Question

How many mL of H2SO4 solution (density = 1.1783) containing 25.0%(w/w) H2SO4 are required to prepare 1800 mL of 0.1000 N solution?

Answer 1

Normality of acid = Molarity x Number of H+ ions

We are given the normality and the volume of acid solution. From it, we will calculate moles of acid.

Mol = molarity x volume in L

Molarity = Normality / number of proton per acid molecule = 0.1000 / 2 = 0.0500

Mol = 0.0500 M x 1.800 L = 0.09 mol

Now we need to calculate volume of acid

We know,

Molarity = moles / volume in L

Therefore,

Volume in L = moles / molarity

Calculation of molarity

Molarity = (mas in g / molar mass) / Volume of solution in L     ….(I)

Density = mass / volume

Lets plug density formula into equation I,

Molarity = (mass in g )/( (volume of solution in mL / 1000) x molar mass )

Molarity = ( density x 1000) / molar mass = (1.1783 g/mL) x 1000 / 98.079 g per mol

=12.014 M

Volume in L = mol / molarity = 0.09 mol / 12.014 M = 0.007491 L = 7.5 mL

Volume of H2SO4 required would be 7.5 mL