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.

Step-by-step 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 * V_(1) = 1.00 M * 250 mL\\V_(1) = (1.00 M * 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.