A solid mixture consists of 34.0g of KNO3 and 6.0g of K2SO4. The mixture is adde

Question

A solid mixture consists of 34.0g of KNO3 and 6.0g of K2SO4. The mixture is added to 130.0g of water. (this problem includes a solubility curve for other answers).

If the solution is cooled to 0 C, what mass of K2SO4 should crystallize?

*At 0 C on the solubility curve, K2SO4 is at approx 8g/100g H2O.

***I have put in 10.4 g and tried 8 g and even 6 g but it is more than the 6.0 g of original K2S04. I know that all of remains dissolved. Now I don't understand what mass of K2SO4 should crystallize.

Explanation / Answer

what mass of K2SO4 should crystallize. help for this the solubility of K2SO4 is 10.4/130=0,08g(K2SO4)per gram of water. in your mixture, you have 7.8/52=0,15g(K2SO4)per gram of water. which means that in your mixture, not all the K2SO4 is dissolved, (some precipitate). so only what was dissolved will crystalyse, and this correspond to : 0,08*(52-7.8)=3,536g. (52g of mixture correspond to 44.2g of water and 7.8g of K2SO4)

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