What is the molar solubility of AgCl in 0. 40 mol L-1 NH3? Ksp for AgCl is and Kf for Ag(NH3)2+ is

A) 1.3 × 10-5 mol L-1 B) 2.0 × 10-5 mol L-1 C) 2.2 × 10-2 mol L-1 D) 5.5 × 10-2 mol L-1 A) 1.3 × 10-5 mol L-1 B) 2.0 × 10-5 mol L-1 C) 2.2 × 10-2 mol L-1 D) 5.5 × 10-2 mol L-1 C

What is the pH of a buffer system prepared by dissolving 10.70 grams of NH4Cl and 25.00 mL of 12 mol L-1 NH3 in enough water to make 1.000 L of solution? Kb = 1.80 × 10-5 for NH3.

A) 9.08 B) 9.26 C) 9. 43 D) 11. 32 A) 9.08 B) 9.26 C) 9. 43 D) 11. 32

Calculate the Ksp for silver carbonate if the solubility of Ag2CO3 in pure water is 3.5 × 10-2 g L-1.

A) 2.1 × 10-12 B) 8.2 × 10-12 C) 1.6 × 10-8 D) 3.2 × 10-8 A) 2.1 × 10-12 B) 8.2 × 10-12 C) 1.6 × 10-8 D) 3.2 × 10-8

Consider the Ksp values for two compounds: MZ, Ksp = 1.5 × 10-20 and MZ2, Ksp = 1.5 × 10-20. Why don't these compounds have the same molar solubility?

These two compounds have the same solubi

Exam 16: Aqueous Ionic Equilibrium

What is the pH of a buffer solution that is 0.295 mol L^-1 in hypochlorous acid (HClO) and 0.373 mol L^-1 in sodium hypochlorite (NaClO)? The of hypochlorous acid is 3.8 × .

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(Multiple Choice)

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Question 1

Correct Answer:

Verified

What is the molar solubility of AgCl in 0. 40 mol L^-1 NH₃? K_sp for AgCl is and K_f for Ag(NH₃)₂⁺ is

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(Multiple Choice)

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Question 2

Correct Answer:

Verified

Determine the molar solubility of AgBr in a solution containing 0.150 mol L^-1 NaBr. K_sp (AgBr) = 7.7 × 10^-13.

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(Multiple Choice)

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Question 3

Correct Answer:

Verified

Calculate the percent ionization of nitrous acid in a solution that is 0.249 mol L^-1 in nitrous acid. The acid dissociation constant of nitrous acid is

(Multiple Choice)

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Question 4

What is the pH of the resulting solution if 25.00 mL of 0.10 mol L^-1 acetic acid is added to 10.00 mL of 0.10 mol L^-1 NaOH? Assume that the volumes of the solutions are additive. K_a = 1.8 × 10^-5for CH₃COOH

(Multiple Choice)

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Question 5

What is the maximum ratio of conjugate base to acid in an effective buffer?

(Multiple Choice)

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Question 6

A solution containing CaCl₂ is mixed with a solution of Li₂C₂O₄ to form a solution that is 3.5 × 10^-4 mol L^-1 in calcium ion and 2.33 × 10^-4mol L^-1 in oxalate ion. What will happen once these solutions are mixed? K_sp (CaC₂O₄) = 2.3 × 10^-9.

(Multiple Choice)

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Question 7

What is the pH of a solution made by mixing 40.00 mL of 0.100 mol L^-1 HCl with 25.00 mL of 0.100 mol L^-1 KOH? Assume that the volumes of the solutions are additive.

(Multiple Choice)

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Question 8

What is the pH of a buffer system prepared by dissolving 10.70 grams of NH₄Cl and 25.00 mL of 12 mol L^-1 NH₃ in enough water to make 1.000 L of solution? K_b = 1.80 × 10^-5for NH₃.

(Multiple Choice)

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Question 9

Calculate the K_sp for silver carbonate if the solubility of Ag₂CO₃ in pure water is 3.5 × 10^-2g L^-1.

(Multiple Choice)

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Question 10

When titrating a strong monoprotic acid with KOH at 25 °C, the ________.

(Multiple Choice)

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Question 11

A sample contains Ba₃(PO₄)₂,CdS, AgCl, NH₄Cl, and ZnS. Identify the precipitate formed after the addition of 6 mol L^-1 HCl followed by the addition of H₂S and 0.2 mol L^-1 HCl.

(Multiple Choice)

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Question 12

A solution containing CaCl₂ is mixed with a solution of Li₂C₂O₄ to form a solution that is 2.1 × 10^-5 mol L^-1 in calcium ion and 4.75 × 10^-5mol L^-1 in oxalate ion. What will happen once these solutions are mixed? K_sp (CaC₂O₄) = 2.3 × 10^-9.

(Multiple Choice)

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Question 13

A 100.0 mL sample of 0.20 mol L^-1 HF is titrated with 0.10 mol L^-1 KOH. Determine the pH of the solution after the addition of 300.0 mL of KOH. The K_a of HF is 3.5 × 10^-4.

(Multiple Choice)

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Question 14

Consider the K_sp values for two compounds: MZ, K_sp = 1.5 × 10^-20 and MZ₂, K_sp = 1.5 × 10^-20. Why don't these compounds have the same molar solubility?

(Essay)

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Question 15

Identify the indicator that can be used at the highest pH.

(Multiple Choice)

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Question 16

Identify the pH of normal blood.

(Multiple Choice)

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Question 17

A solution of NaF is added dropwise to a solution that is 0.0188 mol L^-1 in . When the concentration of exceeds ________ mol L^-1, will precipitate. Neglect volume changes. For ,

(Multiple Choice)

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Question 18

A sample contains Ba₃(PO₄)₂,CdS, AgCl, NH₄Cl, and ZnS. Identify the precipitate formed after the addition of 6 mol L^-1 HCl, followed by the addition of H₂S and 0.2 mol L^-1 HCl, and subsequently the addition of OH^- to a pH of 8.

(Multiple Choice)

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Question 19

Match the following. -pH > 7

(Multiple Choice)

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Question 20

Showing 1 - 20 of 173

Exam 16: Aqueous Ionic Equilibrium

What is the pH of a buffer solution that is 0.295 mol L-1 in hypochlorous acid (HClO) and 0.373 mol L-1 in sodium hypochlorite (NaClO)? The of hypochlorous acid is 3.8 × .

What is the molar solubility of AgCl in 0. 40 mol L-1 NH3? Ksp for AgCl is and Kf for Ag(NH3)2+ is

Determine the molar solubility of AgBr in a solution containing 0.150 mol L-1 NaBr. Ksp (AgBr) = 7.7 × 10-13.

Calculate the percent ionization of nitrous acid in a solution that is 0.249 mol L-1 in nitrous acid. The acid dissociation constant of nitrous acid is

What is the pH of the resulting solution if 25.00 mL of 0.10 mol L-1 acetic acid is added to 10.00 mL of 0.10 mol L-1 NaOH? Assume that the volumes of the solutions are additive. Ka = 1.8 × 10-5 for CH3COOH

What is the maximum ratio of conjugate base to acid in an effective buffer?

A solution containing CaCl2 is mixed with a solution of Li2C2O4 to form a solution that is 3.5 × 10-4 mol L-1 in calcium ion and 2.33 × 10-4 mol L-1 in oxalate ion. What will happen once these solutions are mixed? Ksp (CaC2O4) = 2.3 × 10-9.

What is the pH of a solution made by mixing 40.00 mL of 0.100 mol L-1 HCl with 25.00 mL of 0.100 mol L-1 KOH? Assume that the volumes of the solutions are additive.

What is the pH of a buffer system prepared by dissolving 10.70 grams of NH4Cl and 25.00 mL of 12 mol L-1 NH3 in enough water to make 1.000 L of solution? Kb = 1.80 × 10-5 for NH3.

Calculate the Ksp for silver carbonate if the solubility of Ag2CO3 in pure water is 3.5 × 10-2 g L-1.

When titrating a strong monoprotic acid with KOH at 25 °C, the ________.

A sample contains Ba3(PO4)2, CdS, AgCl, NH4Cl, and ZnS. Identify the precipitate formed after the addition of 6 mol L-1 HCl followed by the addition of H2S and 0.2 mol L-1 HCl.

A solution containing CaCl2 is mixed with a solution of Li2C2O4 to form a solution that is 2.1 × 10-5 mol L-1 in calcium ion and 4.75 × 10-5 mol L-1 in oxalate ion. What will happen once these solutions are mixed? Ksp (CaC2O4) = 2.3 × 10-9.

A 100.0 mL sample of 0.20 mol L-1 HF is titrated with 0.10 mol L-1 KOH. Determine the pH of the solution after the addition of 300.0 mL of KOH. The Ka of HF is 3.5 × 10-4.

Consider the Ksp values for two compounds: MZ, Ksp = 1.5 × 10-20 and MZ2, Ksp = 1.5 × 10-20. Why don't these compounds have the same molar solubility?

Identify the indicator that can be used at the highest pH.

Identify the pH of normal blood.

A solution of NaF is added dropwise to a solution that is 0.0188 mol L-1 in . When the concentration of exceeds ________ mol L-1, will precipitate. Neglect volume changes. For ,

A sample contains Ba3(PO4)2, CdS, AgCl, NH4Cl, and ZnS. Identify the precipitate formed after the addition of 6 mol L-1 HCl, followed by the addition of H2S and 0.2 mol L-1 HCl, and subsequently the addition of OH- to a pH of 8.

Match the following. -pH > 7

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What is the pH of a buffer solution that is 0.295 mol L^-1 in hypochlorous acid (HClO) and 0.373 mol L^-1 in sodium hypochlorite (NaClO)? The of hypochlorous acid is 3.8 × .

What is the molar solubility of AgCl in 0. 40 mol L^-1 NH₃? K_sp for AgCl is and K_f for Ag(NH₃)₂⁺ is

Determine the molar solubility of AgBr in a solution containing 0.150 mol L^-1 NaBr. K_sp (AgBr) = 7.7 × 10^-13.

Calculate the percent ionization of nitrous acid in a solution that is 0.249 mol L^-1 in nitrous acid. The acid dissociation constant of nitrous acid is

What is the pH of the resulting solution if 25.00 mL of 0.10 mol L^-1 acetic acid is added to 10.00 mL of 0.10 mol L^-1 NaOH? Assume that the volumes of the solutions are additive. K_a = 1.8 × 10^-5for CH₃COOH

A solution containing CaCl₂ is mixed with a solution of Li₂C₂O₄ to form a solution that is 3.5 × 10^-4 mol L^-1 in calcium ion and 2.33 × 10^-4mol L^-1 in oxalate ion. What will happen once these solutions are mixed? K_sp (CaC₂O₄) = 2.3 × 10^-9.

What is the pH of a solution made by mixing 40.00 mL of 0.100 mol L^-1 HCl with 25.00 mL of 0.100 mol L^-1 KOH? Assume that the volumes of the solutions are additive.

What is the pH of a buffer system prepared by dissolving 10.70 grams of NH₄Cl and 25.00 mL of 12 mol L^-1 NH₃ in enough water to make 1.000 L of solution? K_b = 1.80 × 10^-5for NH₃.

Calculate the K_sp for silver carbonate if the solubility of Ag₂CO₃ in pure water is 3.5 × 10^-2g L^-1.

A sample contains Ba₃(PO₄)₂,CdS, AgCl, NH₄Cl, and ZnS. Identify the precipitate formed after the addition of 6 mol L^-1 HCl followed by the addition of H₂S and 0.2 mol L^-1 HCl.

A solution containing CaCl₂ is mixed with a solution of Li₂C₂O₄ to form a solution that is 2.1 × 10^-5 mol L^-1 in calcium ion and 4.75 × 10^-5mol L^-1 in oxalate ion. What will happen once these solutions are mixed? K_sp (CaC₂O₄) = 2.3 × 10^-9.

A 100.0 mL sample of 0.20 mol L^-1 HF is titrated with 0.10 mol L^-1 KOH. Determine the pH of the solution after the addition of 300.0 mL of KOH. The K_a of HF is 3.5 × 10^-4.

Consider the K_sp values for two compounds: MZ, K_sp = 1.5 × 10^-20 and MZ₂, K_sp = 1.5 × 10^-20. Why don't these compounds have the same molar solubility?

A solution of NaF is added dropwise to a solution that is 0.0188 mol L^-1 in . When the concentration of exceeds ________ mol L^-1, will precipitate. Neglect volume changes. For ,

A sample contains Ba₃(PO₄)₂,CdS, AgCl, NH₄Cl, and ZnS. Identify the precipitate formed after the addition of 6 mol L^-1 HCl, followed by the addition of H₂S and 0.2 mol L^-1 HCl, and subsequently the addition of OH^- to a pH of 8.