Problem: 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.]

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FREE Expert Solution

• 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.

For Ce(IO3)3(s):

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:

$\mathbf{Q}\mathbf{=}\frac{\mathbf{products}}{\overline{)\mathbf{reactants}}}\phantom{\rule{0ex}{0ex}}\mathbf{Q}\mathbf{=}\left[{\mathrm{Ce}}^{3+}\right]{\left[{{\mathrm{IO}}_{3}}^{-}\right]}^{\mathbf{3}}$

Note that each concentration is raised by the stoichiometric coefficient: [Ce3+] is raised to 1 and [IO3] is raised to 3.

Solving for Q:

Problem Details

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.]