Calculate the concentration of IO3– in a 9.23 mM Pb(NO3)2 solution saturated with Pb(IO3)2. The Ksp of Pb(IO3)2 is 2.5 × 10-13. Assume that Pb(IO3)2 is a negligible source of Pb2 compared to Pb(NO3)2.

Pb(NO3)2 => Pb2+ + 2 NO3-

[Pb2+] = [Pb(NO3)2] = 7.77 mM = 7.77 x 10-3 M

Pb(IO3)2 <=> Pb2+ + 2 IO3-
Ksp = [Pb2+][IO3-]2 = 2.5 x 10-13
7.77 x 10-3 x [IO3-]2 = 2.5 x 10-13
[IO3-] = 5.67 x 10-6 M ˜ 5.7 x 10-6 M

I agree with the last answer.

replace the 7.77 with 9.23

answer in end in 5.20 x 10^-6

To calculate the concentration of IO3– in the Pb(NO3)2 solution saturated with Pb(IO3)2, you need to use the concept of solubility product constant (Ksp) and the given information.

1. Write the balanced equation for the dissociation of Pb(IO3)2:
Pb(IO3)2 ↔ Pb2+ + 2IO3–

2. Write the expression for the solubility product constant (Ksp):
Ksp = [Pb2+][IO3–]^2

3. Identify the concentrations to be determined. In this case, you need to find the concentration of IO3–, which is denoted as [IO3–].

4. Use the given information to determine the concentration of Pb2+ in the solution. Since it is stated that Pb(NO3)2 is a negligible source of Pb2 compared to Pb(IO3)2, we can assume that all of the Pb2+ ions come from the dissociation of Pb(IO3)2 and not from Pb(NO3)2. Therefore, the concentration of Pb2+ is equal to the concentration of Pb(IO3)2, which is also the solubility of Pb(IO3)2 in the saturated solution.

5. Substitute the concentration values into the solubility product expression and solve for [IO3–]:
Ksp = [Pb2+][IO3–]^2
[IO3–] = √(Ksp / [Pb2+])

6. Plug in the values from the problem:
Ksp = 2.5 × 10^(-13)
[Pb2+] = 9.23 mM

7. Calculate the concentration of IO3–:
[IO3–] = √(2.5 × 10^(-13) / 9.23 mM)

Note: Make sure to use consistent units for the concentration and Ksp values. If necessary, convert the units to match before performing the calculation.

By following these steps, you can calculate the concentration of IO3– in the given solution.