We’re asked to determine the mass of Cr(NO3)3•9H2O crystals expected to form at equilibrium based on its solubility at 15°C.
Recall that a saturated solution contains the maximum amount of solute that can be dissolved in a solvent at a particular temperature.
We know that 313 g of Cr(NO3)3•9H2O is dissolved in 100 g water at 35°C to make a solution.
When this solution is cooled to 15°C; no precipitate forms.
We're given the solubility of Cr(NO3)3•9H2O at 15°C.
We will now find the mass of Cr(NO3)3•9H2O crystals that will precipitate at equilibrium or in a saturated solution.
The solubility of Cr ( NO3 )3 9 H2O in water is 208 g per 100 g of water at 15 oC. A solution of Cr ( NO3 )3 9 H2O in water at 35 oC is formed by dissolving 313 g in 100 g water. When this solution is slowly cooled to 15 oC, no precipitate forms.
At equilibrium, what mass of crystals do you expect to form?
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