# Will a Precipitate Form? Calculation of Ion Product (Q) using Ksp of PbI₂

What is the ion product (Q) in the given scenario, and will a precipitate form?

The ion product (Q) is calculated using the concentrations of the reactants. Calculating Q and comparing it to the solubility product constant (Ksp) determines whether a precipitate will form. In this case, Q is less than Ksp, so no precipitate will form.

## Understanding Ion Product (Q) and Precipitation

**Precipitation in Chemistry:**Precipitation is the formation of a solid, insoluble substance from a solution due to a chemical reaction.

## Calculation of Ion Product (Q):

The ion product Q is calculated by multiplying the concentrations of the ions involved in the reaction. In this case, we are dealing with the dissociation of Pb(NO₃)₂ and NaI to form Pb²⁺ and I⁻ ions.**Given Concentrations:**- Volume of Pb(NO₃)₂ solution = 150.0 mL, concentration = 0.0050 M - Volume of NaI solution = 350 mL, concentration = 0.0015 M

**Calculating Q:**The concentration of Pb²⁺ is 0.0050 M since its concentration is the same as Pb(NO₃)₂. The concentration of I⁻ can be calculated using the molarity and volume of NaI solution.

**Q = [Pb²⁺] * [I⁻]²**Q = (0.0050 M) * (0.0015 M)² Q = 1.125 x 10⁻⁸

## Determining Precipitation:

To determine if a precipitate will form, we compare Q to the Ksp of PbI₂, which is 3.2 x 10⁻⁸ in this case. If Q is greater than Ksp, a precipitate will form. If Q is less than Ksp, no precipitate will form.**Final Answer:**Based on the calculations, the ion product (Q) is 1.125 x 10⁻⁸, which is less than the Ksp of PbI₂. Therefore, no precipitate will form in this scenario.