# 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?

May 12, 2017

You know you should add acid to water.................I get approx., $71 \cdot m L$

#### Explanation:

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

$\text{Molarity or concentration"="Moles of solute"/"Volume of solution}$

And thus, since ${C}_{1} {V}_{1} = {C}_{2} {V}_{2}$........(because the moles of solute was a constant and depends on the initial concentration).

${V}_{2} = \frac{{C}_{1} {V}_{1}}{C} _ 2 = \frac{250 \cdot m L \times 4.5 \cdot m o l \cdot {L}^{-} 1}{3.5 \cdot m o l \cdot {L}^{-} 1} = 321.4 \cdot m L$

But since ${V}_{1} = 250 \cdot m L$, we need to ADD $71.4 \cdot m L$ to the initial $250 \cdot m L$ volume to give the required concentration.