Question

What would be the final volume of a diluted solutions that was made by diluting 250 mL a 4.5M solutions of H2SO4 to make a 3.5M solution? How much water would have to be added to reach the final volume?

Answer 1

You know you should add acid to water.................I get approx., `71*mL`

Explanation:

Normally, we add ACID to WATER. However, the acid is not too concentrated, and so you would get away with reverse addition.

`"Molarity or concentration"="Moles of solute"/"Volume of solution"`

And thus, since `C_1V_1=C_2V_2`........(because the moles of solute was a constant and depends on the initial concentration).

`V_2=(C_1V_1)/C_2=(250*mLxx4.5*mol*L^-1)/(3.5*mol*L^-1)=321.4*mL`

But since `V_1=250*mL`, we need to ADD `71.4*mL` to the initial `250*mL` volume to give the required concentration.