1. The problem statement, all variables and given/known data How many mL of 50.0% by mass HNO3 solution, with a density of 2.00 g/mL is required to make a 500 mL of a 2.00 M HNO3? 2. Relevant equations initial Molarity X initial Volume = final Molarity X final Volume 3. The attempt at a solution (50 g HNO3)(1 mL/2.00 g)(0.001 L/1 mL) = 0.025 L (50 g HNO3)(1 mol HNO3/63.012 g HNO3) = 0.79 mol 0.79 mol/0.025 L = 31.6 M (500 mL)(2 M) = (31.6 M)V V = 31.6 mL Comments I don't know if the process that I used is right. Which leads me to doubt the answer. Any help is much appreciated.