Calculate the mass of a nitric acid solution with a mass fraction of HNO3 52%

| September 17, 2021 | education

Calculate the mass of a nitric acid solution with a mass fraction of HNO3 52% required to obtain copper (II) nitrate with a chemical amount of 0.1 mol from copper (II) oxide.

Let’s write down given:

n (Cu (NO3) 2) = 0.1 mol

W (HNO3) = 52% or 0.52

m solution (HNO3) -?

Solution.

Let us write the equation for the reaction of the interaction of copper oxide () with nitric acid:

CuO + 2 HNO3 = Cu (NO3) 2 + H2O

M (HNO3) = 1 + 14 + 3 * 16 = 63 g / mol

According to the reaction equation, 1 mol (Cu (NO3) 2) is formed from 2 mol (HNO3)

According to the condition of the problem, 0.1 mol (Cu (NO3) 2) is formed from x mol (HNO3)

X = 0.1 mol * 2 mol / 1 mol = 0.2 mol (HNO3)

Let’s calculate the mass of the formed acid:

m (HNO3) = 63 g / mol * 0.2 mol = 12.6 g

Let’s calculate the mass of the acid solution:

W = m (substance) * 100% / m (solution)

m (solution) = m (substance) * 100% / W

m solution (HNO3) = 12.6 * 100% / 52% = 24.23 g

Answer: 24.23 g solution (HNO3)



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