Answer:
We need 5.55 mL of H2SO4
Step-by-step 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