Question

a concentrated solution of sulfuric acid, H2SO4, has a concentration of 18.0 M. How many mL of the concentrated acid would be required to make 250. mL of a 1.00 MH2SO4 solution?

Answer 1

Answer: A 13.88 mL of the concentrated acid would be required to make 250. mL of a 1.00 M $H_{2}SO_{4}$ solution.

Explanation:

Given: $M_{1}$ = 18.0 M,     $V_{1}$ = ?

$M_{2}$ = 1.00 M,         $V_{2}$ = 250 mL

Formula used to calculate the volume of concentrated acid is as follows.

$M_{1}V_{1} = M_{2}V_{2}$

Substitute the values into above formula as follows.

$M_{1}V_{1} = M_{2}V_{2}\\18.0 M \times V_{1} = 1.00 M \times 250 mL\\V_{1} = \frac{1.00 M \times 250 mL}{18.0 M}\\= 13.88 mL$

Thus, we can conclude that 13.88 mL of the concentrated acid would be required to make 250. mL of a 1.00 M $H_{2}SO_{4}$ solution.