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A sample of concentrated nitric acid has a density of 1.41

Principles of General Chemistry | 2nd Edition | ISBN: 9780073511085 | Authors: Martin S. Silberberg ISBN: 9780073511085 71

Solution for problem 72P Chapter 3

Principles of General Chemistry | 2nd Edition

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Principles of General Chemistry | 2nd Edition | ISBN: 9780073511085 | Authors: Martin S. Silberberg

Principles of General Chemistry | 2nd Edition

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Problem 72P

Problem 72P

A sample of concentrated nitric acid has a density of 1.41 g/mL and contains 70.0% HNO3 by mass.

(a) What mass of HNO3 is present per liter of solution?

(b) What is the molarity of the solution?

Step-by-Step Solution:

Solution 72P

Step 1 of 2

a.

Here, we have to calculate the mass of HNO3 is present in the litre solution.

Density:

The ratio of the mass of an object to its volume.

Density = 

Let’s calculate the mass of HNO3 Solution

Given

Volume of solution = 1L

Density = 1.41 g/mL.

Write the equality and conversion factor.

1 g = 1ml

1 L = 103 ml.

So, the conversion factors are  and 

Mass = Density  x  volume.

         = 1.41  

        = 1410 g/L.

Let’s calculate the mass of solution per one litre.

If the solution is 100g, the given Mass % of HNO3 is 70.0%.

Mass of HNO3 solution =

Given

Total mass of solution =100g

Mass of HNO3 = 70g

Mass of solution per litre = 1410 g/L

Mass of HNO3 Solution = 

                                       = 987 g/L.

Therefore, mass of HNO3 solution per litre is 987 g/L.

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Step 2 of 2

Chapter 3, Problem 72P is Solved
Textbook: Principles of General Chemistry
Edition: 2
Author: Martin S. Silberberg
ISBN: 9780073511085

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A sample of concentrated nitric acid has a density of 1.41