Name: Scenario
Your teacher writes on the board "Law of Conservation of Mass: Matter is not created or destroyed
in a chemical reaction, but rather transformed into new substances." Your teacher then sets up a
reaction with a test tube inside of a flask. The flask has a solution of sodium sulfate inside, while
the test tube has a solution of calcium chloride inside. Your teacher seals the flask and weighs it,
writing the mass on the board. The teacher then flips the flask over, so the two solutions mix. You
can see white flakes form in the solution. Your teacher re-weighs the flask, writing the mass again
on the board.
CaCl
solution
Caso, white
precipitate
in Naci
solution
Na so
solution

C. control over the business

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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.