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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Chemistry

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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Answers (1)

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Oconnor · Answer 1

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