Reason for formation of precipitate of NaCl when HCl gas is passed into a saturated NaCl has to be determined. Concept Introduction: Addition of similar type of ion in partially soluble salt is termed as common ion effect. The common ion present in it decides the shift of equilibrium according to Le Chatelier’s principle. According to this principle with increase in concentration of reactants reaction moves towards forward direction thus this increases concentration of products. Whereas with increase in concentration of product reaction shifts towards reverse direction. This increases the concentration of reactants.

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Answer 1

Question

Chapter 16, Problem 23RQ

Interpretation Introduction

Interpretation:

Reason for formation of precipitate of NaCl when HCl gas is passed into a saturated NaCl has to be determined.

Concept Introduction:

Addition of similar type of ion in partially soluble salt is termed as common ion effect. The common ion present in it decides the shift of equilibrium according to Le Chatelier’s principle. According to this principle with increase in concentration of reactants reaction moves towards forward direction thus this increases concentration of products. Whereas with increase in concentration of product reaction shifts towards reverse direction. This increases the concentration of reactants.

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Answer 2

Question

Chapter 16, Problem 23RQ

Interpretation Introduction

Interpretation:

Reason for formation of precipitate of NaCl when HCl gas is passed into a saturated NaCl has to be determined.

Concept Introduction:

Addition of similar type of ion in partially soluble salt is termed as common ion effect. The common ion present in it decides the shift of equilibrium according to Le Chatelier’s principle. According to this principle with increase in concentration of reactants reaction moves towards forward direction thus this increases concentration of products. Whereas with increase in concentration of product reaction shifts towards reverse direction. This increases the concentration of reactants.

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Answer 3

Question

Chapter 16, Problem 23RQ

Interpretation Introduction

Interpretation:

Reason for formation of precipitate of NaCl when HCl gas is passed into a saturated NaCl has to be determined.

Concept Introduction:

Addition of similar type of ion in partially soluble salt is termed as common ion effect. The common ion present in it decides the shift of equilibrium according to Le Chatelier’s principle. According to this principle with increase in concentration of reactants reaction moves towards forward direction thus this increases concentration of products. Whereas with increase in concentration of product reaction shifts towards reverse direction. This increases the concentration of reactants.

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Answer 4

Question

Chapter 16, Problem 23RQ

Interpretation Introduction

Interpretation:

Reason for formation of precipitate of NaCl when HCl gas is passed into a saturated NaCl has to be determined.

Concept Introduction:

Addition of similar type of ion in partially soluble salt is termed as common ion effect. The common ion present in it decides the shift of equilibrium according to Le Chatelier’s principle. According to this principle with increase in concentration of reactants reaction moves towards forward direction thus this increases concentration of products. Whereas with increase in concentration of product reaction shifts towards reverse direction. This increases the concentration of reactants.

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Answer 5

Chapter 16, Problem 23RQ

Interpretation Introduction

Interpretation:

Reason for formation of precipitate of NaCl when HCl gas is passed into a saturated NaCl has to be determined.

Concept Introduction:

Addition of similar type of ion in partially soluble salt is termed as common ion effect. The common ion present in it decides the shift of equilibrium according to Le Chatelier’s principle. According to this principle with increase in concentration of reactants reaction moves towards forward direction thus this increases concentration of products. Whereas with increase in concentration of product reaction shifts towards reverse direction. This increases the concentration of reactants.

Answer 6

Chapter 16, Problem 23RQ

Interpretation Introduction

Interpretation:

Reason for formation of precipitate of NaCl when HCl gas is passed into a saturated NaCl has to be determined.

Concept Introduction:

Addition of similar type of ion in partially soluble salt is termed as common ion effect. The common ion present in it decides the shift of equilibrium according to Le Chatelier’s principle. According to this principle with increase in concentration of reactants reaction moves towards forward direction thus this increases concentration of products. Whereas with increase in concentration of product reaction shifts towards reverse direction. This increases the concentration of reactants.

Answer 7

Chapter 16, Problem 23RQ

Interpretation Introduction

Interpretation:

Reason for formation of precipitate of NaCl when HCl gas is passed into a saturated NaCl has to be determined.

Concept Introduction:

Addition of similar type of ion in partially soluble salt is termed as common ion effect. The common ion present in it decides the shift of equilibrium according to Le Chatelier’s principle. According to this principle with increase in concentration of reactants reaction moves towards forward direction thus this increases concentration of products. Whereas with increase in concentration of product reaction shifts towards reverse direction. This increases the concentration of reactants.

Answer 8

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Answer 10

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Answer 11

Ch. 16.1 - Prob. 16.1P Ch. 16.2 - Prob. 16.2P Ch. 16.3 - Prob. 16.3P Ch. 16.3 - Prob. 16.4P Ch. 16.3 - Prob. 16.5P Ch. 16.3 - Prob. 16.6P Ch. 16.4 - Prob. 16.7P Ch. 16.4 - Prob. 16.8P Ch. 16.5 - Prob. 16.9P Ch. 16.5 - Prob. 16.10P

Solution Summary: The author explains the common ion effect, which determines the shift of equilibrium according to Le Chatelier's principle.

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