Determine the mass fractions of sulfuric and nitric acids in the solution if, when an excess of barium chloride was added to 200 g

Determine the mass fractions of sulfuric and nitric acids in the solution if, when an excess of barium chloride was added to 200 g of this solution, 46.6 g of precipitate was released, and to neutralize the resulting solution, 50 ml of a 30% sodium hydroxide solution with a density of 1.33 g / ml were required …

H2SO4 + BaCl2 → BaSO4 ↓ + 2HCl
HNO3 + NaOH → NaNO3 + H2O
m (BaSO4) = 46.6 g
n (BaSO4) = 46.6 / 233 = 0.2 mol
n (NaOH) = (50 x 0.3 x 1.33) / 40 = 0.5 mol
⇒ n (H2SO4) = 0.2 mol
n (HNO3) = 0.5 mol
⇒ m (H2SO4) = 0.2 x 98 = 19.6 g
m (HNO3) = 0.5 x 63 = 31.5 g
ω (H2SO4) = 19.6 / 200 x 100% = 9.8%
ω (HNO3) = 31.5 / 200 x 100% = 15.75%
Answer: the mass fractions of sulfuric and nitric acid in the solution are respectively equal to 9.8% and 15.75%.