Problem: Suppose 50.00 mL of 2.0 × 10–4 M Fe(NO3)3 is added to 50.00 mL of 2.0 ×10-6 M KIO3. Which of the following statements is true? For Fe(IO3)3, Ksp = 1.0 × 10–14.A) A precipitate forms because Qc > Ksp.B) A precipitate forms because Qc < Ksp.C) No precipitate forms because Qc < Ksp.D) No precipitate forms because Qc = Ksp.E) No precipitate forms because Qc > Ksp.

FREE Expert Solution

We’re being asked to determine if a precipitate will form in the given reaction


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.


We're going to determine if a precipitate will form using the following steps:

Step 1. Write the Q expression.
Step 2. Determine the new concentrations of the ions in the solution formed.
Step 3. Calculate Q.
Step 4. Compare Q and Ksp.

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Problem Details

Suppose 50.00 mL of 2.0 × 10–4 M Fe(NO3)3 is added to 50.00 mL of 2.0 ×10-6 M KIO3

Which of the following statements is true? For Fe(IO3)3, Ksp = 1.0 × 10–14.

A) A precipitate forms because Qc > Ksp.

B) A precipitate forms because Qc < Ksp.

C) No precipitate forms because Qc < Ksp.

D) No precipitate forms because Qc = Ksp.

E) No precipitate forms because Qc > Ksp.

Frequently Asked Questions

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.