On adding aqueous Sodium hydroxide causes more P b S to dissolve, whether this affects or violate Le-Chatelier’s principle has to be explained. Concept Introduction: Le Chatelier’s principle: If equilibrium is disturbed by changing conditions, the system will move the equilibrium to reverse the change. The effect of concentration on chemical equilibria: Increasing the concentration of the reactant or decreasing the concentration of the products will favor the forward reaction, causing the equilibrium to shift to the right. Decreasing the concentration of the reactant or increasing the concentration of the products will favor the reverse reaction, causing the equilibrium to shift to the left.

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Answer 1

Question

Chapter 19, Problem 19.94P

Interpretation Introduction

Interpretation:

On adding aqueous Sodium hydroxide causes more PbS to dissolve, whether this affects or violate Le-Chatelier’s principle has to be explained.

Concept Introduction:

Le Chatelier’s principle: If equilibrium is disturbed by changing conditions, the system will move the equilibrium to reverse the change.

The effect of concentration on chemical equilibria:

Increasing the concentration of the reactant or decreasing the concentration of the products will favor the forward reaction, causing the equilibrium to shift to the right.

Decreasing the concentration of the reactant or increasing the concentration of the products will favor the reverse reaction, causing the equilibrium to shift to the left.

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Answer 2

Question

Chapter 19, Problem 19.94P

Interpretation Introduction

Interpretation:

On adding aqueous Sodium hydroxide causes more PbS to dissolve, whether this affects or violate Le-Chatelier’s principle has to be explained.

Concept Introduction:

Le Chatelier’s principle: If equilibrium is disturbed by changing conditions, the system will move the equilibrium to reverse the change.

The effect of concentration on chemical equilibria:

Increasing the concentration of the reactant or decreasing the concentration of the products will favor the forward reaction, causing the equilibrium to shift to the right.

Decreasing the concentration of the reactant or increasing the concentration of the products will favor the reverse reaction, causing the equilibrium to shift to the left.

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Answer 3

Question

Chapter 19, Problem 19.94P

Interpretation Introduction

Interpretation:

On adding aqueous Sodium hydroxide causes more PbS to dissolve, whether this affects or violate Le-Chatelier’s principle has to be explained.

Concept Introduction:

Le Chatelier’s principle: If equilibrium is disturbed by changing conditions, the system will move the equilibrium to reverse the change.

The effect of concentration on chemical equilibria:

Increasing the concentration of the reactant or decreasing the concentration of the products will favor the forward reaction, causing the equilibrium to shift to the right.

Decreasing the concentration of the reactant or increasing the concentration of the products will favor the reverse reaction, causing the equilibrium to shift to the left.

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Answer 4

Question

Chapter 19, Problem 19.94P

Interpretation Introduction

Interpretation:

On adding aqueous Sodium hydroxide causes more PbS to dissolve, whether this affects or violate Le-Chatelier’s principle has to be explained.

Concept Introduction:

Le Chatelier’s principle: If equilibrium is disturbed by changing conditions, the system will move the equilibrium to reverse the change.

The effect of concentration on chemical equilibria:

Increasing the concentration of the reactant or decreasing the concentration of the products will favor the forward reaction, causing the equilibrium to shift to the right.

Decreasing the concentration of the reactant or increasing the concentration of the products will favor the reverse reaction, causing the equilibrium to shift to the left.

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Answer 5

Chapter 19, Problem 19.94P

Interpretation Introduction

Interpretation:

On adding aqueous Sodium hydroxide causes more PbS to dissolve, whether this affects or violate Le-Chatelier’s principle has to be explained.

Concept Introduction:

Le Chatelier’s principle: If equilibrium is disturbed by changing conditions, the system will move the equilibrium to reverse the change.

The effect of concentration on chemical equilibria:

Increasing the concentration of the reactant or decreasing the concentration of the products will favor the forward reaction, causing the equilibrium to shift to the right.

Decreasing the concentration of the reactant or increasing the concentration of the products will favor the reverse reaction, causing the equilibrium to shift to the left.

Answer 6

Chapter 19, Problem 19.94P

Interpretation Introduction

Interpretation:

On adding aqueous Sodium hydroxide causes more PbS to dissolve, whether this affects or violate Le-Chatelier’s principle has to be explained.

Concept Introduction:

Le Chatelier’s principle: If equilibrium is disturbed by changing conditions, the system will move the equilibrium to reverse the change.

The effect of concentration on chemical equilibria:

Increasing the concentration of the reactant or decreasing the concentration of the products will favor the forward reaction, causing the equilibrium to shift to the right.

Decreasing the concentration of the reactant or increasing the concentration of the products will favor the reverse reaction, causing the equilibrium to shift to the left.

Answer 7

Chapter 19, Problem 19.94P

Interpretation Introduction

Interpretation:

On adding aqueous Sodium hydroxide causes more PbS to dissolve, whether this affects or violate Le-Chatelier’s principle has to be explained.

Concept Introduction:

Le Chatelier’s principle: If equilibrium is disturbed by changing conditions, the system will move the equilibrium to reverse the change.

The effect of concentration on chemical equilibria:

Increasing the concentration of the reactant or decreasing the concentration of the products will favor the forward reaction, causing the equilibrium to shift to the right.

Decreasing the concentration of the reactant or increasing the concentration of the products will favor the reverse reaction, causing the equilibrium to shift to the left.

Answer 8

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Answer 10

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Answer 11

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 - Prob. 19.5AFP Ch. 19.3 - Prob. 19.5BFP

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