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).
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?

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  1. 1.
    mL x M = mL x M

    2. How much does 1 L of the solution weigh.
    1.84*1000 mL = 1840
    How many grams H2SO4 are there? 18.4 moles x 98 g/mol = 1803.2 (confirm that).
    %H2SO4 = (g H2SO4/g solution)*100 = ??
    3. This is a stoichiometry problem. Here is a solved example problem. Just follow the steps. (The other product is Na2SO4.)
    4. Take 1,000 mL of the solution. That's 5.2 M = 5.2 moles H2SO4/L soln
    How many g H2SO4 are in the soln? That's 5.2 x 98 g H2SO4/mol = 509.6 g
    How much does the soln weigh? That's 1.38 g/mL x 1000 mL = 1380 g.
    How much does the water weigh? That's 1380 g - 509.6 = ??
    molality = 5.2 moles/L soln.
    My answer is about 5.97 but you should confirm that.

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  2. 370 mL

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