Question

You can purchase nitric acid in a concentrated form that is 70.3% HNO3 by mass and has a density of 1.41 g/mL. Describe exactly how you would prepare 1.15 L of 0.100 M HNO3 from the concentrated solution.

Answer 1

The key to working out the numbers is to multiply the amount of HNO3 needed by the molarity to find out how many moles you need: 0.115. You should be able to figure out the formula weight H is 1, N is 14, O is 16. The product of the number of moles multiplied by the formula weight should give a value in grams. You can use the density to convert to a volume of HNO3 to add to the correct volume of water (note always add concentrated acid to water, rather than the other way round). If you want to try the calculations I'll do them too and we can see if we agree. Best wishes,

Answer 2

Your solution is very convincing, @ebaxter01 - you deserve more than just a medal and a testimonial, but that's all I can give you. Thanks a lot! :D