Determine the mass of the precipitate formed by the interaction of 980 g of a 25% phosphoric acid
Determine the mass of the precipitate formed by the interaction of 980 g of a 25% phosphoric acid solution with calcium hydroxide.
Let’s find the mass of Н3РО4 in solution.
W = m (substance): m (solution) × 100%,
m (substance) = (m (solution) × W): 100%.
m (H3PO4) = (980 g × 25%): 100% = 245 g.
Let’s find the amount of substance Н3РО4.
M (H3PO4) = 98 g / mol.
n = m: M.
n (H3PO4) = 245 g: 98 g / mol = 2.5 mol.
Let’s compose the reaction equation, find the quantitative ratios of substances.
2H3PO4 + 3Ca (OH) 2 = Ca3 (PO4) 2 ↓ + 6H2O.
According to the reaction equation, there is 1 mol of Ca3 (PO4) 2 per 2 mol of Н3РО4. The substances are in quantitative ratios of 2: 1. The amount of Ca3 (PO4) 2 is 2 times less than the amount of H3PO4.
n (Ca3 (PO4) 2) = ½ n (H3PO4) = 2.5: 2 = 1.25 mol.
Let’s find the mass of Ca3 (PO4) 2.
m = n × M,
M (Ca3 (PO4) 2) = 310 g / mol.
m (Ca3 (PO4) 2) = 310 g / mol × 1.25 mol = 387.5 g.
Answer: 387.5 g.