A. At which temperature is a 90-gram sample of NH, a saturated solution?
B. How many grams are required to form a saturated solution of KCIO3
at 40 degrees Celsius?
C. What kind of solution is formed when 10 grams of SO2 dissolve at 10
degrees Celsius?
D. A solution is made by completely dissolving 70 grams of KNO3(s) in 100
grams of H20 in a beaker. The temperature of the solution is 43
Degrees Celsius. Determine the total mass of KNO3(s) that settles to the
bottom of the beaker when the original solution is cooled to 10 degrees
Celsius.

Answerthis solution will not form a precipitateexplanationsolubility equilbrium:         pbf₂(s)  ⇄ pb²⁺(aq) + 2 f⁻(aq)the solubility product expression is    (we exclude solids from the equilibrium expression).now suppose we have the trial ion product q, which we can define as    then, we can interpret  q as the product of the concentration of the ions that we have and ksp as the product of the ion concentrations that are needed to form a saturated solution.if q > ksp, then that implies that there will be a surplus of ions that exceed the amount that is required to form a saturated solution. a precipitate will then form (the precipitate continually  forms until the surplus ions are removed and q is decreased to ksp's value).if q = ksp, the saturated solution that forms is barely saturated and the precipitate will be minimal.if q < ksp, then the ion concentration will not be enough to form a saturated solution (so no precipitate).using our information, we calculate the trial ion product:     since q = 2.7  × 10⁻⁸ < ksp =  4  ×  10⁻⁸, a precipitate will not form.

Um i think answer is a

This is a solution, hope i could