The Ksp of AgCl is 1.7 × 10-10. How many moles of MnCl2 can be dissolved in one liter of a solution in which [AgNO3] = 3.4 × 10-4 M before a precipitate appears?

A) 5.0 × 10-7 mol B) 5.8 × 10-14 mol C) 2.4 × 10-7 mol D) 2.0 × 106 mol E) 2.5 × 10-7 mol A) 5.0 × 10-7 mol B) 5.8 × 10-14 mol C) 2.4 × 10-7 mol D) 2.0 × 106 mol E) 2.5 × 10-7 mol

A solution contains [Ba2+] = 5.0 × 10-5 M, [Ag+] = 3.0 × 10-5 M, and [Zn2+] = 2.0 × 10-7 M. Sodium oxalate is slowly added so that [C2O42-] increases. What is the concentration of the first cation to precipitate when the second cation just begins to precipitate?

A) 1.3 × 10-6 B) 2.2 × 10-6 C) 5.0 × 10-5 D) 1.35 × 10-9 E) 1.1 × 10-11 A) 1.3 × 10-6 B) 2.2 × 10-6 C) 5.0 × 10-5 D) 1.35 × 10-9 E) 1.1 × 10-11

In a qualitative cation analysis, the unknown ion is not precipitated by HCl or H2S, but is precipitated by CO32-. The unknown ion is ________.

A) Ag+ B) Mn2+ C) Ca2+ D) K+ E) Al3+ A) Ag+ B) Mn2+ C) Ca2+ D) K+ E) Al3+

Exam 18: Solubility and Complex-Ion Equilibria

Explore all topics

What molar concentration of silver ion could exist in a solution in which the concentration of CrO₄^2- is 1.0 × 10^-4 M? (Ksp of Ag₂CrO₄ = 1.1 × 10^-12)

(Multiple Choice)

4.8/5

(35)

Question 21

A small amount of solid calcium hydroxide is shaken vigorously in a test tube almost full of water until no further change occurs and most of the solid settles out. The resulting solution is:

(Multiple Choice)

4.8/5

(33)

Question 22

Write the solubility product constant expression for the following salt: CoS.

(Multiple Choice)

4.9/5

(44)

Question 23

A saturated solution of silver iodide has a concentration of 9.1 × 10^-9M. What is the Ksp of this compound?

(Multiple Choice)

4.9/5

(26)

Question 24

Which of the following reduces the solubility of calcium fluoride?

(Multiple Choice)

4.8/5

(35)

Question 25

What is the minimum pH at which cobalt(II) hydroxide [Ksp = 2.0 × 10^-16] will precipitate from a solution 0.020 M in CO₃²⁺?

(Multiple Choice)

4.7/5

(36)

Question 26

The Ksp of AgCl is 1.7 × 10^-10. How many moles of MnCl₂ can be dissolved in one liter of a solution in which [AgNO₃] = 3.4 × 10^-4 M before a precipitate appears?

(Multiple Choice)

4.7/5

(31)

Question 27

The molar solubility of calcium phosphate in a saturated aqueous solution of the salt is given by ________.

(Multiple Choice)

4.8/5

(36)

Question 28

Which of the following is most soluble?

(Multiple Choice)

4.7/5

(37)

Question 29

What is the molar solubility of barium carbonate in pure water? (Ksp = 5.1 × 10^-9)

(Multiple Choice)

4.7/5

(37)

Question 30

What is the minimum concentration of CN- that will prevent the precipitation of AgX(s) from a solution that is 0.149 M in X-(aq) and 0.0184 M in Ag⁺(aq)? (Ksp for AgX(s) = 5.2 × 10^-17; Kf for Ag(CN)^2- = 5.6 × 10¹⁸)

(Multiple Choice)

4.9/5

(34)

Question 31

The diverse ion effect is also called the salt effect.

(True/False)

4.9/5

(45)

Question 32

A solution contains [Ba²⁺] = 5.0 × 10^-5 M, [Ag⁺] = 3.0 × 10^-5 M, and [Zn²⁺] = 2.0 × 10^-7 M. Sodium oxalate is slowly added so that [C₂O₄^2-] increases. What is the concentration of the first cation to precipitate when the second cation just begins to precipitate?

(Multiple Choice)

4.9/5

(37)

Question 33

Fractional precipitation is a method to precipitate only part of the concentration of an ion.

(True/False)

4.9/5

(37)

Question 34

Ion pairs as a limitation to Ksp are more likely to be a problem with NaCl than with MgSO₄.

(True/False)

4.9/5

(41)

Question 35

The solubility of CaF₂ is 0.00021 mole per liter. What is the solubility product constant for CaF₂?

(Multiple Choice)

4.8/5

(29)

Question 36

What is the molar solubility of PbI2 (Ksp = 7.1 × 10^-9) in 0.10 M Pb(NO₃)₂?

(Multiple Choice)

4.9/5

(32)

Question 37

Consider an aqueous solution which is 0.020 M in Pb²⁺ and 0.20 M in Ag⁺. If concentrated potassium iodide solution (so that volume changes may be neglected) is added gradually with good stirring to this solution, which precipitate will form first? Ksp for PbI2 = 7.1 × 10^-9; for AgI = 8.31 × 10^-17

(Multiple Choice)

4.8/5

(34)

Question 38

Predict the molar solubility of the following salt in a solution that contains the given concentration of one of its ions: AgI; [I-] = 7.2 × 10^-6 M; Ksp = 8.5 × 10^-17

(Multiple Choice)

5.0/5

(37)

Question 39

In a qualitative cation analysis, the unknown ion is not precipitated by HCl or H₂S, but is precipitated by CO₃^2-. The unknown ion is ________.

(Multiple Choice)

4.9/5

(45)

Question 40

Showing 21 - 40 of 95

Exam 18: Solubility and Complex-Ion Equilibria

What molar concentration of silver ion could exist in a solution in which the concentration of CrO42- is 1.0 × 10-4 M? (Ksp of Ag2CrO4 = 1.1 × 10-12)

A small amount of solid calcium hydroxide is shaken vigorously in a test tube almost full of water until no further change occurs and most of the solid settles out. The resulting solution is:

Write the solubility product constant expression for the following salt: CoS.

A saturated solution of silver iodide has a concentration of 9.1 × 10-9 M. What is the Ksp of this compound?

Which of the following reduces the solubility of calcium fluoride?

What is the minimum pH at which cobalt(II) hydroxide [Ksp = 2.0 × 10-16] will precipitate from a solution 0.020 M in CO32+?

The Ksp of AgCl is 1.7 × 10-10. How many moles of MnCl2 can be dissolved in one liter of a solution in which [AgNO3] = 3.4 × 10-4 M before a precipitate appears?

The molar solubility of calcium phosphate in a saturated aqueous solution of the salt is given by ________.

Which of the following is most soluble?

What is the molar solubility of barium carbonate in pure water? (Ksp = 5.1 × 10-9)

What is the minimum concentration of CN- that will prevent the precipitation of AgX(s) from a solution that is 0.149 M in X-(aq) and 0.0184 M in Ag+(aq)? (Ksp for AgX(s) = 5.2 × 10-17; Kf for Ag(CN)2- = 5.6 × 1018)

The diverse ion effect is also called the salt effect.

A solution contains [Ba2+] = 5.0 × 10-5 M, [Ag+] = 3.0 × 10-5 M, and [Zn2+] = 2.0 × 10-7 M. Sodium oxalate is slowly added so that [C2O42-] increases. What is the concentration of the first cation to precipitate when the second cation just begins to precipitate?

Fractional precipitation is a method to precipitate only part of the concentration of an ion.

Ion pairs as a limitation to Ksp are more likely to be a problem with NaCl than with MgSO4.

The solubility of CaF2 is 0.00021 mole per liter. What is the solubility product constant for CaF2?

What is the molar solubility of PbI2 (Ksp = 7.1 × 10-9) in 0.10 M Pb(NO3)2?

Consider an aqueous solution which is 0.020 M in Pb2+ and 0.20 M in Ag+. If concentrated potassium iodide solution (so that volume changes may be neglected) is added gradually with good stirring to this solution, which precipitate will form first? Ksp for PbI2 = 7.1 × 10-9; for AgI = 8.31 × 10-17

Predict the molar solubility of the following salt in a solution that contains the given concentration of one of its ions: AgI; [I-] = 7.2 × 10-6 M; Ksp = 8.5 × 10-17

In a qualitative cation analysis, the unknown ion is not precipitated by HCl or H2S, but is precipitated by CO32-. The unknown ion is ________.

Matter - Its Properties and Measurement

Atoms and the Atomic Theory

Chemical Compounds

Chemical Reactions

Introduction to Reactions in Aqueous Solutions

Gases

Thermochemistry

Electrons in Atoms

The Periodic Table and Some Atomic Properties

Chemical Bonding I: Basic Concepts

Chemical Bonding II: Additional Aspects

Intermolecular Forces: Liquids and Solids

Solutions and Their Physical Properties

Chemical Kinetics

Principles of Chemical Equilibrium

Acids and Bases

Additional Aspects of Acid-Base Equilibria

Spontaneous Change: Entropy and Free Energy

Electrochemistry

Main Group Elements I: Groups 1, 2, 13, and 14

Main Group Elements II: Groups 18, 17, 16, 15, and Hydrogen

The Transition Elements

Complex Ions and Coordination Compounds

Nuclear Chemistry 1-41

Structures of Organic Compounds

Reactions of Organic Compounds

Chemistry of the Living State

Filters

What molar concentration of silver ion could exist in a solution in which the concentration of CrO₄^2- is 1.0 × 10^-4 M? (Ksp of Ag₂CrO₄ = 1.1 × 10^-12)

A saturated solution of silver iodide has a concentration of 9.1 × 10^-9M. What is the Ksp of this compound?

What is the minimum pH at which cobalt(II) hydroxide [Ksp = 2.0 × 10^-16] will precipitate from a solution 0.020 M in CO₃²⁺?

The Ksp of AgCl is 1.7 × 10^-10. How many moles of MnCl₂ can be dissolved in one liter of a solution in which [AgNO₃] = 3.4 × 10^-4 M before a precipitate appears?

What is the molar solubility of barium carbonate in pure water? (Ksp = 5.1 × 10^-9)

What is the minimum concentration of CN- that will prevent the precipitation of AgX(s) from a solution that is 0.149 M in X-(aq) and 0.0184 M in Ag⁺(aq)? (Ksp for AgX(s) = 5.2 × 10^-17; Kf for Ag(CN)^2- = 5.6 × 10¹⁸)

A solution contains [Ba²⁺] = 5.0 × 10^-5 M, [Ag⁺] = 3.0 × 10^-5 M, and [Zn²⁺] = 2.0 × 10^-7 M. Sodium oxalate is slowly added so that [C₂O₄^2-] increases. What is the concentration of the first cation to precipitate when the second cation just begins to precipitate?

Ion pairs as a limitation to Ksp are more likely to be a problem with NaCl than with MgSO₄.

The solubility of CaF₂ is 0.00021 mole per liter. What is the solubility product constant for CaF₂?

What is the molar solubility of PbI2 (Ksp = 7.1 × 10^-9) in 0.10 M Pb(NO₃)₂?

Predict the molar solubility of the following salt in a solution that contains the given concentration of one of its ions: AgI; [I-] = 7.2 × 10^-6 M; Ksp = 8.5 × 10^-17

In a qualitative cation analysis, the unknown ion is not precipitated by HCl or H₂S, but is precipitated by CO₃^2-. The unknown ion is ________.