An aqueous stock solution is 85.0% H2SO4 by mass and its density is 1.83 g/mL. What volume of this solution is required to make 1.00 L of 1.35 mol/L H2SO4(aq)? Give your answer in millilitres, accurate to three significant figures.

Answer 1

What's the molarity of the H2SO4 you have?
That's 1.83 g/mL x 1000 mL x 0.85 x (1 mol/98g) = approx 16 M but you need a more accurate answer.

Then c1v1 = c2v2
16M*v = 1.35M x 1000mL
Solve for v in mL but remember to get a better answer for that 16M.