The calcium hydroxide was acted upon with nitric acid weighing 3.15 g.

| February 7, 2021 | education

The calcium hydroxide was acted upon with nitric acid weighing 3.15 g. What mass of calcium nitrate did you get if the mass fraction of its yield is 90% of the theoretical possible?

1. Let’s write the reaction equation:

Ca (OH) 2 + 2HNO3 = Ca (NO3) 2 + 2H2O

2. Find the amount of nitric acid:

n (HNO3) = m (HNO3) / M (HNO3) = 3.15 g / 63 g / mol = 0.05 mol.

3. According to the reaction equation, we find the theoretical amount of calcium nitrate:

ntheor (Ca (NO3) 2) = 0.5n (HNO3) = 0.025 mol.

4. Find the practical amount and then the mass of salt:

nprak (Ca (NO3) 2) = ntheor (Ca (NO3) 2) * η (Ca (NO3) 2) / 100% = 0.025 mol * 90% / 100% = 0.0225 mol.

m ((Ca (NO3) 2)) = nprak (Ca (NO3) 2) * M ((Ca (NO3) 2)) = 0.0225 mol * 164 g / mol = 3.69 g.

Answer: m ((Ca (NO3) 2)) = 3.69 g.



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