In: Chemistry
A solid mixture consists of 51.0 g of KNO3 (potassium nitrate) and 9.0 g of K2SO4 (potassium sulfate). The mixture is added to 130. g of water. Part B If the solution described in the introduction is cooled to 0 ∘C, what mass of KNO3 should crystallize?
Solubility:
When the maximum amount of solute is dissolve in the solvent is called solubility. On the basic of solubility the solution are following types:
Saturate solution:
A solution which contains the maximum amount of dissolved solute at the equilibrium is called saturated solution.
Un-saturate solution:
A solution which contains lesser amount of solute as compare to saturated solution. It will be able to dissolver more solute.
Super -Saturate solution:
A solution which contains the more dissolved amount of solute as compare to saturated solution.
According to the problem;
There is Initially 51.0 g of KNO3 (potassium nitrate) and 9.0 g of K2SO4 (potassium sulfate). are added to 130 g of water.
These means 51.0g of KNO3 is dissolved in 130g of water.
From the other sources like solubility graph or book we know that
14 g KNO3 is soluble in 100g water at 00C
So, amount of KNO3 soluble in 130g water = 14 / 100 * 130
= 18.2 g
Here 51.0 g KNO3 present; out of which 18.2 g KNO3 is soluble
So, amount of KNO3 crystallizes 51.0 – 18.2 = 32.8 g KNO3 will get crystallized