   Chapter 12, Problem 12.103QP General Chemistry - Standalone boo...

11th Edition
Steven D. Gammon + 7 others
ISBN: 9781305580343

Solutions

Chapter
Section General Chemistry - Standalone boo...

11th Edition
Steven D. Gammon + 7 others
ISBN: 9781305580343
Textbook Problem

Commercially, sulfuric acid is usually obtained as an 98% solution. If this solution is 18 M, what is its density? What is its molality?

Interpretation Introduction

Interpretation:

Molality and density of 18 M sulfuric acid which has 98% of its mass in solution have to be calculated.

Concept Introduction:

Mass percent is one of the parameters that is used to express concentration of a solution.  It is expressed as,

Mass percent of a solute = mass of solutemass of solution × 100%

Molarity is a term used to express concentration of a solution.  It is expressed as,

Molarity = number of moles of solutevolume of solution in L

The term Molality is used to express concentration of a solution.  It is expressed as,

Molality = number of moles of solutemass of solvent in kg

Explanation

Assume that volume of solution is 1.000 L , then number of moles of sulfuric acid in 18 M solution is,

Molarity number of moles of H2SO4volume of solution in Lno.of moles = Volume of solution × molarity = 1.000 L × 18 M = 18 mol

In 18M solution of sulphuric acid,

no.of moles of H2SO4 mass of H2SO4molar mass of H2SO4Mass of H2SO4 = molar mass × no.of moles = 98.09 g/mol × 18 mol = 1765.62 g

As we know,

Mass percent of a H2SO4 mass of H2SO4mass of solution × 100%Mass of solution mass of H2SO4Mass percent = 1765

Still sussing out bartleby?

Check out a sample textbook solution.

See a sample solution

The Solution to Your Study Problems

Bartleby provides explanations to thousands of textbook problems written by our experts, many with advanced degrees!

Get Started 