Iron ores contain iron oxide minerals, which often contain ferric and ferrous ions. Such an ore can be analyzed for its iron content by dissolving it in acidic solution, reducing all the iron to ferrous ions, and then titrating with a standard solution of potassium permanganate. In the resulting solution, permanganate ion is reduced to manganese (II) ion, and ferrous ion is oxidized to ferric ion. A sample of iron ore weighed 0.3500 g. The titration required 41.56 mL of the permanganate solution (1.621 x 10-2 M) to reach the light purple end point. Determine the mass percent of iron in the iron ore.

Nonmetal are moldable and easily shaped

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.

Iknow this i just forgot the name