A solution containing potassium bromide is mixed with one containing lead acetate to form a solution that is 0.013 M in KBr and 0.0035 M in Pb(C2H3O2)2. Does a precipitate form in the mixed solution? If so, identify the precipitate.

Verified step by step guidance

1. Identify the possible reaction: When potassium bromide (KBr) and lead acetate (Pb(C_2H_3O_2)_2) are mixed, the possible reaction is the formation of lead bromide (PbBr_2) and potassium acetate (K(C_2H_3O_2)).
2. Write the balanced chemical equation: KBr + Pb(C_2H_3O_2)_2 \rightarrow PbBr_2 + 2K(C_2H_3O_2).
3. Determine the solubility product (K_sp) for PbBr_2: Look up the K_sp value for lead bromide (PbBr_2) in a solubility table.
4. Calculate the ion product (Q) for PbBr_2: Use the concentrations of Pb^{2+} and Br^- ions in the mixed solution to calculate Q. The concentration of Br^- is twice that of KBr, and the concentration of Pb^{2+} is the same as Pb(C_2H_3O_2)_2.
5. Compare Q with K_sp: If Q > K_sp, a precipitate of PbBr_2 will form. If Q < K_sp, no precipitate will form.