World of Chemistry
World of Chemistry
7th Edition
ISBN: 9780618562763
Author: Steven S. Zumdahl
Publisher: Houghton Mifflin College Div
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Chapter 15, Problem 27A

(a)

Interpretation Introduction

Interpretation:

The number of moles and the number of grams of the given solute in a given solutionhave to be calculated.

Concept Introduction:

The 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 methodsare usedto 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.

Molarity: Molarity is defined as the number of moles of solute present in one liter of the solution.

In expression, Molarityofthesolution=Numberofmolesof the solute Volume of the solution(inlitre)

Again Numberofmolesofsolute=MassofthesoluteMolecularweightofthesolute

(a)

Expert Solution
Check Mark

Answer to Problem 27A

    Number of molesNumber of grams
    127 mL of 0.105 M HNO30.0133 mol0.84 gm

Explanation of Solution

Molarityofthesolution=Numberofmolesof the solute Volume of the solution(inlitre)

Data given: Molarity of HNO3 solution= 0.105 M

      Volume of HNO3 solution = 127 mL = 0.127 L

MolarityofHNO3solution=NumberofmolesofHNO3 Volume of HNO3solution(inlitre)

  NumberofmolesofHNO3=MolarityofHNO3solution×Volume of HNO3solution(inlitre)

  =0.105M×0.127L=0.0133mol

NumberofmolesofHNO3=MassofHNO3MolecularweightofHNO3

      MassofHNO3=NumberofmolesofHNO3×MolecularweightofHNO3

      =0.0133mol×63.01gm/mol=0.84gm

(b)

Interpretation Introduction

Interpretation:

The number of moles and the number of grams of the given solute in a given solutionhave to be calculated.

Concept Introduction:

The 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.

Molarity: Molarity is defined as the number of moles of solute present in one liter of the solution.

In expression, Molarityofthesolution=Numberofmolesof the solute Volume of the solution(inlitre)

Again Numberofmolesofsolute=MassofthesoluteMolecularweightofthesolute

(b)

Expert Solution
Check Mark

Answer to Problem 27A

    Number of molesNumber of grams
    155 mL of 15.1 M NH32.34 mol39.79 gm

Explanation of Solution

Molarityofthesolution=Numberofmolesof the solute Volume of the solution(inlitre)

Data given: Molarity of NH3 solution= 15.1 M

      Volume of NH3 solution = 155 mL = 0.155 L

  MolarityofNH3solution=NumberofmolesofNH3 Volume of NH3solution(inlitre)

  NumberofmolesofNH3=MolarityofNH3solution×Volume of NH3solution(inlitre)

  =15.1M×0.155L=2.34mol

NumberofmolesofNH3=MassofNH3MolecularweightofNH3

    MassofNH3=NumberofmolesofNH3×MolecularweightofNH3

    =2.34mol×17gm/mol=39.79gm

(c)

Interpretation Introduction

Interpretation:

The number of moles and the number of grams of the given solute in a given solutionhave to be calculated.

Concept Introduction:

The 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.

Molarity: Molarity is defined as the number of moles of solute present in one liter of the solution.

In expression, Molarityofthesolution=Numberofmolesof the solute Volume of the solution(inlitre)

Again Numberofmolesofsolute=MassofthesoluteMolecularweightofthesolute

(c)

Expert Solution
Check Mark

Answer to Problem 27A

    Number of molesNumber of grams
    2.51 L of 2.01 × 10-3 M KSCN0.005 mol0.49 gm

Explanation of Solution

  Molarityofthesolution=Numberofmolesof the solute Volume of the solution(inlitre)

Data given: Molarity of KSCN solution= 2.01 × 10-3M

      The volume of KSCN solution = 2.51 L

MolarityofKSCNsolution=NumberofmolesofKSCN Volume of KSCNsolution(inlitre)

NumberofmolesofKSCN=MolarityofKSCNsolution×Volume of KSCNsolution(inlitre)

  =2.01×10-3M×2.51L =0.005mol

NumberofmolesofKSCN=MassofKSCNMolecularweightofKSCN

      MassofKSCN=NumberofmolesofKSCN×MolecularweightofKSCN

      =0.005mol×97.18gm/mol =0.49gm

(d)

Interpretation Introduction

Interpretation:

The number of moles and the number of grams of the given solute in a given solutionhave to be calculated.

Concept Introduction:

The 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.

Molarity: Molarity is defined as the number of moles of solute present in one liter of the solution.

In expression, Molarityofthesolution=Numberofmolesof the solute Volume of the solution(inlitre)

Again Numberofmolesofsolute=MassofthesoluteMolecularweightofthesolute

(d)

Expert Solution
Check Mark

Answer to Problem 27A

    Number of molesNumber of grams
    12.2 mL of 2.45 M HCl0.03 mol1.1 gm

Explanation of Solution

  Molarityofthesolution=Numberofmolesof the solute Volume of the solution(inlitre)

Data given: Molarity of HCl solution= 2.45 M

      Volume of HCl solution= 12.2 mL = 0.0122 L

  MolarityofHClsolution=NumberofmolesofHCl Volume of HClsolution(inlitre)

  NumberofmolesofHCl=MolarityofHClsolution×Volume of HClsolution(inlitre)

  =2.45M×0.0122L=0.03mol

  NumberofmolesofHCl=MassofHClMolecularweightofHCl

      MassofHCl=NumberofmolesofHCl×MolecularweightofHCl

      =0.03mol×36.5gm/mol=1.1gm

Chapter 15 Solutions

World of Chemistry

Ch. 15.2 - Prob. 5RQCh. 15.2 - Prob. 6RQCh. 15.2 - Prob. 7RQCh. 15.3 - Prob. 1RQCh. 15.3 - Prob. 2RQCh. 15.3 - Prob. 3RQCh. 15.3 - Prob. 4RQCh. 15.3 - Prob. 5RQCh. 15.3 - Prob. 6RQCh. 15.3 - Prob. 7RQCh. 15.3 - Prob. 8RQCh. 15 - Prob. 1ACh. 15 - Prob. 2ACh. 15 - Prob. 3ACh. 15 - Prob. 4ACh. 15 - Prob. 5ACh. 15 - Prob. 6ACh. 15 - Prob. 7ACh. 15 - Prob. 8ACh. 15 - Prob. 9ACh. 15 - Prob. 10ACh. 15 - Prob. 11ACh. 15 - Prob. 12ACh. 15 - Prob. 13ACh. 15 - Prob. 14ACh. 15 - Prob. 15ACh. 15 - Prob. 16ACh. 15 - Prob. 17ACh. 15 - Prob. 18ACh. 15 - Prob. 19ACh. 15 - Prob. 20ACh. 15 - Prob. 21ACh. 15 - Prob. 22ACh. 15 - Prob. 23ACh. 15 - Prob. 24ACh. 15 - Prob. 25ACh. 15 - Prob. 26ACh. 15 - Prob. 27ACh. 15 - Prob. 28ACh. 15 - Prob. 29ACh. 15 - Prob. 30ACh. 15 - Prob. 31ACh. 15 - Prob. 32ACh. 15 - Prob. 33ACh. 15 - Prob. 34ACh. 15 - Prob. 35ACh. 15 - Prob. 36ACh. 15 - Prob. 37ACh. 15 - Prob. 38ACh. 15 - Prob. 39ACh. 15 - Prob. 40ACh. 15 - Prob. 41ACh. 15 - Prob. 42ACh. 15 - Prob. 43ACh. 15 - Prob. 44ACh. 15 - Prob. 45ACh. 15 - Prob. 46ACh. 15 - Prob. 47ACh. 15 - Prob. 48ACh. 15 - Prob. 49ACh. 15 - Prob. 50ACh. 15 - Prob. 51ACh. 15 - Prob. 52ACh. 15 - Prob. 53ACh. 15 - Prob. 54ACh. 15 - Prob. 55ACh. 15 - Prob. 56ACh. 15 - Prob. 57ACh. 15 - Prob. 58ACh. 15 - Prob. 59ACh. 15 - Prob. 60ACh. 15 - Prob. 61ACh. 15 - Prob. 62ACh. 15 - Prob. 63ACh. 15 - Prob. 1STPCh. 15 - Prob. 2STPCh. 15 - Prob. 3STPCh. 15 - Prob. 4STPCh. 15 - Prob. 5STPCh. 15 - Prob. 6STPCh. 15 - Prob. 7STPCh. 15 - Prob. 8STPCh. 15 - Prob. 9STPCh. 15 - Prob. 10STPCh. 15 - Prob. 11STP
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Solutions: Crash Course Chemistry #27; Author: Crash Course;https://www.youtube.com/watch?v=9h2f1Bjr0p4;License: Standard YouTube License, CC-BY