Concentrated sulfuric acid is 18.4 molar and has a density of 1.84 grams per milliliter. After dilution with water to 5.20 molar the solution has a density of 1.38 grams per milliliter. This concentration of H2SO4 is often used in lead storage batteries(like a car battery).

Question

1.Calculate the volume of concentrated H2SO4 needed to make 1.00L of 5.20 molar solution.
2.Calculate the % concentration H2SO4 in the concentrated solution.
3.Calculate the volume of 5.20 molar H2SO4 required to react completely with 100.0 grams of NaHCO3. (Carbon dioxide and water are two of the three products of this reaction-can you figure out the other?)
4.What is the molality of the 5.20 molar H2SO4 solution?
I understand 3 and 4.
1 I don't understand mL x M = mL x M ??
2. Is number 2. (1803.2/1840)x100=98%H2SO4

Answer 1

mL x M = mL x M is the dilution formula.
mL of the concd acid is the unknown.
M of the concd acid is 18.4 M
mL of the diluted solution is 1,000 mL (you want 1.00 L). M of the diluted solution is 5.20M. Solve for the only unknown which is mL of the concd acid you need to use to dilute to 1.00 L to make the 5.20L..
Yes, it is 98% H2SO4.
This post is so far down that any follow up questions should be directed at the top of the page (make a new post that is) so someone will see it sooner.