🤓 Based on our data, we think this question is relevant for Professor Hummel's class at UIUC.
• Q > Ksp: the solution is supersaturated and a precipitate will form. Reactants are favored.
• Q = Ksp: the solution is at equilibrium and no precipitate will form.
• Q < Ksp: the solution is unsaturated and no precipitate will form. Products are favored.
The sulfate ion, IO3–, has a charge of –1. Ce then has a charge of +3.
The dissociation of Ce(IO3)3(s) in water is as follows:
Ce(IO3)3(s) ⇌ Ce3+(aq) + 3 IO3–(aq)
Calculate the reaction quotient for Ce(IO3)3 is:
Note that each concentration is raised by the stoichiometric coefficient: [Ce3+] is raised to 1 and [IO3–] is raised to 3.
Solving for Q:
A solution contains 2.0 X 10 -3 M Ce3+ and 1.0 X 10 -2 M IO3 3-. Will Ce(IO3)3(s) precipitate? [Ksp for Ce(IO3)3 is 3.2 X 10-10.]