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25 May, 00:19

How many milliliters of concentrate sulfuric acid, which is 96% (w/w) pure H2SO4, are needed to prepare 500.0 mL of a 2.0 M solution of sulfuric acid?

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  1. 25 May, 00:37
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    We need 5.55 mL of H2SO4

    Explanation:

    Step 1: Data given

    96% (w/w) pure H2SO4

    We want to prepare 500.00 mL of a 2.0 M solution of H2SO4

    Molar mass of H2SO4 is 98.08 g/mol

    Density of H2SO4 = 1.84 g/mL

    Step 2: Calculate moles H2SO4

    0.2 M means we have 0.2 moles / 1L

    Moles = molarity * volume

    Moles = 0.2 M * 0.500 L = 0.100 moles of H2SO4

    0.2M = 0.2 mole/L

    Therefore, 0.5L * 0.2M = 0.1 mole of H2SO4 required.

    Step 3: Calculate mass H2SO4 required

    Mass = moles * molar mass

    Mass = 0.100 moles * 98.08 g/mol = 9.808 grams

    Step 4: Calculate volume needed

    Volume = mass / density

    Volume = 9.808 grams / 1.84 g/mL

    Volume = 5.33 mL

    This would be if the purity of H2SO4 was 100%

    The purity of your substance is 96%, therefore you will actually need:

    Volume needed = 5.33 * (1/0.96) = 5.55 mL.

    We need 5.55 mL of H2SO4
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