# 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 &gt; Ksp.B) A precipitate forms because Qc &lt; Ksp.C) No precipitate forms because Qc &lt; Ksp.D) No precipitate forms because Qc = Ksp.E) No precipitate forms because Qc &gt; 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. ###### 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.