When 120 g of 20% sulfuric acid solution interacted with barium hydroxide solution, a precipitate was formed
When 120 g of 20% sulfuric acid solution interacted with barium hydroxide solution, a precipitate was formed. Calculate the mass of the sediment if the practical yield is 97% of the theoretically possible value.
1. We write down the reaction equation:
H2SO4 + Ba (OH) 2 = BaSO4 ↓ + 2H2O;
2.calculate the mass of sulfuric acid:
m (H2SO4) = w (H2SO4) * m (solution);
m (H2SO4) = 0.2 * 120 = 24 g;
3. find the theoretical chemical amount of sulfuric acid:
ntheor (H2SO4) = m (H2SO4): M (H2SO4);
M (H2SO4) = 2 + 32 + 4 * 16 = 98 g / mol;
ntheor (H2SO4) = 24: 98 = 0.245 mol;
4.According to the equation of the ongoing reaction, the theoretical amount of barium sulfate:
ntheor (BaSO4) = ntheor (H2SO4) = 0.245 mol;
5. find the practical amount of sediment:
npract (BaSO4) = ntheor (BaSO4) * ν = 0.245 * 0.97 = 0.23765 mol;
6.Calculate the mass of the sediment:
m (BaSO4) = ntract (BaSO4) * M (BaSO4);
M (BaSO4) = 137 + 32 + 4 * 16 = 233 g / mol;
m (BaSO4) = 0.23765 * 233 = 55.37 g.
Answer: 55.37 g.