Among the given solvents, which solvent should be taken in order to dissolve the maximum amount of C a F 2 ( K s p = 3.2 × 10 − 11 ) to make 1 L of aqueous solution has to be determined. Concept Introduction: Effect of a Common ion on solubility: The addition of a common ion decreases the solubility of a slightly soluble ionic compound. Le Chatelier's principle: Le Chatelier's principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change to reestablish equilibrium.

Question

What is the [OH⁻] of a 1.80 M solution of pyridine (C₅H₅N, Kb = 1.70 × 10⁻⁹)?

Answer 1

Question

Chapter 19, Problem 19.128P

(a)

Interpretation Introduction

Interpretation:

Among the given solvents, which solvent should be taken in order to dissolve the maximum amount of CaF2(Ksp = 3.2×10−11) to make 1 L of aqueous solution has to be determined.

Concept Introduction:

Effect of a Common ion on solubility:

The addition of a common ion decreases the solubility of a slightly soluble ionic compound.

Le Chatelier's principle:

Le Chatelier's principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change to reestablish equilibrium.

(b)

Interpretation Introduction

Interpretation:

Among the given solvents, which solvent should be taken in order to dissolve the least amount of CaF2(Ksp = 3.2×10−11) to make 1 L of aqueous solution has to be determined.

Concept Introduction:

Effect of a Common ion on solubility:

The addition of a common ion decreases the solubility of a slightly soluble ionic compound.

Le Chatelier's principle:

Le Chatelier's principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change to reestablish equilibrium.

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Answer 2

Question

Chapter 19, Problem 19.128P

(a)

Interpretation Introduction

Interpretation:

Among the given solvents, which solvent should be taken in order to dissolve the maximum amount of CaF2(Ksp = 3.2×10−11) to make 1 L of aqueous solution has to be determined.

Concept Introduction:

Effect of a Common ion on solubility:

The addition of a common ion decreases the solubility of a slightly soluble ionic compound.

Le Chatelier's principle:

Le Chatelier's principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change to reestablish equilibrium.

(b)

Interpretation Introduction

Interpretation:

Among the given solvents, which solvent should be taken in order to dissolve the least amount of CaF2(Ksp = 3.2×10−11) to make 1 L of aqueous solution has to be determined.

Concept Introduction:

Effect of a Common ion on solubility:

The addition of a common ion decreases the solubility of a slightly soluble ionic compound.

Le Chatelier's principle:

Le Chatelier's principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change to reestablish equilibrium.

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Answer 3

Question

Chapter 19, Problem 19.128P

(a)

Interpretation Introduction

Interpretation:

Among the given solvents, which solvent should be taken in order to dissolve the maximum amount of CaF2(Ksp = 3.2×10−11) to make 1 L of aqueous solution has to be determined.

Concept Introduction:

Effect of a Common ion on solubility:

The addition of a common ion decreases the solubility of a slightly soluble ionic compound.

Le Chatelier's principle:

Le Chatelier's principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change to reestablish equilibrium.

(b)

Interpretation Introduction

Interpretation:

Among the given solvents, which solvent should be taken in order to dissolve the least amount of CaF2(Ksp = 3.2×10−11) to make 1 L of aqueous solution has to be determined.

Concept Introduction:

Effect of a Common ion on solubility:

The addition of a common ion decreases the solubility of a slightly soluble ionic compound.

Le Chatelier's principle:

Le Chatelier's principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change to reestablish equilibrium.

Expert Solution & Answer

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Answer 4

Question

Chapter 19, Problem 19.128P

(a)

Interpretation Introduction

Interpretation:

Among the given solvents, which solvent should be taken in order to dissolve the maximum amount of CaF2(Ksp = 3.2×10−11) to make 1 L of aqueous solution has to be determined.

Concept Introduction:

Effect of a Common ion on solubility:

The addition of a common ion decreases the solubility of a slightly soluble ionic compound.

Le Chatelier's principle:

Le Chatelier's principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change to reestablish equilibrium.

(b)

Interpretation Introduction

Interpretation:

Among the given solvents, which solvent should be taken in order to dissolve the least amount of CaF2(Ksp = 3.2×10−11) to make 1 L of aqueous solution has to be determined.

Concept Introduction:

Effect of a Common ion on solubility:

The addition of a common ion decreases the solubility of a slightly soluble ionic compound.

Le Chatelier's principle:

Le Chatelier's principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change to reestablish equilibrium.

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Answer 5

Chapter 19, Problem 19.128P

(a)

Interpretation Introduction

Interpretation:

Among the given solvents, which solvent should be taken in order to dissolve the maximum amount of CaF2(Ksp = 3.2×10−11) to make 1 L of aqueous solution has to be determined.

Concept Introduction:

Effect of a Common ion on solubility:

The addition of a common ion decreases the solubility of a slightly soluble ionic compound.

Le Chatelier's principle:

Le Chatelier's principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change to reestablish equilibrium.

(b)

Interpretation Introduction

Interpretation:

Among the given solvents, which solvent should be taken in order to dissolve the least amount of CaF2(Ksp = 3.2×10−11) to make 1 L of aqueous solution has to be determined.

Concept Introduction:

Effect of a Common ion on solubility:

The addition of a common ion decreases the solubility of a slightly soluble ionic compound.

Le Chatelier's principle:

Le Chatelier's principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change to reestablish equilibrium.

Answer 6

Chapter 19, Problem 19.128P

(a)

Interpretation Introduction

Interpretation:

Among the given solvents, which solvent should be taken in order to dissolve the maximum amount of CaF2(Ksp = 3.2×10−11) to make 1 L of aqueous solution has to be determined.

Concept Introduction:

Effect of a Common ion on solubility:

The addition of a common ion decreases the solubility of a slightly soluble ionic compound.

Le Chatelier's principle:

Le Chatelier's principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change to reestablish equilibrium.

Answer 7

Chapter 19, Problem 19.128P

(a)

Interpretation Introduction

Interpretation:

Among the given solvents, which solvent should be taken in order to dissolve the maximum amount of CaF2(Ksp = 3.2×10−11) to make 1 L of aqueous solution has to be determined.

Concept Introduction:

Effect of a Common ion on solubility:

The addition of a common ion decreases the solubility of a slightly soluble ionic compound.

Le Chatelier's principle:

Le Chatelier's principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change to reestablish equilibrium.

Answer 8

(b)

Interpretation Introduction

Interpretation:

Among the given solvents, which solvent should be taken in order to dissolve the least amount of CaF2(Ksp = 3.2×10−11) to make 1 L of aqueous solution has to be determined.

Concept Introduction:

Effect of a Common ion on solubility:

The addition of a common ion decreases the solubility of a slightly soluble ionic compound.

Le Chatelier's principle:

Le Chatelier's principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change to reestablish equilibrium.

Answer 9

(b)

Interpretation Introduction

Interpretation:

Among the given solvents, which solvent should be taken in order to dissolve the least amount of CaF2(Ksp = 3.2×10−11) to make 1 L of aqueous solution has to be determined.

Concept Introduction:

Effect of a Common ion on solubility:

The addition of a common ion decreases the solubility of a slightly soluble ionic compound.

Le Chatelier's principle:

Le Chatelier's principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change to reestablish equilibrium.

Answer 10

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Answer 11

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Answer 21

Ch. 19.1 - Calculate the pH of a buffer consisting of 0.50 M...Ch. 19.1 - Prob. 19.1BFP Ch. 19.1 - Prob. 19.2AFP Ch. 19.1 - The molecular scenes below show three samples of a...Ch. 19.1 - Prob. 19.3AFP Ch. 19.1 - What is the component concentration ratio, [NH3]/...Ch. 19.2 - A chemist titrates 20.00 mL of 0.2000 M HBrO (Ka =...Ch. 19.2 - For the titration of 30.00 mL of 0.1000 M benzoic...Ch. 19.3 - Write the ion-product expression at equilibrium...Ch. 19.3 - Prob. 19.5BFP

Chapter 19 Solutions