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# Nitric acid is usually purchased in concentrated form with ISBN: 9780321910295 34

## Solution for problem 119P Chapter 13

Introductory Chemistry | 5th Edition

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Problem 119P

Nitric acid is usually purchased in concentrated form with a 70.3% HNO3 concentration by mass and a density of 1.41 g/mL. How much of the concentrated stock solution in milliliters should you use to make 2.5 L of 0.500 M HNO3?

Step-by-Step Solution:

You should use 79.45 ml of the stock solution and make it up to a volume of 2.5L

Explanation:

You need 2.5L of 0.5M HNO3 solution.

C = nV

So:

n = CV

So the no. moles HNO3 required = 2.5×0.5=1.25

Now we need to find how many grams this is. We get this by multiplying by the weight of 1 mole of HNO3 which is equal to its Mr (mass required) in grams.

Mr[HNO3]= 63.01

So mass required = 1.25×63.01=78.76g

We know that the concentrated form is 70.30% by mass.

This means that 100g of this concentrated solution contains 70.30g of HNO3.

So...

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##### ISBN: 9780321910295

Introductory Chemistry was written by and is associated to the ISBN: 9780321910295. Since the solution to 119P from 13 chapter was answered, more than 525 students have viewed the full step-by-step answer. This full solution covers the following key subjects: Concentrated, hno, milliliters, Density, form. This expansive textbook survival guide covers 19 chapters, and 2045 solutions. This textbook survival guide was created for the textbook: Introductory Chemistry, edition: 5. The full step-by-step solution to problem: 119P from chapter: 13 was answered by , our top Chemistry solution expert on 05/06/17, 06:45PM. The answer to “Nitric acid is usually purchased in concentrated form with a 70.3% HNO3 concentration by mass and a density of 1.41 g/mL. How much of the concentrated stock solution in milliliters should you use to make 2.5 L of 0.500 M HNO3?” is broken down into a number of easy to follow steps, and 41 words.

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