   # Hydrochloric acid is sold as a concentrated aqueous solution. If the concentration of commercial HCl is 12.0 M and its density is 1.18 g/cm 3 , calculate the following: (a) the molality of the solution (b) the weight percent of HCl in the solution ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

#### Solutions

Chapter
Section ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 13, Problem 9PS
Textbook Problem
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## Hydrochloric acid is sold as a concentrated aqueous solution. If the concentration of commercial HCl is 12.0 M and its density is 1.18 g/cm3, calculate the following: (a) the molality of the solution (b) the weight percent of HCl in the solution

(a)

Interpretation Introduction

Interpretation: The molality of HCl solution has to be identified.

Concept introduction:

Molality: The amount of solute (mol) per kilogram of solvent.

Concentration (C, mol/kg) =  molality of solute = Amount of solute (mol)Mass of solvent (Kg)

### Explanation of Solution

The molality:

Given data:

ConcentrationofHCl= 12.0Mdensity=1.18g/cm3

12.0Mmeans12.0molesin1Lofsolution

No.ofmoles=massmolarmass

MassHCl=12.0 mol×36.46g/mol=437.5g

Massof1Lofsolution=1

(b)

Interpretation Introduction

Interpretation: The weight percent of HCl solution has to be identified.

Concept introduction:

Weight percent: The mass of one component divided by the total mass of the mixture, multiplied by 100%

weight % A = Mass of A Mass of A + Mass of B + Mass of C + ...×100%

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