Problem: The Ksp of AgCl at 25 °C is 1.6 x 10-10. Consider a solution that is 1.0 x 10-2 M CaCl2 and 1.0 x 10-8 M AgNO3.

FREE Expert Solution

We’re being asked to determine if a precipitate will form when 1.0 x 10-2 M CaCl2 and 1.0 x 10-8 M AgNO3. are mixed.


For this, we need to compare the reaction quotient (Q) vs. the solubility product constant (Ksp)

Recall that when:

• 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 expected precipitate is AgCl. The chloride ion, Cl, has a charge of –1. Ag then has a charge of +1. 

The dissociation of AgCl in water is as follows:

AgCl(s)  Ag+(aq) + Cl(aq)


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Problem Details

The Ksp of AgCl at 25 °C is 1.6 x 10-10. Consider a solution that is 1.0 x 10-2 M CaCl2 and 1.0 x 10-8 M AgNO3.

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Selective Precipitation concept. If you need more Selective Precipitation practice, you can also practice Selective Precipitation practice problems.