The amount of i₃⁻(aq) in a solution can be determined by titration with a solution containing a known concentration of s₂o₂⁻³(aq) (thiosulfate ion). the determination is based on the net ionic equation 2s₂o₃²⁻(aq)+i₃⁻(aq)⟶s₄o₆²⁻(aq)+3i⁻( aq). given that it requires 38.1 ml of 0.440 m na₂s₂o₃(aq) to titrate a 25.0 ml sample of i₃⁻(aq), calculate the molarity of i₃⁻(aq) in the solution.

The answer is b because a,c,and d are opinons

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.