Glencoe Chemistry: Matter and Change, Student Edition
Glencoe Chemistry: Matter and Change, Student Edition
1st Edition
ISBN: 9780076774609
Author: McGraw-Hill Education
Publisher: MCGRAW-HILL HIGHER EDUCATION
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Chapter 14.2, Problem 31SSC
Interpretation Introduction

Interpretation:

Five quantitative ways to describe the composition of solution have to be compared and contrasted.

Concept introduction:

Solutions are homogeneous mixtures of two or more than two components. By homogenous mixture we mean that its composition and properties are uniform throughout the mixture.

Composition of a solution can be defined by expressing its concentration. Concentration can be expressed either qualitatively or quantitatively. Concentration can be described qualitatively using the words concentrated or dilute. The solution is either dilute or concentrated depends on the amount of solute present in the solution. In concentrated solution more amount of solute is present compare to dilute solution. There are several ways by which we can describe the concentration of the solution quantitatively. Some commonly used quantitative descriptions are percent by mass, percent by volume, molarity, molality and mole fraction.

Expert Solution & Answer
Check Mark

Answer to Problem 31SSC

Quantitatively concentration of the solution can be expressed in five different ways such as percent by mass, percent by volume, molarity, molality and mole fraction. Among them, molarity, molality, and mole fraction are basedon moles of solute per some other quantity;percent by volume and molarity are defined by per volume of solution basis, molality and molefraction are based on per quantity of solvent basis, percent by mass and percent by volume are the only ratios involving percentages.

Quantitatively concentration of the solution can be expressed in five different ways-

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

Mass % of a component=Mass of the component in the solutionTotal mass of the solution×100

Volume/volume percentage (v/V percent): Percent by volume is expressed as the ratio of the volume of the solute to the total volume of the solution multiplied by 100.

In expression,

Volume percentage (v/V) % of a component=Volumeof the soluteTotal volume of the solution×100

Molarity: Molarity is defined as the number of moles of solute present in one litre of the solution and is expressed as:

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

Molality: Molality (m) is defined as the number of moles of the solute per kilogram (kg) of the solvent and is expressed as:

Molality of the solution=Numberofmolesof the soluteMassof the solvent(inkg)

Mole fraction: Mole fraction defined as the number of moles of one component divided by total the number of moles in the mixture. Mole fraction is denoted as ‘ χi ’ where subscript ‘i’ represents the particular component. The sum of the mole fractions of the components in a mixture (or a solution) is unity. The mole fraction for the solvent ( χA )and the mole fraction for the solute ( χB )can be expressed as follows

Mole fraction χA=nA nA+nB and χB=nB nA+nB Where, χA and χB represent the mole fractions of each substance. nA and nBrepresent the number of moles of each substance.

(χA+χB)=1

Molarity, molality, and mole fraction are based on moles of solute per some other quantity, percent by volume and molarity are defined by per volume of solution basis, molality and mole fraction are based on per quantity of solvent basis, percent by mass and percent by volume are the only ratios involving percentages. Mass percent, mole fraction and molality are independent of temperature, whereas volume percent and molarity are function of temperature. This is because volume depends on temperature and the mass does not.

Explanation of Solution

Quantitatively concentration of the solution can be expressed in five different ways-

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

Mass % of a component=Mass of the component in the solutionTotal mass of the solution×100

Volume/volume percentage (v/V percent): Percent by volume is expressed as the ratio of the volume of the solute to the total volume of the solution multiplied by 100.

In expression,

Volume percentage (v/V) % of a component=Volumeof the soluteTotal volume of the solution×100

Molarity: Molarity is defined as the number of moles of solute present in one litre of the solution and is expressed as:

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

Molality: Molality (m) is defined as the number of moles of the solute per kilogram (kg) of the solvent and is expressed as:

Molality of the solution=Numberofmolesof the soluteMassof the solvent(inkg)

Mole fraction: Mole fraction defined as the number of moles of one component divided by total the number of moles in the mixture. Mole fraction is denoted as ‘ χi ’ where subscript ‘i’ represents the particular component. The sum of the mole fractions of the components in a mixture (or a solution) is unity. The mole fraction for the solvent ( χA )and the mole fraction for the solute ( χB )can be expressed as follows

Mole fraction χA=nA nA+nB and χB=nB nA+nB Where, χA and χB represent the mole fractions of each substance. nA and nBrepresent the number of moles of each substance.

(χA+χB)=1

Molarity, molality, and mole fraction are based on moles of solute per some other quantity, percent by volume and molarity are defined by per volume of solution basis, molality and mole fraction are based on per quantity of solvent basis, percent by mass and percent by volume are the only ratios involving percentages. Mass percent, mole fraction and molality are independent of temperature, whereas volume percent and molarity are function of temperature. This is because volume depends on temperature and the mass does not.

Chapter 14 Solutions

Glencoe Chemistry: Matter and Change, Student Edition

Ch. 14.2 - Prob. 11PPCh. 14.2 - Prob. 12PPCh. 14.2 - Prob. 13PPCh. 14.2 - Prob. 14PPCh. 14.2 - Prob. 15PPCh. 14.2 - Prob. 16PPCh. 14.2 - Prob. 17PPCh. 14.2 - Prob. 18PPCh. 14.2 - Prob. 19PPCh. 14.2 - Prob. 20PPCh. 14.2 - Prob. 21PPCh. 14.2 - Prob. 22PPCh. 14.2 - Prob. 23PPCh. 14.2 - Prob. 24PPCh. 14.2 - Prob. 25PPCh. 14.2 - Prob. 26PPCh. 14.2 - Prob. 27PPCh. 14.2 - Prob. 28PPCh. 14.2 - Prob. 29PPCh. 14.2 - Prob. 30PPCh. 14.2 - Prob. 31SSCCh. 14.2 - Prob. 32SSCCh. 14.2 - Prob. 33SSCCh. 14.2 - Prob. 34SSCCh. 14.2 - Prob. 35SSCCh. 14.3 - Prob. 36PPCh. 14.3 - Prob. 37PPCh. 14.3 - Prob. 38PPCh. 14.3 - Prob. 39SSCCh. 14.3 - Prob. 40SSCCh. 14.3 - Prob. 41SSCCh. 14.3 - Prob. 42SSCCh. 14.3 - Prob. 43SSCCh. 14.3 - Prob. 44SSCCh. 14.4 - Prob. 45PPCh. 14.4 - Prob. 46PPCh. 14.4 - Prob. 47PPCh. 14.4 - Prob. 48SSCCh. 14.4 - Prob. 49SSCCh. 14.4 - Prob. 50SSCCh. 14.4 - Prob. 51SSCCh. 14.4 - Prob. 52SSCCh. 14.4 - Prob. 53SSCCh. 14 - Prob. 54ACh. 14 - What is the difference between a solute and a...Ch. 14 - Prob. 56ACh. 14 - Prob. 57ACh. 14 - Prob. 58ACh. 14 - Prob. 59ACh. 14 - Prob. 60ACh. 14 - Prob. 61ACh. 14 - Prob. 62ACh. 14 - Prob. 63ACh. 14 - Prob. 64ACh. 14 - How do 0.5M and 2.0M aqueous solutions of NaCl...Ch. 14 - Prob. 66ACh. 14 - Prob. 67ACh. 14 - Prob. 68ACh. 14 - Prob. 69ACh. 14 - Prob. 70ACh. 14 - Prob. 71ACh. 14 - Prob. 72ACh. 14 - Prob. 73ACh. 14 - How much CaCl2 , in grams, is needed to make 2.0 L...Ch. 14 - Stock solutions of HCl with various molarities are...Ch. 14 - Prob. 76ACh. 14 - Prob. 77ACh. 14 - Prob. 78ACh. 14 - If you dilute 20.0 mL of a 3.5M solution to...Ch. 14 - Prob. 80ACh. 14 - Prob. 81ACh. 14 - Prob. 82ACh. 14 - Prob. 83ACh. 14 - What is the mole fraction of H 2 S O 4 in a...Ch. 14 - Prob. 85ACh. 14 - Prob. 86ACh. 14 - Prob. 87ACh. 14 - Prob. 88ACh. 14 - Prob. 89ACh. 14 - Prob. 90ACh. 14 - Prob. 91ACh. 14 - Prob. 92ACh. 14 - Prob. 93ACh. 14 - Prob. 94ACh. 14 - Prob. 95ACh. 14 - Prob. 96ACh. 14 - Prob. 97ACh. 14 - Prob. 98ACh. 14 - Prob. 99ACh. 14 - In the lab, you dissolve 179 g of MgCl2 into1.00 L...Ch. 14 - Cooking A cook prepares a solution for boiling by...Ch. 14 - Prob. 102ACh. 14 - Ice Cream A rock salt (NaCl), ice, and water...Ch. 14 - Apply your knowledge of polarity and solubility...Ch. 14 - Prob. 105ACh. 14 - Which solute has the greatest effect on the...Ch. 14 - Study Table 14.4. Analyze solubility and...Ch. 14 - Prob. 108ACh. 14 - If you prepared a saturated aqueous solution of...Ch. 14 - How many grams of calcium nitrate (Ca(NO3)2)...Ch. 14 - Prob. 111ACh. 14 - Prob. 112ACh. 14 - Prob. 113ACh. 14 - Prob. 114ACh. 14 - Infer Dehydration occurs when more fluid is lost...Ch. 14 - Graph Table 14.10 shows solubility data that was...Ch. 14 - Design an Experiment You are given a sample of a...Ch. 14 - Compare Which of the following solutions has...Ch. 14 - Prob. 119ACh. 14 - Prob. 120ACh. 14 - Prob. 121ACh. 14 - Prob. 122ACh. 14 - Prob. 123ACh. 14 - Prob. 124ACh. 14 - Prob. 125ACh. 14 - Prob. 126ACh. 14 - Prob. 127ACh. 14 - Prob. 128ACh. 14 - Prob. 129ACh. 14 - Prob. 1STPCh. 14 - Prob. 2STPCh. 14 - Prob. 3STPCh. 14 - Prob. 4STPCh. 14 - Prob. 5STPCh. 14 - Prob. 6STPCh. 14 - Prob. 7STPCh. 14 - Prob. 8STPCh. 14 - Prob. 9STPCh. 14 - Prob. 10STPCh. 14 - Prob. 11STPCh. 14 - Prob. 12STPCh. 14 - Prob. 13STPCh. 14 - Prob. 14STPCh. 14 - Prob. 15STPCh. 14 - Prob. 16STPCh. 14 - Prob. 17STPCh. 14 - Prob. 18STPCh. 14 - Prob. 19STP
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