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?

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...