A 3.0 mL sample of HNO_3HNO3 solution is exactly neutralized by 6.0 mL of .50 M KOHKOH. What is the molarity of the HNO_3HNO3 solution?

1 Answer
Apr 25, 2016

The key in any neutralization problem is to match the number of moles of acid and base.

Explanation:

In this case, the number of moles of base is
6.0 mL times (1 L)/(1000 mL) times 0.50 (mol)/L = 3.0 times 10^-3 mol6.0mL×1L1000mL×0.50molL=3.0×103mol

This must be equal to the number of moles of HNO_3HNO3, so the concentration of that solution must be:
(3.0 times 10^-3 mol)/(3.0 mL) times (1000 mL)/(1L) = 1.0 (mol)/L3.0×103mol3.0mL×1000mL1L=1.0molL