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5 kg of a saturated solution of KNO3 at 70°C is cooled to 10°C. After equilibrium...

5 kg of a saturated solution of KNO3 at 70°C is cooled to 10°C. After equilibrium is established, what mass of KNO3 crystals have precipitated from solution? What percentage of the KNO3 originally in solution has precipitated?

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Answer #1

solubility of KNO3 at 75?C = 155 g per 100 g of water

solubility of KNO3 at 10?C = 23 g per 100 g of water

5 kg of saturated solution at 75?C

solution will contain =

5000 g solution x 155 g KNO3/(155+100)g solution

= 3039 g KNO3

Mass of water in initial solution

m water = 5000 ?3039 = 1961 g

KNO3 can be dissolved in 1961 g at 10°C

= 1961 g water x 23 g KNO3/(100)g water

= 451.03 g KNO3

mass of KNO3 crystals have precipitated from solution

= 1961 - 451.03 = 1509.97 g = 1.51 kg

% KNO3 = 1.51 x 100/5 = 30.20%

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