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Get Full Access to Introductory Chemistry - 5 Edition - Chapter 13 - Problem 119p
Get Full Access to Introductory Chemistry - 5 Edition - Chapter 13 - Problem 119p

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# Solved: Nitric acid is usually purchased in concentrated form with a 70.3% HNO3

ISBN: 9780321910295 34

## Solution for problem 119P Chapter 13

Introductory Chemistry | 5th Edition

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Problem 119P

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:
Step 1 of 3

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 now we need to work out what volume of concentrated solution will give us the mass we need:

There are:

70.30g HNO3 in 100 g of concentrated solution.

1g is present in 100/70.30g of concentrated solution.

So:

78.76g is present in 100/70.30×78.76=112.03g of concentrated solution.

The density of the solution = 1.41g/ml

density = mass/volume

So volume = mass/density

So the volume required = =79.45ml

Step 2 of 3

Step 3 of 3

##### 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 823 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 2046 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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