Pb `(IO_(3))_(2)`, a sparingly soluble salt in water, has a `K_(sp)` value of `2.6 xx 10^(-13)`. To 35mL of a 0.15 M Pb `(NO_(3))_(2)` solution, 15mL of a 0.8 M `KIO_(3)` solution is added and a precipitate of `Pb(IO_(3))_(2)` formed. Find the concentration of `Pb^(2+) and IO_(3)^(-)` left in the solution.

Explanation

To find the concentrations of \( \text{Pb}^{2+} \) and \( \text{IO}_3^{-} \) left in the solution after the precipitation of \( \text{Pb(IO}_3)_2 \), we will follow these steps:

### Step 1: Calculate the moles of \( \text{Pb}^{2+} \) and \( \text{IO}_3^{-} \) before precipitation.

1. **Calculate moles of \( \text{Pb}^{2+} \):**
\[ \text{Moles of } \text{Pb}^{2+} = \text{Concentration} \times \text{Volume} = 0.15 \, \text{M} \times 0.035 \, \text{L} = 0.00525 \, \text{mol} \]
...