The solubility of cr(no3)3⋅9h2o in water is 208 g per 100 g of water at 15 ∘c. a solution of cr(no3)3⋅9h2o in water at 35 ∘c is formed by dissolving 310 g in 100 g water. when this solution is slowly cooled to 15 ∘c, no precipitate forms. at equilibrium, what mass of crystals do you expect to form?

102g of crystals

Explanation:

When the Cr(NO₃)₃⋅9H₂O is dissolved in water at 15°C, the maximum mass that water will dissolve in the equilibrium is 208 g per 100g of water. When you heat the water, this mass will increases.

In this problem, at 35°C the water dissolves 310g in 100g of water, as in the equilibrium at 15°C the maximum mass is 208g, the mass of crystals that will form is:

310g - 208g = 102g of crystals

-Crystals are the Cr(NO₃)₃⋅9H₂O that is not dissolved-.

I hope it helps!

pie chart because it is in percents ( % )