Question

To what volume should you dilute 30 mL of a 11 M H2SO4 solution to obtain a 0.17 M H2SO4 solution?

Answer #1

Given,

We have 30 mL of a 11 M H2SO4 solution

Volume = 30 mL = 0.03 L

Molarity = 11 M

We know that,

Moles = Molarity x Volume (in L)

=> Moles of H2SO4 = 11 x 0.03 = 0.33 moles of H2SO4

Now we need to add water to this solution so this becomes 0.17 M in concentration.

Moles of H2SO4 = 0.33 moles

Let final volume of solution = V liters

Molarity = Moless / Volume

=> 0.17 = 0.33 / V

=> V = 1.941 liters.

Therefore, **we have to dilute the solution to 1941
mL**

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