What mass of a nitric acid solution (the mass fraction of HNO3 in it is 7%) must be spent on the reaction

| March 1, 2021 | education

What mass of a nitric acid solution (the mass fraction of HNO3 in it is 7%) must be spent on the reaction with 5 mol of sodium carbonate?

Data: ωHNO3 – mass fraction of acid (ωHNO3 = 7% = 0.07); νNa2CO3 is the amount of sodium carbonate thing (νNa2CO3 = 5 mol).

Const: MHNO3 – molar mass of nitric acid (MHNO3 ≈ 63 g / mol).

1) The reaction level: Na2CO3 (sodium carbonate) + 2HNO3 (nitric acid) = 2NaNO3 (sodium nitrate) + CO2 ↑ (carbon dioxide) + H2O (water).

2) Amount of nitric acid: νHNO3 / νNa2CO3 = 2/1 and νHNO3 = 2 * νNa2CO3 = 2 * 5 = 10 mol.

3) The mass in the specified solution of pure nitric acid: mHNO3 = νHNO3 * MHNO3 = 10 * 63 = 630 g.

4) Required mass of solution: m = mHNO3 / ωHNO3 = 630 / 0.07 = 9000 g.

Answer: It is necessary to spend 9 kg of solution.



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