Question

A sulfuric acid solution containing 571.6 g of H2SO4 per liter of aqueous solution has a density of 1.329 g/cm^3.Calculate:a. Mass percentageb. Mole fractionc. Molalityd. molarity of H2SO4 in this solution.

Answer 1

Given :

Mass of
`H_2SO_4` is 571.6 g per liter .

Density of solution ,
`\rho=1.329\ g/cm^3` .

To Find :

a. Mass percentage

b. Mole fraction

c. Molality

d. molarity of H2SO4 in this solution.

Solution :

Molar mass of
`H_2SO_4` , m = 1329 g/mol .

a ) Mass of
`H_2SO_4` contain in 1 liter is 1329 g .

`mass \ \%=(571.6)/(1329)* 100=43.01 \%`

b ) Moles of
`H_2SO_4` =
`(571.6\ g)/(98\g/mol)=5.83\ mol` .

Moles of
`H_2O` =
`(1329-571.6\ g)/(18\ g/mol)=42.08\ mol` .

Mole fraction
`=(5.83)/(5.83+42.08)=0.12` .

c ) Molarity of
`H_2SO_4`
`=(5.83\ mol)/(1 \ L)=5.83\ M` .

Hence , this is the required solution .