Chemistry, 01.05.2021 17:40 dancekb2

B. Solubility Equilibrium: Finding a Value for Ksp 1. Volume 0.30 M Pb(NO3)2 = 5.0 mL.
Number of moles Pb2+ = [M x V(stock sln)] = 0.0015 moles
2.
a. Volume 0.30 M HCl used: 5.0 mL
b. Number of moles Cl- added: 0.0015 moles
3. Observations:
a. in hot water: the solid settled on the bottom then completely dissolved
b. in cold water: No change, it stayed dissolved
4. Volume H2O added to dissolve PbCl2: 4.0 mL
a. Total volume of solution: 12.0 mL
b. Explain why PbCl2 did not precipitate immediately on addition of HCl.
c. Explain your observations in step 3 (hot versus cold water).
d. Explain why the PbCl2 dissolved when water was added in Step 5.
e. Given the number of moles of Pb2+ and Cl- in the final solution in Step 4, and the volume of that solution, calculate [Pb2+] and [Cl-] in that solution.
Can anyone help with 4b-e please. My answers from lab are in bold for the 1st part(1-4a).

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B. Solubility Equilibrium: Finding a Value for Ksp 1. Volume 0.30 M Pb(NO3)2 = 5.0 mL.
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