Find the mass of an 18.3% sulfuric acid solution capable of reacting with 12.2 liters

Find the mass of an 18.3% sulfuric acid solution capable of reacting with 12.2 liters of methylamine to form a medium salt.

We write down the equation of reactions.
2CH3NH2 + H2SO4 = (CH3NH3) 2SO4
Using the reaction equation, we find the volume of sulfuric acid.
X l H2SO4 – 12.2 l CH3NH2
22.4 L H2SO4 – 3 * 22.4 L CH3NH2
X = 22.4 * 12.2: (3 * 22.4) = 273.28 / 67.2 = 4.07 l.
We find the mass of sulfuric acid.
n = m / M.
n = V / Vm.
m / M = V / Vm.
Find the molar mass of sulfuric acid.
M (H2SO4) = 1 * 2 + 32 + 16 * 4 = 98 g / mol.
m = V * M / Vm = 4.07 * 98 / 22.4 = 17.8 g H2SO4.
m solution = m (H2SO4) / W (H2SO4) = 17.8 g / 0.183 = 97.3 g H2SO4.
This means that the mass of the sulfuric acid solution is 97.3 g.
Answer: m (H2SO4) = 97.3 g.