How many grams of calcium phosphate is formed during the neutralization reaction of calcium hydroxide weighing 7.4 g?
Let’s implement the solution:
1. Let us write the equation according to the problem statement:
m = 7.4 g. X g -?
Ca (OH) 2 + H2SO4 = CaSO4 + 2H2O – ion exchange reaction, obtained a precipitate of calcium sulfate, water;
2. Let’s calculate the molar masses of inorganic substances:
M Ca (OH) 2 = 74 g / mol;
M (CaSO4) = 136 g / mol.
3. Calculate the number of moles of the starting material, if the mass is known:
Y Ca (OH) 2 = m / M = 7.4 / 74 = 0.1 mol;
Y CaSO4 = 0.1 mol since the amount of these substances according to the equation is 1 mol.
4. Find the mass of salt:
m (CaSO4) = Y * M = 0.1 * 136 = 13.6 g.
Answer: during the reaction, calcium sulfate with a mass of 13.6 g was obtained.
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