   # Concentrated sulfuric acid has a density of 1.84 g/cm 3 and is 95.0% by weight H 2 SO 4 . What is the molality of this acid? What is its molarity? ### 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 10PS
Textbook Problem
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## Concentrated sulfuric acid has a density of 1.84 g/cm3 and is 95.0% by weight H2SO4. What is the molality of this acid? What is its molarity?

Interpretation Introduction

Interpretation:

The molarity and molality of H2SO4 has to be calculated.

Concept Introduction:

Molarity: It is defined as the number of moles per liter of the solution.

Molarity=nV

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

Molarity:

weight % of H2SO4= 95%density=1.84g/cm3=1.84g/ml3=1840 g/L

Thus weight of H2SO4 is 1840gin1L of solution.

Given that H2SO4 is present 95% by weight in the solution.

0.95×1840=1748g

Molarity is defined as the number of moles per liter of the solution.

Molarity=nV

No.ofmoles=massmolarmass

Molarity=(1748 g/ 98g.mol-1)1L=17.837mol/L=17

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