Problem: In which of the following mixtures will a precipitate form? Circle all that apply.a) 10.0 mL of 0.010 M AgNO 3 and 10.0 mL of 0.10 M Na 2SO4 (Ksp for Ag2SO4 = 1.2 x 10 -5)b) 1.0 mL of 0.10 M Ca(NO 3)2 and 1.0 L of 0.010 M NaF (K sp for CaF2 = 3.45 × 10 -11)c) 50.0 mL of 0.0020 M AgNO 3 and 250.0 mL of 0.020 M KBrO 3 (Ksp for AgBrO3 = 1.2 x 10 -11)A. a) and b)B. a) and c)C. b) and c)D. All of the aboveE. None of the above

FREE Expert Solution

We’re being asked to determine which of the given solutions a precipitate will form

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

In which of the following mixtures will a precipitate form? Circle all that apply.

a) 10.0 mL of 0.010 M AgNO 3 and 10.0 mL of 0.10 M Na 2SO4 (Ksp for Ag2SO4 = 1.2 x 10 -5)

b) 1.0 mL of 0.10 M Ca(NO 3)2 and 1.0 L of 0.010 M NaF (K sp for CaF2 = 3.45 × 10 -11)

c) 50.0 mL of 0.0020 M AgNO 3 and 250.0 mL of 0.020 M KBrO 3 (Ksp for AgBrO3 = 1.2 x 10 -11)


A. a) and b)

B. a) and c)

C. b) and c)

D. All of the above

E. None of the above

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.