Final answer:
In an aqueous displacement reaction involving Li+ and Na+ ions, the equilibrium is likely to favor Li+ ions in solution due to lithium being more reactive than sodium, thus avoiding displacement by Na+. The addition of NaCl to PbCl2 solution demonstrates the common ion effect, decreasing PbCl2 solubility due to the influx of chloride ions.
Step-by-step explanation:
The likely position of the equilibrium in the aqueous displacement reaction involving Li+ and Na+ ions can be deduced based on the reactivity of the metals and their positions in the electrochemical series.
Lithium is more reactive than sodium, implying that in an equilibrium reaction, lithium is more likely to remain in solution as ions rather than being displaced by sodium ions.
In chemical terms, the displacement reaction will not proceed in the direction of sodium displacing lithium; rather, the reaction will favor lithium ions in solution and solid sodium, if present.
Common ion effect plays an important role in the solubility equilibria of ionic compounds. In the case of adding sodium chloride to a saturated solution of lead(II) chloride, the added chloride ions from NaCl increase the chloride concentration in the solution.
Since the concentration of lead(II) ions is fixed at 1.62 x 10-2 M, the dissolution of PbCl2 is not favored, leading to a shift of the equilibrium to the left, resulting in precipitation and a decrease in solubility due to the increased chloride ion concentration.