The precipitation reaction should be given from given process and formula of the precipitate should be given. Concept introduction: Precipitation reaction: The precipitate is formed, when the two solutions mixed together is called precipitation reaction and precipitate is a insoluble new product of reaction of two solutions. Solubility guideline: Compound containing alkali metal cations and ammonium ion are soluble in water. Compound contains nitrate, acetate and chlorate ions are soluble in water. Except Ag + , Hg 2+ and pb 2+ ions , compounds containing chloride, bromide and iodide ions are soluble in water. Except Ag + , Hg 2+ , pb 2+ , Ca 2+ , Sr 2+ and Ba 2+ ions, compounds containing sulfate ion are soluble. Except Li + , Na + , K + , Rb + , Cs + and NH 4 + ions, compounds containing carbonate, phosphate, chromate and sulfite ions are insoluble in water. Except Li + , Na + , K + , Rb + , Cs + and Ba 2+ ions, compounds containing hydroxide ions are insoluble in water.

Question

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Answer 1

Question

Chapter 9, Problem 9.24QP

(a)

Interpretation Introduction

Interpretation:

The precipitation reaction should be given from given process and formula of the precipitate should be given.

Concept introduction:

Precipitation reaction:

The precipitate is formed, when the two solutions mixed together is called precipitation reaction and precipitate is a insoluble new product of reaction of two solutions.

Solubility guideline:

Compound containing alkali metal cations and ammonium ion are soluble in water.

Compound contains nitrate, acetate and chlorate ions are soluble in water.

Except $Ag+$ , $Hg2+$ and $pb2+$ ions , compounds containing chloride, bromide and iodide ions are soluble in water.

Except $Ag+$ , $Hg2+$ , $pb2+$ , $Ca2+$ , $Sr2+$ and $Ba2+$ ions, compounds containing sulfate ion are soluble.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $NH4+$ ions, compounds containing carbonate, phosphate, chromate and sulfite ions are insoluble in water.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $Ba2+$ ions, compounds containing hydroxide ions are insoluble in water.

(a)

Expert Solution

Answer to Problem 9.24QP

The water solubility of given compounds are,

$Fe(OH)3(s)$ precipitate is formed.

Explanation of Solution

The balanced equation for reaction of $FeCl3(aq)$ and $LiOH(aq)$ is,

$FeCl3(aq)+3LiOH(aq)→Fe(OH)3(s)↓+3LiCl(aq)$

According to the solubility guideline, $Fe(OH)3$ is contains hydroxide ion so it is insoluble in water so it get precipitated.

(b)

Interpretation Introduction

Interpretation:

The precipitation reaction should be given from given process and formula of the precipitate should be given.

Concept introduction:

Precipitation reaction:

The precipitate is formed, when the two solutions mixed together is called precipitation reaction and precipitate is a insoluble new product of reaction of two solutions.

Solubility guideline:

Compound containing alkali metal cations and ammonium ion are soluble in water.

Compound contains nitrate, acetate and chlorate ions are soluble in water.

Except $Ag+$ , $Hg2+$ and $pb2+$ ions , compounds containing chloride, bromide and iodide ions are soluble in water.

Except $Ag+$ , $Hg2+$ , $pb2+$ , $Ca2+$ , $Sr2+$ and $Ba2+$ ions, compounds containing sulfate ion are soluble.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $NH4+$ ions, compounds containing carbonate, phosphate, chromate and sulfite ions are insoluble in water.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $Ba2+$ ions, compounds containing hydroxide ions are insoluble in water.

(b)

Expert Solution

Answer to Problem 9.24QP

The water solubility of given compounds are,

It is not a precipitation reaction

Explanation of Solution

The balanced equation for reaction of $KNO3(aq)$ and $CaCl2(aq)$ is,

$2KNO3(aq)+CaCl2(aq)→Ca(NO3)2(aq)+2KCl(aq)$

According to the solubility guideline, $Ca(NO3)2(aq) and 2KCl(aq)$ soluble in water there is no precipitation take place so not precipitated formed.

(c)

Interpretation Introduction

Interpretation:

The precipitation reaction should be given from given process and formula of the precipitate should be given.

Concept introduction:

Precipitation reaction:

The precipitate is formed, when the two solutions mixed together is called precipitation reaction and precipitate is a insoluble new product of reaction of two solutions.

Solubility guideline:

Compound containing alkali metal cations and ammonium ion are soluble in water.

Compound contains nitrate, acetate and chlorate ions are soluble in water.

Except $Ag+$ , $Hg2+$ and $pb2+$ ions , compounds containing chloride, bromide and iodide ions are soluble in water.

Except $Ag+$ , $Hg2+$ , $pb2+$ , $Ca2+$ , $Sr2+$ and $Ba2+$ ions, compounds containing sulfate ion are soluble.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $NH4+$ ions, compounds containing carbonate, phosphate, chromate and sulfite ions are insoluble in water.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $Ba2+$ ions, compounds containing hydroxide ions are insoluble in water.

(c)

Expert Solution

Answer to Problem 9.24QP

The water solubility of given compounds are,

It is not a precipitation reaction

Explanation of Solution

The balanced equation for reaction of $(NH4)2CO3(aq)$ and $NaCO3(aq)$ is,

$(NH4)2CO3(aq)+Na2CO3(aq)→(NH4)2CO3(aq)+Na2CO3(aq)$

No reaction takes place so no new product formed.

(d)

Interpretation Introduction

Interpretation:

The precipitation reaction should be given from given process and formula of the precipitate should be given.

Concept introduction:

Precipitation reaction:

The precipitate is formed, when the two solutions mixed together is called precipitation reaction and precipitate is a insoluble new product of reaction of two solutions.

Solubility guideline:

Compound containing alkali metal cations and ammonium ion are soluble in water.

Compound contains nitrate, acetate and chlorate ions are soluble in water.

Except $Ag+$ , $Hg2+$ and $pb2+$ ions , compounds containing chloride, bromide and iodide ions are soluble in water.

Except $Ag+$ , $Hg2+$ , $pb2+$ , $Ca2+$ , $Sr2+$ and $Ba2+$ ions, compounds containing sulfate ion are soluble.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $NH4+$ ions, compounds containing carbonate, phosphate, chromate and sulfite ions are insoluble in water.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $Ba2+$ ions, compounds containing hydroxide ions are insoluble in water.

(d)

Expert Solution

Answer to Problem 9.24QP

The water solubility of given compounds are,

$Sr(OH)2(s)$ precipitate is formed.

Explanation of Solution

The balanced equation for reaction of $Sr(NO3)2(aq)$ and $Ca(OH)2(aq)$ is,

$Sr(NO3)2(aq)+Ca(OH)2(aq)→Sr(OH)2(s)↓+Ca(NO3)2(aq)$

According to the solubility guideline, $Sr(OH)2(s)$ is contains hydroxide ion so it is insoluble in water so it get precipitated.

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Answer 2

Question

Chapter 9, Problem 9.24QP

(a)

Interpretation Introduction

Interpretation:

The precipitation reaction should be given from given process and formula of the precipitate should be given.

Concept introduction:

Precipitation reaction:

The precipitate is formed, when the two solutions mixed together is called precipitation reaction and precipitate is a insoluble new product of reaction of two solutions.

Solubility guideline:

Compound containing alkali metal cations and ammonium ion are soluble in water.

Compound contains nitrate, acetate and chlorate ions are soluble in water.

Except $Ag+$ , $Hg2+$ and $pb2+$ ions , compounds containing chloride, bromide and iodide ions are soluble in water.

Except $Ag+$ , $Hg2+$ , $pb2+$ , $Ca2+$ , $Sr2+$ and $Ba2+$ ions, compounds containing sulfate ion are soluble.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $NH4+$ ions, compounds containing carbonate, phosphate, chromate and sulfite ions are insoluble in water.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $Ba2+$ ions, compounds containing hydroxide ions are insoluble in water.

(a)

Expert Solution

Answer to Problem 9.24QP

The water solubility of given compounds are,

$Fe(OH)3(s)$ precipitate is formed.

Explanation of Solution

The balanced equation for reaction of $FeCl3(aq)$ and $LiOH(aq)$ is,

$FeCl3(aq)+3LiOH(aq)→Fe(OH)3(s)↓+3LiCl(aq)$

According to the solubility guideline, $Fe(OH)3$ is contains hydroxide ion so it is insoluble in water so it get precipitated.

(b)

Interpretation Introduction

Interpretation:

The precipitation reaction should be given from given process and formula of the precipitate should be given.

Concept introduction:

Precipitation reaction:

The precipitate is formed, when the two solutions mixed together is called precipitation reaction and precipitate is a insoluble new product of reaction of two solutions.

Solubility guideline:

Compound containing alkali metal cations and ammonium ion are soluble in water.

Compound contains nitrate, acetate and chlorate ions are soluble in water.

Except $Ag+$ , $Hg2+$ and $pb2+$ ions , compounds containing chloride, bromide and iodide ions are soluble in water.

Except $Ag+$ , $Hg2+$ , $pb2+$ , $Ca2+$ , $Sr2+$ and $Ba2+$ ions, compounds containing sulfate ion are soluble.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $NH4+$ ions, compounds containing carbonate, phosphate, chromate and sulfite ions are insoluble in water.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $Ba2+$ ions, compounds containing hydroxide ions are insoluble in water.

(b)

Expert Solution

Answer to Problem 9.24QP

The water solubility of given compounds are,

It is not a precipitation reaction

Explanation of Solution

The balanced equation for reaction of $KNO3(aq)$ and $CaCl2(aq)$ is,

$2KNO3(aq)+CaCl2(aq)→Ca(NO3)2(aq)+2KCl(aq)$

According to the solubility guideline, $Ca(NO3)2(aq) and 2KCl(aq)$ soluble in water there is no precipitation take place so not precipitated formed.

(c)

Interpretation Introduction

Interpretation:

The precipitation reaction should be given from given process and formula of the precipitate should be given.

Concept introduction:

Precipitation reaction:

The precipitate is formed, when the two solutions mixed together is called precipitation reaction and precipitate is a insoluble new product of reaction of two solutions.

Solubility guideline:

Compound containing alkali metal cations and ammonium ion are soluble in water.

Compound contains nitrate, acetate and chlorate ions are soluble in water.

Except $Ag+$ , $Hg2+$ and $pb2+$ ions , compounds containing chloride, bromide and iodide ions are soluble in water.

Except $Ag+$ , $Hg2+$ , $pb2+$ , $Ca2+$ , $Sr2+$ and $Ba2+$ ions, compounds containing sulfate ion are soluble.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $NH4+$ ions, compounds containing carbonate, phosphate, chromate and sulfite ions are insoluble in water.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $Ba2+$ ions, compounds containing hydroxide ions are insoluble in water.

(c)

Expert Solution

Answer to Problem 9.24QP

The water solubility of given compounds are,

It is not a precipitation reaction

Explanation of Solution

The balanced equation for reaction of $(NH4)2CO3(aq)$ and $NaCO3(aq)$ is,

$(NH4)2CO3(aq)+Na2CO3(aq)→(NH4)2CO3(aq)+Na2CO3(aq)$

No reaction takes place so no new product formed.

(d)

Interpretation Introduction

Interpretation:

The precipitation reaction should be given from given process and formula of the precipitate should be given.

Concept introduction:

Precipitation reaction:

The precipitate is formed, when the two solutions mixed together is called precipitation reaction and precipitate is a insoluble new product of reaction of two solutions.

Solubility guideline:

Compound containing alkali metal cations and ammonium ion are soluble in water.

Compound contains nitrate, acetate and chlorate ions are soluble in water.

Except $Ag+$ , $Hg2+$ and $pb2+$ ions , compounds containing chloride, bromide and iodide ions are soluble in water.

Except $Ag+$ , $Hg2+$ , $pb2+$ , $Ca2+$ , $Sr2+$ and $Ba2+$ ions, compounds containing sulfate ion are soluble.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $NH4+$ ions, compounds containing carbonate, phosphate, chromate and sulfite ions are insoluble in water.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $Ba2+$ ions, compounds containing hydroxide ions are insoluble in water.

(d)

Expert Solution

Answer to Problem 9.24QP

The water solubility of given compounds are,

$Sr(OH)2(s)$ precipitate is formed.

Explanation of Solution

The balanced equation for reaction of $Sr(NO3)2(aq)$ and $Ca(OH)2(aq)$ is,

$Sr(NO3)2(aq)+Ca(OH)2(aq)→Sr(OH)2(s)↓+Ca(NO3)2(aq)$

According to the solubility guideline, $Sr(OH)2(s)$ is contains hydroxide ion so it is insoluble in water so it get precipitated.

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Answer 3

Question

Chapter 9, Problem 9.24QP

(a)

Interpretation Introduction

Interpretation:

The precipitation reaction should be given from given process and formula of the precipitate should be given.

Concept introduction:

Precipitation reaction:

The precipitate is formed, when the two solutions mixed together is called precipitation reaction and precipitate is a insoluble new product of reaction of two solutions.

Solubility guideline:

Compound containing alkali metal cations and ammonium ion are soluble in water.

Compound contains nitrate, acetate and chlorate ions are soluble in water.

Except $Ag+$ , $Hg2+$ and $pb2+$ ions , compounds containing chloride, bromide and iodide ions are soluble in water.

Except $Ag+$ , $Hg2+$ , $pb2+$ , $Ca2+$ , $Sr2+$ and $Ba2+$ ions, compounds containing sulfate ion are soluble.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $NH4+$ ions, compounds containing carbonate, phosphate, chromate and sulfite ions are insoluble in water.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $Ba2+$ ions, compounds containing hydroxide ions are insoluble in water.

(a)

Expert Solution

Answer to Problem 9.24QP

The water solubility of given compounds are,

$Fe(OH)3(s)$ precipitate is formed.

Explanation of Solution

The balanced equation for reaction of $FeCl3(aq)$ and $LiOH(aq)$ is,

$FeCl3(aq)+3LiOH(aq)→Fe(OH)3(s)↓+3LiCl(aq)$

According to the solubility guideline, $Fe(OH)3$ is contains hydroxide ion so it is insoluble in water so it get precipitated.

(b)

Interpretation Introduction

Interpretation:

The precipitation reaction should be given from given process and formula of the precipitate should be given.

Concept introduction:

Precipitation reaction:

The precipitate is formed, when the two solutions mixed together is called precipitation reaction and precipitate is a insoluble new product of reaction of two solutions.

Solubility guideline:

Compound containing alkali metal cations and ammonium ion are soluble in water.

Compound contains nitrate, acetate and chlorate ions are soluble in water.

Except $Ag+$ , $Hg2+$ and $pb2+$ ions , compounds containing chloride, bromide and iodide ions are soluble in water.

Except $Ag+$ , $Hg2+$ , $pb2+$ , $Ca2+$ , $Sr2+$ and $Ba2+$ ions, compounds containing sulfate ion are soluble.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $NH4+$ ions, compounds containing carbonate, phosphate, chromate and sulfite ions are insoluble in water.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $Ba2+$ ions, compounds containing hydroxide ions are insoluble in water.

(b)

Expert Solution

Answer to Problem 9.24QP

The water solubility of given compounds are,

It is not a precipitation reaction

Explanation of Solution

The balanced equation for reaction of $KNO3(aq)$ and $CaCl2(aq)$ is,

$2KNO3(aq)+CaCl2(aq)→Ca(NO3)2(aq)+2KCl(aq)$

According to the solubility guideline, $Ca(NO3)2(aq) and 2KCl(aq)$ soluble in water there is no precipitation take place so not precipitated formed.

(c)

Interpretation Introduction

Interpretation:

The precipitation reaction should be given from given process and formula of the precipitate should be given.

Concept introduction:

Precipitation reaction:

The precipitate is formed, when the two solutions mixed together is called precipitation reaction and precipitate is a insoluble new product of reaction of two solutions.

Solubility guideline:

Compound containing alkali metal cations and ammonium ion are soluble in water.

Compound contains nitrate, acetate and chlorate ions are soluble in water.

Except $Ag+$ , $Hg2+$ and $pb2+$ ions , compounds containing chloride, bromide and iodide ions are soluble in water.

Except $Ag+$ , $Hg2+$ , $pb2+$ , $Ca2+$ , $Sr2+$ and $Ba2+$ ions, compounds containing sulfate ion are soluble.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $NH4+$ ions, compounds containing carbonate, phosphate, chromate and sulfite ions are insoluble in water.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $Ba2+$ ions, compounds containing hydroxide ions are insoluble in water.

(c)

Expert Solution

Answer to Problem 9.24QP

The water solubility of given compounds are,

It is not a precipitation reaction

Explanation of Solution

The balanced equation for reaction of $(NH4)2CO3(aq)$ and $NaCO3(aq)$ is,

$(NH4)2CO3(aq)+Na2CO3(aq)→(NH4)2CO3(aq)+Na2CO3(aq)$

No reaction takes place so no new product formed.

(d)

Interpretation Introduction

Interpretation:

The precipitation reaction should be given from given process and formula of the precipitate should be given.

Concept introduction:

Precipitation reaction:

The precipitate is formed, when the two solutions mixed together is called precipitation reaction and precipitate is a insoluble new product of reaction of two solutions.

Solubility guideline:

Compound containing alkali metal cations and ammonium ion are soluble in water.

Compound contains nitrate, acetate and chlorate ions are soluble in water.

Except $Ag+$ , $Hg2+$ and $pb2+$ ions , compounds containing chloride, bromide and iodide ions are soluble in water.

Except $Ag+$ , $Hg2+$ , $pb2+$ , $Ca2+$ , $Sr2+$ and $Ba2+$ ions, compounds containing sulfate ion are soluble.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $NH4+$ ions, compounds containing carbonate, phosphate, chromate and sulfite ions are insoluble in water.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $Ba2+$ ions, compounds containing hydroxide ions are insoluble in water.

(d)

Expert Solution

Answer to Problem 9.24QP

The water solubility of given compounds are,

$Sr(OH)2(s)$ precipitate is formed.

Explanation of Solution

The balanced equation for reaction of $Sr(NO3)2(aq)$ and $Ca(OH)2(aq)$ is,

$Sr(NO3)2(aq)+Ca(OH)2(aq)→Sr(OH)2(s)↓+Ca(NO3)2(aq)$

According to the solubility guideline, $Sr(OH)2(s)$ is contains hydroxide ion so it is insoluble in water so it get precipitated.

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Answer 4

Question

Chapter 9, Problem 9.24QP

(a)

Interpretation Introduction

Interpretation:

The precipitation reaction should be given from given process and formula of the precipitate should be given.

Concept introduction:

Precipitation reaction:

The precipitate is formed, when the two solutions mixed together is called precipitation reaction and precipitate is a insoluble new product of reaction of two solutions.

Solubility guideline:

Compound containing alkali metal cations and ammonium ion are soluble in water.

Compound contains nitrate, acetate and chlorate ions are soluble in water.

Except $Ag+$ , $Hg2+$ and $pb2+$ ions , compounds containing chloride, bromide and iodide ions are soluble in water.

Except $Ag+$ , $Hg2+$ , $pb2+$ , $Ca2+$ , $Sr2+$ and $Ba2+$ ions, compounds containing sulfate ion are soluble.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $NH4+$ ions, compounds containing carbonate, phosphate, chromate and sulfite ions are insoluble in water.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $Ba2+$ ions, compounds containing hydroxide ions are insoluble in water.

(a)

Expert Solution

Answer to Problem 9.24QP

The water solubility of given compounds are,

$Fe(OH)3(s)$ precipitate is formed.

Explanation of Solution

The balanced equation for reaction of $FeCl3(aq)$ and $LiOH(aq)$ is,

$FeCl3(aq)+3LiOH(aq)→Fe(OH)3(s)↓+3LiCl(aq)$

According to the solubility guideline, $Fe(OH)3$ is contains hydroxide ion so it is insoluble in water so it get precipitated.

(b)

Interpretation Introduction

Interpretation:

The precipitation reaction should be given from given process and formula of the precipitate should be given.

Concept introduction:

Precipitation reaction:

The precipitate is formed, when the two solutions mixed together is called precipitation reaction and precipitate is a insoluble new product of reaction of two solutions.

Solubility guideline:

Compound containing alkali metal cations and ammonium ion are soluble in water.

Compound contains nitrate, acetate and chlorate ions are soluble in water.

Except $Ag+$ , $Hg2+$ and $pb2+$ ions , compounds containing chloride, bromide and iodide ions are soluble in water.

Except $Ag+$ , $Hg2+$ , $pb2+$ , $Ca2+$ , $Sr2+$ and $Ba2+$ ions, compounds containing sulfate ion are soluble.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $NH4+$ ions, compounds containing carbonate, phosphate, chromate and sulfite ions are insoluble in water.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $Ba2+$ ions, compounds containing hydroxide ions are insoluble in water.

(b)

Expert Solution

Answer to Problem 9.24QP

The water solubility of given compounds are,

It is not a precipitation reaction

Explanation of Solution

The balanced equation for reaction of $KNO3(aq)$ and $CaCl2(aq)$ is,

$2KNO3(aq)+CaCl2(aq)→Ca(NO3)2(aq)+2KCl(aq)$

According to the solubility guideline, $Ca(NO3)2(aq) and 2KCl(aq)$ soluble in water there is no precipitation take place so not precipitated formed.

(c)

Interpretation Introduction

Interpretation:

The precipitation reaction should be given from given process and formula of the precipitate should be given.

Concept introduction:

Precipitation reaction:

The precipitate is formed, when the two solutions mixed together is called precipitation reaction and precipitate is a insoluble new product of reaction of two solutions.

Solubility guideline:

Compound containing alkali metal cations and ammonium ion are soluble in water.

Compound contains nitrate, acetate and chlorate ions are soluble in water.

Except $Ag+$ , $Hg2+$ and $pb2+$ ions , compounds containing chloride, bromide and iodide ions are soluble in water.

Except $Ag+$ , $Hg2+$ , $pb2+$ , $Ca2+$ , $Sr2+$ and $Ba2+$ ions, compounds containing sulfate ion are soluble.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $NH4+$ ions, compounds containing carbonate, phosphate, chromate and sulfite ions are insoluble in water.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $Ba2+$ ions, compounds containing hydroxide ions are insoluble in water.

(c)

Expert Solution

Answer to Problem 9.24QP

The water solubility of given compounds are,

It is not a precipitation reaction

Explanation of Solution

The balanced equation for reaction of $(NH4)2CO3(aq)$ and $NaCO3(aq)$ is,

$(NH4)2CO3(aq)+Na2CO3(aq)→(NH4)2CO3(aq)+Na2CO3(aq)$

No reaction takes place so no new product formed.

(d)

Interpretation Introduction

Interpretation:

The precipitation reaction should be given from given process and formula of the precipitate should be given.

Concept introduction:

Precipitation reaction:

The precipitate is formed, when the two solutions mixed together is called precipitation reaction and precipitate is a insoluble new product of reaction of two solutions.

Solubility guideline:

Compound containing alkali metal cations and ammonium ion are soluble in water.

Compound contains nitrate, acetate and chlorate ions are soluble in water.

Except $Ag+$ , $Hg2+$ and $pb2+$ ions , compounds containing chloride, bromide and iodide ions are soluble in water.

Except $Ag+$ , $Hg2+$ , $pb2+$ , $Ca2+$ , $Sr2+$ and $Ba2+$ ions, compounds containing sulfate ion are soluble.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $NH4+$ ions, compounds containing carbonate, phosphate, chromate and sulfite ions are insoluble in water.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $Ba2+$ ions, compounds containing hydroxide ions are insoluble in water.

(d)

Expert Solution

Answer to Problem 9.24QP

The water solubility of given compounds are,

$Sr(OH)2(s)$ precipitate is formed.

Explanation of Solution

The balanced equation for reaction of $Sr(NO3)2(aq)$ and $Ca(OH)2(aq)$ is,

$Sr(NO3)2(aq)+Ca(OH)2(aq)→Sr(OH)2(s)↓+Ca(NO3)2(aq)$

According to the solubility guideline, $Sr(OH)2(s)$ is contains hydroxide ion so it is insoluble in water so it get precipitated.

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Answer 5

Chapter 9, Problem 9.24QP

(a)

Interpretation Introduction

Interpretation:

The precipitation reaction should be given from given process and formula of the precipitate should be given.

Concept introduction:

Precipitation reaction:

The precipitate is formed, when the two solutions mixed together is called precipitation reaction and precipitate is a insoluble new product of reaction of two solutions.

Solubility guideline:

Compound containing alkali metal cations and ammonium ion are soluble in water.

Compound contains nitrate, acetate and chlorate ions are soluble in water.

Except $Ag+$ , $Hg2+$ and $pb2+$ ions , compounds containing chloride, bromide and iodide ions are soluble in water.

Except $Ag+$ , $Hg2+$ , $pb2+$ , $Ca2+$ , $Sr2+$ and $Ba2+$ ions, compounds containing sulfate ion are soluble.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $NH4+$ ions, compounds containing carbonate, phosphate, chromate and sulfite ions are insoluble in water.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $Ba2+$ ions, compounds containing hydroxide ions are insoluble in water.

(a)

Expert Solution

Answer to Problem 9.24QP

The water solubility of given compounds are,

$Fe(OH)3(s)$ precipitate is formed.

Explanation of Solution

The balanced equation for reaction of $FeCl3(aq)$ and $LiOH(aq)$ is,

$FeCl3(aq)+3LiOH(aq)→Fe(OH)3(s)↓+3LiCl(aq)$

According to the solubility guideline, $Fe(OH)3$ is contains hydroxide ion so it is insoluble in water so it get precipitated.

(b)

Interpretation Introduction

Interpretation:

The precipitation reaction should be given from given process and formula of the precipitate should be given.

Concept introduction:

Precipitation reaction:

The precipitate is formed, when the two solutions mixed together is called precipitation reaction and precipitate is a insoluble new product of reaction of two solutions.

Solubility guideline:

Compound containing alkali metal cations and ammonium ion are soluble in water.

Compound contains nitrate, acetate and chlorate ions are soluble in water.

Except $Ag+$ , $Hg2+$ and $pb2+$ ions , compounds containing chloride, bromide and iodide ions are soluble in water.

Except $Ag+$ , $Hg2+$ , $pb2+$ , $Ca2+$ , $Sr2+$ and $Ba2+$ ions, compounds containing sulfate ion are soluble.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $NH4+$ ions, compounds containing carbonate, phosphate, chromate and sulfite ions are insoluble in water.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $Ba2+$ ions, compounds containing hydroxide ions are insoluble in water.

(b)

Expert Solution

Answer to Problem 9.24QP

The water solubility of given compounds are,

It is not a precipitation reaction

Explanation of Solution

The balanced equation for reaction of $KNO3(aq)$ and $CaCl2(aq)$ is,

$2KNO3(aq)+CaCl2(aq)→Ca(NO3)2(aq)+2KCl(aq)$

According to the solubility guideline, $Ca(NO3)2(aq) and 2KCl(aq)$ soluble in water there is no precipitation take place so not precipitated formed.

(c)

Interpretation Introduction

Interpretation:

The precipitation reaction should be given from given process and formula of the precipitate should be given.

Concept introduction:

Precipitation reaction:

The precipitate is formed, when the two solutions mixed together is called precipitation reaction and precipitate is a insoluble new product of reaction of two solutions.

Solubility guideline:

Compound containing alkali metal cations and ammonium ion are soluble in water.

Compound contains nitrate, acetate and chlorate ions are soluble in water.

Except $Ag+$ , $Hg2+$ and $pb2+$ ions , compounds containing chloride, bromide and iodide ions are soluble in water.

Except $Ag+$ , $Hg2+$ , $pb2+$ , $Ca2+$ , $Sr2+$ and $Ba2+$ ions, compounds containing sulfate ion are soluble.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $NH4+$ ions, compounds containing carbonate, phosphate, chromate and sulfite ions are insoluble in water.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $Ba2+$ ions, compounds containing hydroxide ions are insoluble in water.

(c)

Expert Solution

Answer to Problem 9.24QP

The water solubility of given compounds are,

It is not a precipitation reaction

Explanation of Solution

The balanced equation for reaction of $(NH4)2CO3(aq)$ and $NaCO3(aq)$ is,

$(NH4)2CO3(aq)+Na2CO3(aq)→(NH4)2CO3(aq)+Na2CO3(aq)$

No reaction takes place so no new product formed.

(d)

Interpretation Introduction

Interpretation:

The precipitation reaction should be given from given process and formula of the precipitate should be given.

Concept introduction:

Precipitation reaction:

The precipitate is formed, when the two solutions mixed together is called precipitation reaction and precipitate is a insoluble new product of reaction of two solutions.

Solubility guideline:

Compound containing alkali metal cations and ammonium ion are soluble in water.

Compound contains nitrate, acetate and chlorate ions are soluble in water.

Except $Ag+$ , $Hg2+$ and $pb2+$ ions , compounds containing chloride, bromide and iodide ions are soluble in water.

Except $Ag+$ , $Hg2+$ , $pb2+$ , $Ca2+$ , $Sr2+$ and $Ba2+$ ions, compounds containing sulfate ion are soluble.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $NH4+$ ions, compounds containing carbonate, phosphate, chromate and sulfite ions are insoluble in water.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $Ba2+$ ions, compounds containing hydroxide ions are insoluble in water.

(d)

Expert Solution

Answer to Problem 9.24QP

The water solubility of given compounds are,

$Sr(OH)2(s)$ precipitate is formed.

Explanation of Solution

The balanced equation for reaction of $Sr(NO3)2(aq)$ and $Ca(OH)2(aq)$ is,

$Sr(NO3)2(aq)+Ca(OH)2(aq)→Sr(OH)2(s)↓+Ca(NO3)2(aq)$

According to the solubility guideline, $Sr(OH)2(s)$ is contains hydroxide ion so it is insoluble in water so it get precipitated.

Answer 6

Chapter 9, Problem 9.24QP

(a)

Interpretation Introduction

Interpretation:

The precipitation reaction should be given from given process and formula of the precipitate should be given.

Concept introduction:

Precipitation reaction:

The precipitate is formed, when the two solutions mixed together is called precipitation reaction and precipitate is a insoluble new product of reaction of two solutions.

Solubility guideline:

Compound containing alkali metal cations and ammonium ion are soluble in water.

Compound contains nitrate, acetate and chlorate ions are soluble in water.

Except $Ag+$ , $Hg2+$ and $pb2+$ ions , compounds containing chloride, bromide and iodide ions are soluble in water.

Except $Ag+$ , $Hg2+$ , $pb2+$ , $Ca2+$ , $Sr2+$ and $Ba2+$ ions, compounds containing sulfate ion are soluble.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $NH4+$ ions, compounds containing carbonate, phosphate, chromate and sulfite ions are insoluble in water.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $Ba2+$ ions, compounds containing hydroxide ions are insoluble in water.

(a)

Expert Solution

Answer to Problem 9.24QP

The water solubility of given compounds are,

$Fe(OH)3(s)$ precipitate is formed.

Explanation of Solution

The balanced equation for reaction of $FeCl3(aq)$ and $LiOH(aq)$ is,

$FeCl3(aq)+3LiOH(aq)→Fe(OH)3(s)↓+3LiCl(aq)$

According to the solubility guideline, $Fe(OH)3$ is contains hydroxide ion so it is insoluble in water so it get precipitated.

Answer 7

Chapter 9, Problem 9.24QP

(a)

Interpretation Introduction

Interpretation:

The precipitation reaction should be given from given process and formula of the precipitate should be given.

Concept introduction:

Precipitation reaction:

The precipitate is formed, when the two solutions mixed together is called precipitation reaction and precipitate is a insoluble new product of reaction of two solutions.

Solubility guideline:

Compound containing alkali metal cations and ammonium ion are soluble in water.

Compound contains nitrate, acetate and chlorate ions are soluble in water.

Except $Ag+$ , $Hg2+$ and $pb2+$ ions , compounds containing chloride, bromide and iodide ions are soluble in water.

Except $Ag+$ , $Hg2+$ , $pb2+$ , $Ca2+$ , $Sr2+$ and $Ba2+$ ions, compounds containing sulfate ion are soluble.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $NH4+$ ions, compounds containing carbonate, phosphate, chromate and sulfite ions are insoluble in water.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $Ba2+$ ions, compounds containing hydroxide ions are insoluble in water.

Answer 8

(a)

Expert Solution

Answer to Problem 9.24QP

The water solubility of given compounds are,

$Fe(OH)3(s)$ precipitate is formed.

Answer 9

(a)

Expert Solution

Answer 10

(a)

Expert Solution

Answer 11

Expert Solution

Answer 12

Explanation of Solution

The balanced equation for reaction of $FeCl3(aq)$ and $LiOH(aq)$ is,

$FeCl3(aq)+3LiOH(aq)→Fe(OH)3(s)↓+3LiCl(aq)$

According to the solubility guideline, $Fe(OH)3$ is contains hydroxide ion so it is insoluble in water so it get precipitated.

Answer 13

(b)

Interpretation Introduction

Interpretation:

The precipitation reaction should be given from given process and formula of the precipitate should be given.

Concept introduction:

Precipitation reaction:

The precipitate is formed, when the two solutions mixed together is called precipitation reaction and precipitate is a insoluble new product of reaction of two solutions.

Solubility guideline:

Compound containing alkali metal cations and ammonium ion are soluble in water.

Compound contains nitrate, acetate and chlorate ions are soluble in water.

Except $Ag+$ , $Hg2+$ and $pb2+$ ions , compounds containing chloride, bromide and iodide ions are soluble in water.

Except $Ag+$ , $Hg2+$ , $pb2+$ , $Ca2+$ , $Sr2+$ and $Ba2+$ ions, compounds containing sulfate ion are soluble.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $NH4+$ ions, compounds containing carbonate, phosphate, chromate and sulfite ions are insoluble in water.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $Ba2+$ ions, compounds containing hydroxide ions are insoluble in water.

(b)

Expert Solution

Answer to Problem 9.24QP

The water solubility of given compounds are,

It is not a precipitation reaction

Explanation of Solution

The balanced equation for reaction of $KNO3(aq)$ and $CaCl2(aq)$ is,

$2KNO3(aq)+CaCl2(aq)→Ca(NO3)2(aq)+2KCl(aq)$

According to the solubility guideline, $Ca(NO3)2(aq) and 2KCl(aq)$ soluble in water there is no precipitation take place so not precipitated formed.

Answer 14

(b)

Interpretation Introduction

Interpretation:

The precipitation reaction should be given from given process and formula of the precipitate should be given.

Concept introduction:

Precipitation reaction:

The precipitate is formed, when the two solutions mixed together is called precipitation reaction and precipitate is a insoluble new product of reaction of two solutions.

Solubility guideline:

Compound containing alkali metal cations and ammonium ion are soluble in water.

Compound contains nitrate, acetate and chlorate ions are soluble in water.

Except $Ag+$ , $Hg2+$ and $pb2+$ ions , compounds containing chloride, bromide and iodide ions are soluble in water.

Except $Ag+$ , $Hg2+$ , $pb2+$ , $Ca2+$ , $Sr2+$ and $Ba2+$ ions, compounds containing sulfate ion are soluble.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $NH4+$ ions, compounds containing carbonate, phosphate, chromate and sulfite ions are insoluble in water.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $Ba2+$ ions, compounds containing hydroxide ions are insoluble in water.

Answer 15

(b)

Expert Solution

Answer to Problem 9.24QP

The water solubility of given compounds are,

It is not a precipitation reaction

Answer 16

(b)

Expert Solution

Answer 17

(b)

Expert Solution

Answer 18

Expert Solution

Answer 19

Explanation of Solution

The balanced equation for reaction of $KNO3(aq)$ and $CaCl2(aq)$ is,

$2KNO3(aq)+CaCl2(aq)→Ca(NO3)2(aq)+2KCl(aq)$

According to the solubility guideline, $Ca(NO3)2(aq) and 2KCl(aq)$ soluble in water there is no precipitation take place so not precipitated formed.

Answer 20

(c)

Interpretation Introduction

Interpretation:

The precipitation reaction should be given from given process and formula of the precipitate should be given.

Concept introduction:

Precipitation reaction:

The precipitate is formed, when the two solutions mixed together is called precipitation reaction and precipitate is a insoluble new product of reaction of two solutions.

Solubility guideline:

Compound containing alkali metal cations and ammonium ion are soluble in water.

Compound contains nitrate, acetate and chlorate ions are soluble in water.

Except $Ag+$ , $Hg2+$ and $pb2+$ ions , compounds containing chloride, bromide and iodide ions are soluble in water.

Except $Ag+$ , $Hg2+$ , $pb2+$ , $Ca2+$ , $Sr2+$ and $Ba2+$ ions, compounds containing sulfate ion are soluble.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $NH4+$ ions, compounds containing carbonate, phosphate, chromate and sulfite ions are insoluble in water.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $Ba2+$ ions, compounds containing hydroxide ions are insoluble in water.

(c)

Expert Solution

Answer to Problem 9.24QP

The water solubility of given compounds are,

It is not a precipitation reaction

Explanation of Solution

The balanced equation for reaction of $(NH4)2CO3(aq)$ and $NaCO3(aq)$ is,

$(NH4)2CO3(aq)+Na2CO3(aq)→(NH4)2CO3(aq)+Na2CO3(aq)$

No reaction takes place so no new product formed.

Answer 21

(c)

Interpretation Introduction

Interpretation:

The precipitation reaction should be given from given process and formula of the precipitate should be given.

Concept introduction:

Precipitation reaction:

The precipitate is formed, when the two solutions mixed together is called precipitation reaction and precipitate is a insoluble new product of reaction of two solutions.

Solubility guideline:

Compound containing alkali metal cations and ammonium ion are soluble in water.

Compound contains nitrate, acetate and chlorate ions are soluble in water.

Except $Ag+$ , $Hg2+$ and $pb2+$ ions , compounds containing chloride, bromide and iodide ions are soluble in water.

Except $Ag+$ , $Hg2+$ , $pb2+$ , $Ca2+$ , $Sr2+$ and $Ba2+$ ions, compounds containing sulfate ion are soluble.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $NH4+$ ions, compounds containing carbonate, phosphate, chromate and sulfite ions are insoluble in water.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $Ba2+$ ions, compounds containing hydroxide ions are insoluble in water.

Answer 22

(c)

Expert Solution

Answer to Problem 9.24QP

The water solubility of given compounds are,

It is not a precipitation reaction

Answer 23

(c)

Expert Solution

Answer 24

(c)

Expert Solution

Answer 25

Expert Solution

Answer 26

Explanation of Solution

The balanced equation for reaction of $(NH4)2CO3(aq)$ and $NaCO3(aq)$ is,

$(NH4)2CO3(aq)+Na2CO3(aq)→(NH4)2CO3(aq)+Na2CO3(aq)$

No reaction takes place so no new product formed.

Answer 27

(d)

Interpretation Introduction

Interpretation:

The precipitation reaction should be given from given process and formula of the precipitate should be given.

Concept introduction:

Precipitation reaction:

The precipitate is formed, when the two solutions mixed together is called precipitation reaction and precipitate is a insoluble new product of reaction of two solutions.

Solubility guideline:

Compound containing alkali metal cations and ammonium ion are soluble in water.

Compound contains nitrate, acetate and chlorate ions are soluble in water.

Except $Ag+$ , $Hg2+$ and $pb2+$ ions , compounds containing chloride, bromide and iodide ions are soluble in water.

Except $Ag+$ , $Hg2+$ , $pb2+$ , $Ca2+$ , $Sr2+$ and $Ba2+$ ions, compounds containing sulfate ion are soluble.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $NH4+$ ions, compounds containing carbonate, phosphate, chromate and sulfite ions are insoluble in water.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $Ba2+$ ions, compounds containing hydroxide ions are insoluble in water.

(d)

Expert Solution

Answer to Problem 9.24QP

The water solubility of given compounds are,

$Sr(OH)2(s)$ precipitate is formed.

Explanation of Solution

The balanced equation for reaction of $Sr(NO3)2(aq)$ and $Ca(OH)2(aq)$ is,

$Sr(NO3)2(aq)+Ca(OH)2(aq)→Sr(OH)2(s)↓+Ca(NO3)2(aq)$

According to the solubility guideline, $Sr(OH)2(s)$ is contains hydroxide ion so it is insoluble in water so it get precipitated.

Answer 28

(d)

Interpretation Introduction

Interpretation:

The precipitation reaction should be given from given process and formula of the precipitate should be given.

Concept introduction:

Precipitation reaction:

The precipitate is formed, when the two solutions mixed together is called precipitation reaction and precipitate is a insoluble new product of reaction of two solutions.

Solubility guideline:

Compound containing alkali metal cations and ammonium ion are soluble in water.

Compound contains nitrate, acetate and chlorate ions are soluble in water.

Except $Ag+$ , $Hg2+$ and $pb2+$ ions , compounds containing chloride, bromide and iodide ions are soluble in water.

Except $Ag+$ , $Hg2+$ , $pb2+$ , $Ca2+$ , $Sr2+$ and $Ba2+$ ions, compounds containing sulfate ion are soluble.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $NH4+$ ions, compounds containing carbonate, phosphate, chromate and sulfite ions are insoluble in water.

Except $Li+$ , $Na+$ , $K+$ , $Rb+$ , $Cs+$ and $Ba2+$ ions, compounds containing hydroxide ions are insoluble in water.

Answer 29

(d)

Expert Solution

Answer to Problem 9.24QP

The water solubility of given compounds are,

$Sr(OH)2(s)$ precipitate is formed.

Answer 30

(d)

Expert Solution

Answer 31

(d)

Expert Solution

Answer 32

Expert Solution

Answer 33

Explanation of Solution

The balanced equation for reaction of $Sr(NO3)2(aq)$ and $Ca(OH)2(aq)$ is,

$Sr(NO3)2(aq)+Ca(OH)2(aq)→Sr(OH)2(s)↓+Ca(NO3)2(aq)$

According to the solubility guideline, $Sr(OH)2(s)$ is contains hydroxide ion so it is insoluble in water so it get precipitated.

Answer 34

Ch. 9.1 - Sports drinks typically contain sucrose...Ch. 9.1 - Prob. 1PPA Ch. 9.1 - Prob. 1PPB Ch. 9.1 - Prob. 1PPC Ch. 9.1 - Prob. 9.1.1SR Ch. 9.1 - Prob. 9.1.2SR Ch. 9.1 - Prob. 9.1.3SR Ch. 9.2 - Classify each of the following compounds as...Ch. 9.2 - Prob. 2PPA Ch. 9.2 - Prob. 2PPB

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Answer to Problem 9.24QP

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Answer to Problem 9.24QP

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