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