# 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. ###### 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