(a) Interpretation: The net ionic equation for the precipitation of ( NH 4 ) 2 HPO 4 ( s ) should be given. Concept introduction: According to the Le Chatelier’s principle, a change in one of the variables that describe a system at equilibrium produces a shift in the position of the equilibrium that counteracts the effect of this change. Usually, diprotic and polyprotic acid dissociation is undergoes through several equilibrium steps.

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Answer 1

Question

Chapter 5, Problem 30E

Interpretation Introduction

(a)

Interpretation:

The net ionic equation for the precipitation of ( NH4)2HPO4(s) should be given.

Concept introduction:

According to the Le Chatelier’s principle, a change in one of the variables that describe a system at equilibrium produces a shift in the position of the equilibrium that counteracts the effect of this change.

Usually, diprotic and polyprotic acid dissociation is undergoes through several equilibrium steps.

Interpretation Introduction

(b)

Interpretation:

The net ionic equation for the precipitation of NH4NO2 should be given.

Concept introduction:

According to the Le Chatelier’s principle, a change in one of the variables that describe a system at equilibrium produces a shift in the position of the equilibrium that counteracts the effect of this change.

Usually, diprotic and polyprotic acid dissociation is undergoes through several equilibrium steps.

Interpretation Introduction

(c)

Interpretation:

The net ionic equation for the precipitation of ( NH4)2SO4 should be given.

Concept introduction:

Follow the lower-numbered guideline when two guidelines are in conflict. This leads to the correct prediction in most cases.

Salts of group 1 cations (with some exceptions for Li⁺) and the NH₄+ cation are soluble.

Nitrates, acetates, and perchlorates are soluble.

Salts of silver, lead, and mercury (I) are insoluble.

Chlorides, bromides, and iodides are soluble

Carbonates, phosphates, sulfides, oxides, and hydroxides are insoluble (sulfides of group 2 cations and hydroxides of Ca²⁺, Sr²⁺, and Ba²+ are slightly soluble).

Sulfates are soluble except for those of calcium, strontium, and barium.

There are only two possibilities. Either some cation−anion combination leads to an insoluble solid—a precipitate—or no such combination is possible, or there is no reaction at all.

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Answer 2

Question

Chapter 5, Problem 30E

Interpretation Introduction

(a)

Interpretation:

The net ionic equation for the precipitation of ( NH4)2HPO4(s) should be given.

Concept introduction:

According to the Le Chatelier’s principle, a change in one of the variables that describe a system at equilibrium produces a shift in the position of the equilibrium that counteracts the effect of this change.

Usually, diprotic and polyprotic acid dissociation is undergoes through several equilibrium steps.

Interpretation Introduction

(b)

Interpretation:

The net ionic equation for the precipitation of NH4NO2 should be given.

Concept introduction:

According to the Le Chatelier’s principle, a change in one of the variables that describe a system at equilibrium produces a shift in the position of the equilibrium that counteracts the effect of this change.

Usually, diprotic and polyprotic acid dissociation is undergoes through several equilibrium steps.

Interpretation Introduction

(c)

Interpretation:

The net ionic equation for the precipitation of ( NH4)2SO4 should be given.

Concept introduction:

Follow the lower-numbered guideline when two guidelines are in conflict. This leads to the correct prediction in most cases.

Salts of group 1 cations (with some exceptions for Li⁺) and the NH₄+ cation are soluble.

Nitrates, acetates, and perchlorates are soluble.

Salts of silver, lead, and mercury (I) are insoluble.

Chlorides, bromides, and iodides are soluble

Carbonates, phosphates, sulfides, oxides, and hydroxides are insoluble (sulfides of group 2 cations and hydroxides of Ca²⁺, Sr²⁺, and Ba²+ are slightly soluble).

Sulfates are soluble except for those of calcium, strontium, and barium.

There are only two possibilities. Either some cation−anion combination leads to an insoluble solid—a precipitate—or no such combination is possible, or there is no reaction at all.

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Answer 3

Question

Chapter 5, Problem 30E

Interpretation Introduction

(a)

Interpretation:

The net ionic equation for the precipitation of ( NH4)2HPO4(s) should be given.

Concept introduction:

According to the Le Chatelier’s principle, a change in one of the variables that describe a system at equilibrium produces a shift in the position of the equilibrium that counteracts the effect of this change.

Usually, diprotic and polyprotic acid dissociation is undergoes through several equilibrium steps.

Interpretation Introduction

(b)

Interpretation:

The net ionic equation for the precipitation of NH4NO2 should be given.

Concept introduction:

According to the Le Chatelier’s principle, a change in one of the variables that describe a system at equilibrium produces a shift in the position of the equilibrium that counteracts the effect of this change.

Usually, diprotic and polyprotic acid dissociation is undergoes through several equilibrium steps.

Interpretation Introduction

(c)

Interpretation:

The net ionic equation for the precipitation of ( NH4)2SO4 should be given.

Concept introduction:

Follow the lower-numbered guideline when two guidelines are in conflict. This leads to the correct prediction in most cases.

Salts of group 1 cations (with some exceptions for Li⁺) and the NH₄+ cation are soluble.

Nitrates, acetates, and perchlorates are soluble.

Salts of silver, lead, and mercury (I) are insoluble.

Chlorides, bromides, and iodides are soluble

Carbonates, phosphates, sulfides, oxides, and hydroxides are insoluble (sulfides of group 2 cations and hydroxides of Ca²⁺, Sr²⁺, and Ba²+ are slightly soluble).

Sulfates are soluble except for those of calcium, strontium, and barium.

There are only two possibilities. Either some cation−anion combination leads to an insoluble solid—a precipitate—or no such combination is possible, or there is no reaction at all.

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Answer 4

Question

Chapter 5, Problem 30E

Interpretation Introduction

(a)

Interpretation:

The net ionic equation for the precipitation of ( NH4)2HPO4(s) should be given.

Concept introduction:

According to the Le Chatelier’s principle, a change in one of the variables that describe a system at equilibrium produces a shift in the position of the equilibrium that counteracts the effect of this change.

Usually, diprotic and polyprotic acid dissociation is undergoes through several equilibrium steps.

Interpretation Introduction

(b)

Interpretation:

The net ionic equation for the precipitation of NH4NO2 should be given.

Concept introduction:

According to the Le Chatelier’s principle, a change in one of the variables that describe a system at equilibrium produces a shift in the position of the equilibrium that counteracts the effect of this change.

Usually, diprotic and polyprotic acid dissociation is undergoes through several equilibrium steps.

Interpretation Introduction

(c)

Interpretation:

The net ionic equation for the precipitation of ( NH4)2SO4 should be given.

Concept introduction:

Follow the lower-numbered guideline when two guidelines are in conflict. This leads to the correct prediction in most cases.

Salts of group 1 cations (with some exceptions for Li⁺) and the NH₄+ cation are soluble.

Nitrates, acetates, and perchlorates are soluble.

Salts of silver, lead, and mercury (I) are insoluble.

Chlorides, bromides, and iodides are soluble

Carbonates, phosphates, sulfides, oxides, and hydroxides are insoluble (sulfides of group 2 cations and hydroxides of Ca²⁺, Sr²⁺, and Ba²+ are slightly soluble).

Sulfates are soluble except for those of calcium, strontium, and barium.

There are only two possibilities. Either some cation−anion combination leads to an insoluble solid—a precipitate—or no such combination is possible, or there is no reaction at all.

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Answer 5

Chapter 5, Problem 30E

Interpretation Introduction

(a)

Interpretation:

The net ionic equation for the precipitation of ( NH4)2HPO4(s) should be given.

Concept introduction:

According to the Le Chatelier’s principle, a change in one of the variables that describe a system at equilibrium produces a shift in the position of the equilibrium that counteracts the effect of this change.

Usually, diprotic and polyprotic acid dissociation is undergoes through several equilibrium steps.

Interpretation Introduction

(b)

Interpretation:

The net ionic equation for the precipitation of NH4NO2 should be given.

Concept introduction:

According to the Le Chatelier’s principle, a change in one of the variables that describe a system at equilibrium produces a shift in the position of the equilibrium that counteracts the effect of this change.

Usually, diprotic and polyprotic acid dissociation is undergoes through several equilibrium steps.

Interpretation Introduction

(c)

Interpretation:

The net ionic equation for the precipitation of ( NH4)2SO4 should be given.

Concept introduction:

Follow the lower-numbered guideline when two guidelines are in conflict. This leads to the correct prediction in most cases.

Salts of group 1 cations (with some exceptions for Li⁺) and the NH₄+ cation are soluble.

Nitrates, acetates, and perchlorates are soluble.

Salts of silver, lead, and mercury (I) are insoluble.

Chlorides, bromides, and iodides are soluble

Carbonates, phosphates, sulfides, oxides, and hydroxides are insoluble (sulfides of group 2 cations and hydroxides of Ca²⁺, Sr²⁺, and Ba²+ are slightly soluble).

Sulfates are soluble except for those of calcium, strontium, and barium.

There are only two possibilities. Either some cation−anion combination leads to an insoluble solid—a precipitate—or no such combination is possible, or there is no reaction at all.

Answer 6

Chapter 5, Problem 30E

Interpretation Introduction

(a)

Interpretation:

The net ionic equation for the precipitation of ( NH4)2HPO4(s) should be given.

Concept introduction:

According to the Le Chatelier’s principle, a change in one of the variables that describe a system at equilibrium produces a shift in the position of the equilibrium that counteracts the effect of this change.

Usually, diprotic and polyprotic acid dissociation is undergoes through several equilibrium steps.

Answer 7

Chapter 5, Problem 30E

Interpretation Introduction

(a)

Interpretation:

The net ionic equation for the precipitation of ( NH4)2HPO4(s) should be given.

Concept introduction:

According to the Le Chatelier’s principle, a change in one of the variables that describe a system at equilibrium produces a shift in the position of the equilibrium that counteracts the effect of this change.

Usually, diprotic and polyprotic acid dissociation is undergoes through several equilibrium steps.

Answer 8

Interpretation Introduction

(b)

Interpretation:

The net ionic equation for the precipitation of NH4NO2 should be given.

Concept introduction:

According to the Le Chatelier’s principle, a change in one of the variables that describe a system at equilibrium produces a shift in the position of the equilibrium that counteracts the effect of this change.

Usually, diprotic and polyprotic acid dissociation is undergoes through several equilibrium steps.

Answer 9

Interpretation Introduction

(b)

Interpretation:

The net ionic equation for the precipitation of NH4NO2 should be given.

Concept introduction:

According to the Le Chatelier’s principle, a change in one of the variables that describe a system at equilibrium produces a shift in the position of the equilibrium that counteracts the effect of this change.

Usually, diprotic and polyprotic acid dissociation is undergoes through several equilibrium steps.

Answer 10

Interpretation Introduction

(c)

Interpretation:

The net ionic equation for the precipitation of ( NH4)2SO4 should be given.

Concept introduction:

Follow the lower-numbered guideline when two guidelines are in conflict. This leads to the correct prediction in most cases.

Salts of group 1 cations (with some exceptions for Li⁺) and the NH₄+ cation are soluble.

Nitrates, acetates, and perchlorates are soluble.

Salts of silver, lead, and mercury (I) are insoluble.

Chlorides, bromides, and iodides are soluble

Carbonates, phosphates, sulfides, oxides, and hydroxides are insoluble (sulfides of group 2 cations and hydroxides of Ca²⁺, Sr²⁺, and Ba²+ are slightly soluble).

Sulfates are soluble except for those of calcium, strontium, and barium.

There are only two possibilities. Either some cation−anion combination leads to an insoluble solid—a precipitate—or no such combination is possible, or there is no reaction at all.

Answer 11

Interpretation Introduction

(c)

Interpretation:

The net ionic equation for the precipitation of ( NH4)2SO4 should be given.

Concept introduction:

Follow the lower-numbered guideline when two guidelines are in conflict. This leads to the correct prediction in most cases.

Salts of group 1 cations (with some exceptions for Li⁺) and the NH₄+ cation are soluble.

Nitrates, acetates, and perchlorates are soluble.

Salts of silver, lead, and mercury (I) are insoluble.

Chlorides, bromides, and iodides are soluble

Carbonates, phosphates, sulfides, oxides, and hydroxides are insoluble (sulfides of group 2 cations and hydroxides of Ca²⁺, Sr²⁺, and Ba²+ are slightly soluble).

Sulfates are soluble except for those of calcium, strontium, and barium.

There are only two possibilities. Either some cation−anion combination leads to an insoluble solid—a precipitate—or no such combination is possible, or there is no reaction at all.

Answer 12

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Answer 13

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Answer 14

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Answer 15

Ch. 5 - Using information from this chapter, indicate...Ch. 5 - Select the (a) best and (b) poorest electrical...Ch. 5 - What response would you expect in the apparatus of...Ch. 5 - NH2(aq) conducts electric current only weakly. The...Ch. 5 - Sketches (a-c) are molecular views of the solute...Ch. 5 - Prob. 6E Ch. 5 - Determine the concentration of the ion indicated...Ch. 5 - Which solution has the greatest [SO42] ? a....Ch. 5 - A solution is prepared by dissolving...Ch. 5 - Prob. 10E

Solution Summary: The author explains the net ionic equation for the precipitation of leftNH_4).

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