Chemistry, 07.05.2020 02:00, linnybear300
Enter your answer in the provided box. Lead(II) nitrate is added slowly to a solution that is 0.0400 M in Cl− ions. Calculate the concentration of Pb2+ ions (in mol / L) required to initiate the precipitation of PbCl2.
(Ksp for PbCl2 is 2.40 × 10−4.)
Answers: 3
![[Pb^{2+}] } = 0.15 mol/L](/tpl/images/0651/0478/c6ffa.png)
is 
![K_{sp} = [Pb^{2+}][Cl^{-}]^2](/tpl/images/0651/0478/939e9.png)
![2.4 0 * 10^{-4} = 0.0400^2 * [Pb^{2+}]](/tpl/images/0651/0478/b2e7f.png)
![[Pb^{2+}] } = \frac{2.4 0 * 10^{-4} }{0.0400^2 }](/tpl/images/0651/0478/f08bf.png)
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