Question 1

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 2

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?

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Question 3

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

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Question 4

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.

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Question 5

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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Question 6

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 when 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.

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Question 7

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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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 percent of Ag⁺ remains in solution at this point?

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Question 9

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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Question 10

Calculate the molar solubility of lead (II)fluoride (K_sp (PbF₂ = 4.1 x 10^-8))

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Question 11

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 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?

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Question 13

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?

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Question 14

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?

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Question 15

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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Question 16

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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Question 17

Calculate the molar solubility of silver carbonate (K_sp (Ag₂CO₃ = 8.1 x 10^-12))

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Question 18

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]

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Question 19

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 20

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]

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Quiz 16: Acid-Base Equilibria and Solubility Equilibria

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.)

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?

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

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.

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 concentration of H+ in the lake?

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?

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 lead (II)fluoride (Ksp (PbF2 = 4.1 x 10-8))

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?

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?

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?

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?

Calculate the molar solubility of silver carbonate (Ksp (Ag2CO3 = 8.1 x 10-12))

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]

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]

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.)

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?

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

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.

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.

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?

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?

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 lead (II)fluoride (K_sp (PbF₂ = 4.1 x 10^-8))

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?

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?

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?

Calculate the molar solubility of silver carbonate (K_sp (Ag₂CO₃ = 8.1 x 10^-12))

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]

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]