 M Pb²⁺ and 0.0050 M Ag⁺.[K_sp (PbI₂)= 1.4 * 10^-8; K_sp (AgI)= 8.3 * 10^-17] What compound will precipitate first?

Solid sodium iodide is slowly added to a solution that is 0.0050 M Pb²⁺ and 0.0050 M Ag⁺.[K_sp (PbI₂)= 1.4 * 10^-8; K_sp (AgI)= 8.3 * 10^-17] Calculate the Ag⁺ concentration when PbI₂ just begins to precipitate.

Calculate the equilibrium constant K_c for the net reaction shown below. AgI(s)+ 2NH₃(aq) Ag(NH₃)₂⁺(aq)+ I^-(aq) For AgI, K_sp = 8.3 * 10^-17; for Ag(NH₃)₂⁺, K_f = 1.5 * 10⁷.

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]

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.

A 50.0 mL sample of 2.0 * 10^-4 M CuNO₃ is added to 50.0 mL of 4.0 M NaCN. The formation constant of the complex ion Cu(CN)₃^2- is 1.0 * 10⁹. What is the copper(I)ion concentration in this system at equilibrium?

The concentration of Mg²⁺ in seawater is 5.0 * 10^-2M. What hydroxide concentration is needed to remove 90% of the Mg²⁺ by precipitation? (For Mg(OH)₂, K_sp = 1.2 * 10^-11.)

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)

Describe how to prepare 500.mL of a cyanic acid (HCNO)/sodium cyanate (NaCNO)buffer having a pH of 4.80. [K_a(HCNO)= 2.0 * 10^-4]