Question

What volume, in mL, of concentrated 16 M nitric acid would you need to use in order to prepare 500.0 mL of a 0.250 M HNO3(aq) solution?

Answer 1

Given :

Initial concentration of nitric acid, $C_1 = 16\ M$.

Final concentration of nitric acid, $C_2 = 0.250 \ M$.

Volume of $HNO_3$, $V _2= 500\ mL = 0.5\ L .$

To Find :

Volume needed( $V_1$ ).

Solution :

We know,

$C_1V_1 =C_2V_2\\\\16 \times V_1 = 0.250 \times 0.5 \\\\V_1 = \dfrac{0.250 \times 0.5}{16}\\\\V_1 = 0.0078125\ L = 7.8125 \ mL$

Hence, this is the required solution.