Stock solutions of nitric acid have concentration of 16.0 m. what volume of stock solution is needed to prepare 2.00 l of 2.00 m solution of nitric acid by dilution with water?

0.083 L of concentrated 12.0M HNO3

This is a dilution chemistry problem. For problems like this one, use the following equation

M1V1=M2V2

Where
M1=molarity of solution 1
V1=volume of solution 1
M2=molarity of solution 2
V2=volume of solution 2

Whenever you dilute a concentrated stock solution, or for that matter, any solution, you are essentially changing the volume of that solution by adding water. If we look at what Molarity exactly is,

Molarity=moles1 Liter solution

you can see when you increase the volume, you decrease the molarity(concentration). In dilution cases, you are adding water so moles of the solute do not change, only the volume of the solution changes.

Using our equation from above, we can find the number of moles of nitric acid, HNO3, from what we are given.

We will let M1 and V1 be 8.0M and 125 mL respectively. Make sure to convert mLto L first. For M2, use the 12.0M. Isolate V2 and solve.

0.083 L

a is the answer to this question

explanation: