A 3.0 mL sample of #HNO_3# solution is exactly neutralized by 6.0 mL of .50 M #KOH#. What is the molarity of the #HNO_3# solution?

1 Answer
Apr 25, 2016

Answer:

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 mol#

This must be equal to the number of moles of #HNO_3#, so the concentration of that solution must be:
#(3.0 times 10^-3 mol)/(3.0 mL) times (1000 mL)/(1L) = 1.0 (mol)/L#