Chapter 15, Problem 13A

(a)

Interpretation Introduction

Interpretation:

Amount of ammonium chloride present in 375 gm of 1.51% of ammonium chloride solution has to be calculated.

Concept Introduction:

Composition of a solution can be defined by expressing its concentration. The concentrations of solutions can be expressed in different ways, which are involved in the quantity of solute and the quantity of solution or solvent. Various methods are used to describe the concentration of the solution quantitatively. Some commonly used quantitative concentration terms are percent by mass, percent by volume, molarity, molality and mole fraction.

Mass percentage or percent by mass (w/W %): The mass percentage of a component of a solution is defined as:

  $\mathrm{Mass}\%ofacomponent=\frac{Mass of the component in the solution}{Total mass of the solution}\times 100$

Answer to Problem 13A

5.66 gm of ammonium chloride present in 375 gm of 1.51% of ammonium chloride solution.

  $\mathrm{Mass}\%ofacomponent=\frac{Mass of the component in the solution}{Total mass of the solution}\times 100$

Data given: Total mass of the solution = 375 gm

Percent by mass = 1.51%

  $\begin{array}{l}Masspercentage=\frac{Massof ammoniumchloride}{Total mass of the ammoniumchloridesolution}\times 100\\ Massof ammoniumchloride=\frac{Masspercentage\times Total mass of the ammoniumchloridesolution}{100}\\ Massof ammoniumchloride=\frac{1.51\times 375gm}{100}=5.66gm\end{array}$

(b)

Interpretation:

Amount of sodium chloride present in 125 gm of 2.91% of sodium chloride solution has to be calculated.

Concept Introduction:

Composition of a solution can be defined by expressing its concentration. The concentrations of solutions can be expressed in different ways, which are involved in the quantity of solute and the quantity of solution or solvent. Various methods are used to describe the concentration of the solution quantitatively. Some commonly used quantitative concentration terms are percent by mass, percent by volume, molarity, molality and mole fraction.

Mass percentage or percent by mass (w/W %): The mass percentage of a component of a solution is defined as:

  $\mathrm{Mass}\%ofacomponent=\frac{Mass of the component in the solution}{Total mass of the solution}\times 100$

3.64 gm of sodium chloride present in 125 gm of 2.91% of sodium chloride solution.

  $\mathrm{Mass}\%ofacomponent=\frac{Mass of the component in the solution}{Total mass of the solution}\times 100$

Data given: Total mass of the solution = 125 gm

Percent by mass = 2.91%

  $\begin{array}{l}Masspercentage=\frac{Massof sodiumchloride}{Total mass of the sodiumchloridesolution}\times 100\\ Massof sodiumchloride=\frac{Masspercentage\times Total mass of the sodiumchloridesolution}{100}\\ Massof sodiumchloride=\frac{2.91\times 125gm}{100}=3.64gm\end{array}$

(c)

Interpretation:

Amount of potassium nitrate present in 1.31 kg of 4.92% of potassium nitrate solution has to be calculated.

Concept Introduction:

Composition of a solution can be defined by expressing its concentration. The concentrations of solutions can be expressed in different ways, which are involved in the quantity of solute and the quantity of solution or solvent. Various methods are used to describe the concentration of the solution quantitatively. Some commonly used quantitative concentration terms are percent by mass, percent by volume, molarity, molality and mole fraction.

Mass percentage or percent by mass (w/W %): The mass percentage of a component of a solution is defined as:

  $\mathrm{Mass}\%ofacomponent=\frac{Mass of the component in the solution}{Total mass of the solution}\times 100$

64.5 gm of potassium nitrate present in 1.31 kg of 4.92% of potassium nitrate solution.

  $\mathrm{Mass}\%ofacomponent=\frac{Mass of the component in the solution}{Total mass of the solution}\times 100$

Data given: Total mass of the solution = 1.31 kg

Percent by mass = 4.92%

  $\begin{array}{l}Masspercentage=\frac{Massof potassiumnitrate}{Total mass of the potassiumnitratesolution}\times 100\\ Massof potassiumnitrate=\frac{Masspercentage\times Total mass of the potassiumnitratesolution}{100}\\ Massof potassiumnitrate=\frac{4.92\times 1.31kg}{100}=0.0645kg=64.5gm\end{array}$

(d)

Interpretation:

Amount of ammonium nitrate present in 478 mg of 12.5% of ammonium nitrate solution has to be calculated.

Concept Introduction:

Composition of a solution can be defined by expressing its concentration. The concentrations of solutions can be expressed in different ways, which are involved in the quantity of solute and the quantity of solution or solvent. Various methods are used to describe the concentration of the solution quantitatively. Some commonly used quantitative concentration terms are percent by mass, percent by volume, molarity, molality and mole fraction.

Mass percentage or percent by mass (w/W %): The mass percentage of a component of a solution is defined as:

  $\mathrm{Mass}\%ofacomponent=\frac{Mass of the component in the solution}{Total mass of the solution}\times 100$

0.059 gm of ammonium nitrate present in 478 mg of 12.5% of ammonium nitrate solution.

  $\mathrm{Mass}\%ofacomponent=\frac{Mass of the component in the solution}{Total mass of the solution}\times 100$

Data given: Total mass of the solution = 478 mg

Percent by mass = 12.5%

  $\begin{array}{l}Masspercentage=\frac{Massof ammoniumnitrate}{Total mass of the ammoniumnitratesolution}\times 100\\ Massof ammoniumnitrate=\frac{Masspercentage\times Total mass of the ammoniumnitratesolution}{100}\\ Massof ammoniumnitrate=\frac{12.5\times 478mg}{100}=59.75mg=0.059gm\end{array}$

Explanation of Solution

  $\mathrm{Mass}\%ofacomponent=\frac{Mass of the component in the solution}{Total mass of the solution}\times 100$

Data given: Total mass of the solution = 375 gm

Percent by mass = 1.51%

  $\begin{array}{l}Masspercentage=\frac{Massof ammoniumchloride}{Total mass of the ammoniumchloridesolution}\times 100\\ Massof ammoniumchloride=\frac{Masspercentage\times Total mass of the ammoniumchloridesolution}{100}\\ Massof ammoniumchloride=\frac{1.51\times 375gm}{100}=5.66gm\end{array}$

(b)

Interpretation Introduction

Interpretation:

Amount of sodium chloride present in 125 gm of 2.91% of sodium chloride solution has to be calculated.

Concept Introduction:

Composition of a solution can be defined by expressing its concentration. The concentrations of solutions can be expressed in different ways, which are involved in the quantity of solute and the quantity of solution or solvent. Various methods are used to describe the concentration of the solution quantitatively. Some commonly used quantitative concentration terms are percent by mass, percent by volume, molarity, molality and mole fraction.

Mass percentage or percent by mass (w/W %): The mass percentage of a component of a solution is defined as:

  $\mathrm{Mass}\%ofacomponent=\frac{Mass of the component in the solution}{Total mass of the solution}\times 100$

Answer to Problem 13A

3.64 gm of sodium chloride present in 125 gm of 2.91% of sodium chloride solution.

  $\mathrm{Mass}\%ofacomponent=\frac{Mass of the component in the solution}{Total mass of the solution}\times 100$

Data given: Total mass of the solution = 125 gm

Percent by mass = 2.91%

  $\begin{array}{l}Masspercentage=\frac{Massof sodiumchloride}{Total mass of the sodiumchloridesolution}\times 100\\ Massof sodiumchloride=\frac{Masspercentage\times Total mass of the sodiumchloridesolution}{100}\\ Massof sodiumchloride=\frac{2.91\times 125gm}{100}=3.64gm\end{array}$

(c)

Interpretation:

Amount of potassium nitrate present in 1.31 kg of 4.92% of potassium nitrate solution has to be calculated.

Concept Introduction:

Composition of a solution can be defined by expressing its concentration. The concentrations of solutions can be expressed in different ways, which are involved in the quantity of solute and the quantity of solution or solvent. Various methods are used to describe the concentration of the solution quantitatively. Some commonly used quantitative concentration terms are percent by mass, percent by volume, molarity, molality and mole fraction.

Mass percentage or percent by mass (w/W %): The mass percentage of a component of a solution is defined as:

  $\mathrm{Mass}\%ofacomponent=\frac{Mass of the component in the solution}{Total mass of the solution}\times 100$

64.5 gm of potassium nitrate present in 1.31 kg of 4.92% of potassium nitrate solution.

  $\mathrm{Mass}\%ofacomponent=\frac{Mass of the component in the solution}{Total mass of the solution}\times 100$

Data given: Total mass of the solution = 1.31 kg

Percent by mass = 4.92%

  $\begin{array}{l}Masspercentage=\frac{Massof potassiumnitrate}{Total mass of the potassiumnitratesolution}\times 100\\ Massof potassiumnitrate=\frac{Masspercentage\times Total mass of the potassiumnitratesolution}{100}\\ Massof potassiumnitrate=\frac{4.92\times 1.31kg}{100}=0.0645kg=64.5gm\end{array}$

(d)

Interpretation:

Amount of ammonium nitrate present in 478 mg of 12.5% of ammonium nitrate solution has to be calculated.

Concept Introduction:

Composition of a solution can be defined by expressing its concentration. The concentrations of solutions can be expressed in different ways, which are involved in the quantity of solute and the quantity of solution or solvent. Various methods are used to describe the concentration of the solution quantitatively. Some commonly used quantitative concentration terms are percent by mass, percent by volume, molarity, molality and mole fraction.

Mass percentage or percent by mass (w/W %): The mass percentage of a component of a solution is defined as:

  $\mathrm{Mass}\%ofacomponent=\frac{Mass of the component in the solution}{Total mass of the solution}\times 100$

0.059 gm of ammonium nitrate present in 478 mg of 12.5% of ammonium nitrate solution.

  $\mathrm{Mass}\%ofacomponent=\frac{Mass of the component in the solution}{Total mass of the solution}\times 100$

Data given: Total mass of the solution = 478 mg

Percent by mass = 12.5%

  $\begin{array}{l}Masspercentage=\frac{Massof ammoniumnitrate}{Total mass of the ammoniumnitratesolution}\times 100\\ Massof ammoniumnitrate=\frac{Masspercentage\times Total mass of the ammoniumnitratesolution}{100}\\ Massof ammoniumnitrate=\frac{12.5\times 478mg}{100}=59.75mg=0.059gm\end{array}$

Explanation of Solution

  $\mathrm{Mass}\%ofacomponent=\frac{Mass of the component in the solution}{Total mass of the solution}\times 100$

Data given: Total mass of the solution = 125 gm

Percent by mass = 2.91%

  $\begin{array}{l}Masspercentage=\frac{Massof sodiumchloride}{Total mass of the sodiumchloridesolution}\times 100\\ Massof sodiumchloride=\frac{Masspercentage\times Total mass of the sodiumchloridesolution}{100}\\ Massof sodiumchloride=\frac{2.91\times 125gm}{100}=3.64gm\end{array}$

(c)

Interpretation Introduction

Interpretation:

Amount of potassium nitrate present in 1.31 kg of 4.92% of potassium nitrate solution has to be calculated.

Concept Introduction:

Composition of a solution can be defined by expressing its concentration. The concentrations of solutions can be expressed in different ways, which are involved in the quantity of solute and the quantity of solution or solvent. Various methods are used to describe the concentration of the solution quantitatively. Some commonly used quantitative concentration terms are percent by mass, percent by volume, molarity, molality and mole fraction.

Mass percentage or percent by mass (w/W %): The mass percentage of a component of a solution is defined as:

  $\mathrm{Mass}\%ofacomponent=\frac{Mass of the component in the solution}{Total mass of the solution}\times 100$

Answer to Problem 13A

64.5 gm of potassium nitrate present in 1.31 kg of 4.92% of potassium nitrate solution.

  $\mathrm{Mass}\%ofacomponent=\frac{Mass of the component in the solution}{Total mass of the solution}\times 100$

Data given: Total mass of the solution = 1.31 kg

Percent by mass = 4.92%

  $\begin{array}{l}Masspercentage=\frac{Massof potassiumnitrate}{Total mass of the potassiumnitratesolution}\times 100\\ Massof potassiumnitrate=\frac{Masspercentage\times Total mass of the potassiumnitratesolution}{100}\\ Massof potassiumnitrate=\frac{4.92\times 1.31kg}{100}=0.0645kg=64.5gm\end{array}$

(d)

Interpretation:

Amount of ammonium nitrate present in 478 mg of 12.5% of ammonium nitrate solution has to be calculated.

Concept Introduction:

Composition of a solution can be defined by expressing its concentration. The concentrations of solutions can be expressed in different ways, which are involved in the quantity of solute and the quantity of solution or solvent. Various methods are used to describe the concentration of the solution quantitatively. Some commonly used quantitative concentration terms are percent by mass, percent by volume, molarity, molality and mole fraction.

Mass percentage or percent by mass (w/W %): The mass percentage of a component of a solution is defined as:

  $\mathrm{Mass}\%ofacomponent=\frac{Mass of the component in the solution}{Total mass of the solution}\times 100$

0.059 gm of ammonium nitrate present in 478 mg of 12.5% of ammonium nitrate solution.

  $\mathrm{Mass}\%ofacomponent=\frac{Mass of the component in the solution}{Total mass of the solution}\times 100$

Data given: Total mass of the solution = 478 mg

Percent by mass = 12.5%

  $\begin{array}{l}Masspercentage=\frac{Massof ammoniumnitrate}{Total mass of the ammoniumnitratesolution}\times 100\\ Massof ammoniumnitrate=\frac{Masspercentage\times Total mass of the ammoniumnitratesolution}{100}\\ Massof ammoniumnitrate=\frac{12.5\times 478mg}{100}=59.75mg=0.059gm\end{array}$

Explanation of Solution

  $\mathrm{Mass}\%ofacomponent=\frac{Mass of the component in the solution}{Total mass of the solution}\times 100$

Data given: Total mass of the solution = 1.31 kg

Percent by mass = 4.92%

  $\begin{array}{l}Masspercentage=\frac{Massof potassiumnitrate}{Total mass of the potassiumnitratesolution}\times 100\\ Massof potassiumnitrate=\frac{Masspercentage\times Total mass of the potassiumnitratesolution}{100}\\ Massof potassiumnitrate=\frac{4.92\times 1.31kg}{100}=0.0645kg=64.5gm\end{array}$

(d)

Interpretation Introduction

Interpretation:

Amount of ammonium nitrate present in 478 mg of 12.5% of ammonium nitrate solution has to be calculated.

Concept Introduction:

Composition of a solution can be defined by expressing its concentration. The concentrations of solutions can be expressed in different ways, which are involved in the quantity of solute and the quantity of solution or solvent. Various methods are used to describe the concentration of the solution quantitatively. Some commonly used quantitative concentration terms are percent by mass, percent by volume, molarity, molality and mole fraction.

Mass percentage or percent by mass (w/W %): The mass percentage of a component of a solution is defined as:

  $\mathrm{Mass}\%ofacomponent=\frac{Mass of the component in the solution}{Total mass of the solution}\times 100$

Answer to Problem 13A

0.059 gm of ammonium nitrate present in 478 mg of 12.5% of ammonium nitrate solution.

  $\mathrm{Mass}\%ofacomponent=\frac{Mass of the component in the solution}{Total mass of the solution}\times 100$

Data given: Total mass of the solution = 478 mg

Percent by mass = 12.5%

  $\begin{array}{l}Masspercentage=\frac{Massof ammoniumnitrate}{Total mass of the ammoniumnitratesolution}\times 100\\ Massof ammoniumnitrate=\frac{Masspercentage\times Total mass of the ammoniumnitratesolution}{100}\\ Massof ammoniumnitrate=\frac{12.5\times 478mg}{100}=59.75mg=0.059gm\end{array}$

Explanation of Solution

  $\mathrm{Mass}\%ofacomponent=\frac{Mass of the component in the solution}{Total mass of the solution}\times 100$

Data given: Total mass of the solution = 478 mg

Percent by mass = 12.5%

  $\begin{array}{l}Masspercentage=\frac{Massof ammoniumnitrate}{Total mass of the ammoniumnitratesolution}\times 100\\ Massof ammoniumnitrate=\frac{Masspercentage\times Total mass of the ammoniumnitratesolution}{100}\\ Massof ammoniumnitrate=\frac{12.5\times 478mg}{100}=59.75mg=0.059gm\end{array}$