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 1 of 3
You should use 79.45 ml of the stock solution and make it up to a volume of 2.5L
You need 2.5L of 0.5M HNO3 solution.
C = nV
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.
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.
Textbook: Introductory Chemistry
Author: Nivaldo J Tro
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.