How many grams of a nitric acid solution with a mass fraction of HNO3 of 20% is required to neutralize a solution containing KOH, weighing 5.6 g
w% (HNO3) = 20%
m (KOH) = 5.6g
Find: m (HNO3) -?
1) Reaction equation:
HNO3 + KOH = KNO3 + H2O
2) Find the amount of KOH that has reacted:
n (KOH) = m: M = 5.6 g: 56 g / mol = 0.1 mol
3) We compose a logical expression:
If 1 mol of HNO3 requires 1 mol of KOH,
then x mol HNO3 requires 0.1 mol KOH,
then x = 0.1 mol HNO3.
4) Find the mass of nitric acid in solution:
m (HNO3) = n * M = 0.1 mol * 63 g / mol = 6.3 g HNO3
5) Find the mass of the acid solution that has reacted, based on its concentration:
m (solution HNO3) = 6.3 g: 0.2 = 31.5 g.
Answer: m (solution HNO3) = 31.5 g.
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