Will a precipitate of magnesium fluoride form when 200. mL of 1.9 * 10-3 M MgCl2 are added to 300. mL of 1.4 * 10-2 M NaF? [Ksp (MgF2)= 6.9 * 10-9]

A) Yes, Q > Ksp B) No, Q sp C) No, Q = Ksp D) Yes, Q sp A) Yes, Q > Ksp B) No, Q sp C) No, Q = Ksp D) Yes, Q sp

Exam 17: Acid-Base Equilibria and Solubility Equilibria

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?

(Short Answer)

4.8/5

(77)

Question 61

Assuming equal concentrations of conjugate base and acid, which one of the following mixtures is suitable for making a buffer solution with an optimum pH of 9.2-9.3?

(Multiple Choice)

5.0/5

(71)

Question 62

Will a precipitate of magnesium fluoride form when 200. mL of 1.9 * 10^-3 M MgCl₂ are added to 300. mL of 1.4 * 10^-2 M NaF? [K_sp (MgF₂)= 6.9 * 10^-9]

(Multiple Choice)

4.9/5

(77)

Question 63

Calculate the silver ion concentration in a saturated solution of silver(I)carbonate (K_sp = 8.1 * 10^-12).

(Multiple Choice)

4.8/5

(86)

Question 64

What is the net ionic equation for the reaction that occurs when small amounts of hydrochloric acid are added to a HOCl/NaOCl buffer solution?

(Multiple Choice)

4.8/5

(85)

Question 65

You are asked to go into the lab and prepare an acetic acid - sodium acetate buffer solution with a pH of 4.00 ± 0.02. What molar ratio of CH₃COOH to CH₃COONa should be used?

(Multiple Choice)

4.8/5

(91)

Question 66

The molar solubility of tin(II)iodide is 1.28 * 10^-2 mol/L. What is K_sp for this compound?

(Multiple Choice)

4.8/5

(73)

Question 67

The molar solubility of magnesium carbonate is 1.8 * 10^-4 mol/L. What is K_sp for this compound?

(Multiple Choice)

4.8/5

(73)

Question 68

Assuming equal concentrations of conjugate base and acid, which one of the following mixtures is suitable for making a buffer solution with an optimum pH of 4.6-4.8?

(Multiple Choice)

4.8/5

(89)

Question 69

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)

4.9/5

(85)

Question 70

The solubility of a salt increases as its K_sp increases.

(True/False)

4.9/5

(89)

Question 71

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)

4.9/5

(73)

Question 72

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)

4.9/5

(95)

Question 73

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?

(Essay)

4.8/5

(91)

Question 74

Write an equation showing the net reaction that occurs when a strong acid 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)

4.8/5

(91)

Question 75

What mass of ammonium nitrate must be added to 350. mL of a 0.150 M solution of ammonia to give a buffer having a pH of 9.00? (K_b(NH₃)= 1.8 * 10^-5)

(Multiple Choice)

4.8/5

(83)

Question 76

Which of the following would decrease the K_sp for PbI₂?

(Multiple Choice)

4.9/5

(70)

Question 77

The solubility product for calcium phosphate is K_sp = 1.3 * 10^-26. What is the molar solubility of calcium phosphate?

(Multiple Choice)

4.9/5

(84)

Question 78

Find the concentration of calcium ions in a solution made by adding 3.50 g of calcium fluoride to 750. mL of 0.125 M NaF. [For CaF₂, K_sp = 3.95 * 10^-11.]

(Multiple Choice)

4.9/5

(68)

Question 79

What is the pH at the equivalence point in the titration of 100 mL of 0.10 M HCl with 0.10 M NaOH?

(Multiple Choice)

4.8/5

(79)

Question 80

Showing 61 - 80 of 92

Exam 17: Acid-Base Equilibria and Solubility Equilibria

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?

Assuming equal concentrations of conjugate base and acid, which one of the following mixtures is suitable for making a buffer solution with an optimum pH of 9.2-9.3?

Will a precipitate of magnesium fluoride form when 200. mL of 1.9 * 10-3 M MgCl2 are added to 300. mL of 1.4 * 10-2 M NaF? [Ksp (MgF2)= 6.9 * 10-9]

Calculate the silver ion concentration in a saturated solution of silver(I)carbonate (Ksp = 8.1 * 10-12).

What is the net ionic equation for the reaction that occurs when small amounts of hydrochloric acid are added to a HOCl/NaOCl buffer solution?

You are asked to go into the lab and prepare an acetic acid - sodium acetate buffer solution with a pH of 4.00 ± 0.02. What molar ratio of CH3COOH to CH3COONa should be used?

The molar solubility of tin(II)iodide is 1.28 * 10-2 mol/L. What is Ksp for this compound?

The molar solubility of magnesium carbonate is 1.8 * 10-4 mol/L. What is Ksp for this compound?

Assuming equal concentrations of conjugate base and acid, which one of the following mixtures is suitable for making a buffer solution with an optimum pH of 4.6-4.8?

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

The solubility of a salt increases as its Ksp increases.

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?

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]

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?

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

What mass of ammonium nitrate must be added to 350. mL of a 0.150 M solution of ammonia to give a buffer having a pH of 9.00? (Kb(NH3)= 1.8 * 10-5)

Which of the following would decrease the Ksp for PbI2?

The solubility product for calcium phosphate is Ksp = 1.3 * 10-26. What is the molar solubility of calcium phosphate?

Find the concentration of calcium ions in a solution made by adding 3.50 g of calcium fluoride to 750. mL of 0.125 M NaF. [For CaF2, Ksp = 3.95 * 10-11.]

What is the pH at the equivalence point in the titration of 100 mL of 0.10 M HCl with 0.10 M NaOH?

Introduction

Atoms, Molecules, and Ions

Stoichiometry

Reactions in Aqueous Solution

Gases

Energy Relationships in Chemical Reactions

The Electronic Structure of Atoms

The Periodic Table

Chemical Bonding I: the Covalent Bond

Chemical Bonding Ii: Molecular Geometry and Hybridization of Atomic Orbitals

Introduction to Organic Chemistry

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Thermodynamics

Redox Reactions and Electrochemistry

The Chemistry of Coordination Compounds

Nuclear Chemistry

Organic Polymerssynthetic and Natural

Filters

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?

Will a precipitate of magnesium fluoride form when 200. mL of 1.9 * 10^-3 M MgCl₂ are added to 300. mL of 1.4 * 10^-2 M NaF? [K_sp (MgF₂)= 6.9 * 10^-9]

Calculate the silver ion concentration in a saturated solution of silver(I)carbonate (K_sp = 8.1 * 10^-12).

You are asked to go into the lab and prepare an acetic acid - sodium acetate buffer solution with a pH of 4.00 ± 0.02. What molar ratio of CH₃COOH to CH₃COONa should be used?

The molar solubility of tin(II)iodide is 1.28 * 10^-2 mol/L. What is K_sp for this compound?

The molar solubility of magnesium carbonate is 1.8 * 10^-4 mol/L. What is K_sp for this compound?

The solubility of a salt increases as its K_sp increases.

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]

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?

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

What mass of ammonium nitrate must be added to 350. mL of a 0.150 M solution of ammonia to give a buffer having a pH of 9.00? (K_b(NH₃)= 1.8 * 10^-5)

Which of the following would decrease the K_sp for PbI₂?

The solubility product for calcium phosphate is K_sp = 1.3 * 10^-26. What is the molar solubility of calcium phosphate?

Find the concentration of calcium ions in a solution made by adding 3.50 g of calcium fluoride to 750. mL of 0.125 M NaF. [For CaF₂, K_sp = 3.95 * 10^-11.]