Question

Calculate the weight of pure H2SO4 required to prepare 500 ml of a 0.05 M H2SO4 solution.

Answer 1

Do you have the density of pure H2SO4? I THINK that's 1.83 g/mL but you should confirm that. So what is the molarity of pure H2SO4?

1.83 g/mL x 1,000 mL x (1/98) = 18.7 moles/L = 18.7 M
What volume of this solution must be used to prepare the 0.05 M solution. That is mLa x Ma = mLb x M b
mLa x 18.7 = 500 mL x 0.05
mLa = 1.34 is required. How much will that weight?
density = 1.83 g/mL
mass = volume x density
mass = 1.34 mL x 1.83 g/mL = ? grams H2SO4 needed.