Question

Commercially available sulphuric acid contains 93% by mass and
has has a density of 1.84 g/cm3 . Calculate the volume of concentrated acid required to prepare 2.5mL of 0.50 M of H2SO4.

Answer 1

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Correct question - Conc. aq. sulphuric acid is 98% H2SO4 by mass and has a density of 1.84g cm-3. What volume of the concentrated acid is required to make 5 litres of 0.5M H2SO4?

Answer ⬇️

To make 0.5 M H2SO4, you need 0.5 moles/liter. To make 5 liters, you need 0.5 moles/L x 5 L = 2.5 moles of H2SO4.

Molar mass of H2SO4 is 98 g/mole. 2.5 moles x 98 g/mole = 245 g of H2SO4 needed.

1.84 g/ml (x ml) = 245 g and x = 133.15 ml needed, if it were pure, 100% H2SO4.

Correcting for the 98% purity, you need 133.15/0.98 = 135.87 ml of the 98% H2SO4.

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