Question

If (0.1M , {Pb(C}_2{H}_3{O}_2)_2) is added to shift the equilibrium, which statement is true? Check all that apply.

Options:
a. PbBr₂(s) + Pb²⁺(aq) + 2Br⁻(aq) is formed
b. Pb(C₂H₃O₂)₂ is consumed
c. The concentration of Pb²⁺ increases
d. The concentration of Br⁻ decreases

Answer 1

Adding 0.1M Pb(C2H3O2)2 to the system will result in Pb(C2H3O2)2 being consumed and an increase in the concentration of Pb2+ ions, as per Le Châtelier's Principle.

Step-by-step explanation:

If 0.1M Pb(C2H3O2)2 is added to a system at equilibrium, we must consider Le Châtelier's Principle to determine how the system will respond. When Pb(C2H3O2)2 is added, it will dissociate into Pb2+ and C2H3O2− ions. As a result, the concentration of Pb2+ ions will increase, causing a shift that opposes this change.

Considering the system PbCl2 (s) = Pb2+ (aq) + 2Cl− (aq), the addition of Pb2+ from Pb(C2H3O2)2 will shift the equilibrium towards the solid PbCl2, leading to an increased precipitation and a decrease in the solubility of PbCl2. Therefore, answers (b) and (c) are true: Pb(C2H3O2)2 is consumed and the concentration of Pb2+ increases.