   # A solution was prepared by mixing 50.00 mL of 0.100 M HNO 3 and 100.00 mL of 0.200 M HNO 3 . Calculate the molarity of the final solution of nitric acid. ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

#### Solutions

Chapter
Section ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 6, Problem 40E
Textbook Problem
1509 views

## A solution was prepared by mixing 50.00 mL of 0.100 M HNO3 and 100.00 mL of 0.200 M HNO3. Calculate the molarity of the final solution of nitric acid.

Interpretation Introduction

Interpretation: To calculate the final molarity of this mixture of 50ml of 0.100MHNO3 and 100mlof0.200MHNO3 .

Concept Introduction:  The number of moles of solute dissolved in one litre of solution.

Formula:

Mole=volumeofsolution (L)×molarity (M)litre (L) (1)

### Explanation of Solution

Explanation

Volume and molarity of HNO3 is = 50ml and 0.100M

Calculate the moles of 50mlof0.100M

Mole of HNO3 solution = 0.005mole which is calculated as follows,

Substitute volume and molarity in formula (1) we get the mole of solutions.

Mole=volumeofsolution (L)×molarity (M)litre (L) (1)

Substitute the volume and molarity of solution in mole formula (1) to get mole of HNO3 solution

Given:

Volume = 0.05L

Molarity = 0.100M

= 0.05(L)×0.100(M)1(L)

Mole of HNO3 solution (1) = 0.005mole

Volume and molarity of HNO3 is 100ml and 0.200M the volume is divided by 1000 we get L

• calculate the moles of 0.1 Lof0

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