Question

5. Which of the following would decrease the K for PbCl2? 2. Lower the pH of the solution b. Add a solution of Pb(NO3)2 c. Add a solution of KCI d. Both band e. None of the above the Ky of a compound is constant at constant tempera mperature, 6. In which of the following aqueous solutions would you expect AgBr to have the HIGHES solubility? a. 0.10 M LIBE b. 0.10 M AgNO3 c. 0.20 M NaBr d. 0.15 M KB e. pure water _ is NOT affected by the pH of the solution. 7. The molar solubility of a. Ca3(PO4)2 b. CaF2 C. Ca(NO3)2 d. Ca(CN)2 e. Cas 8. In which aqueous system is Pbl, LEAST soluble? a. H2O b. 0.5 MHI C. 0.2 MHI d. 1.0 M HNO3 e. 0.8 MKI required to start 9. If a solution is 0.10 M NaCl, what is the minimum concentration of Pb precipitation? For PbCl2, Ksp = 1.7 x 10 a. 6.0 x 10 b. 1.7 x 10 C. 1.7 x 10 d. 3.0 x 10 e. 1.7 x 10

Answer 1

5. Option D, due to common ion effect of pb+2 and Cl- ions solubility decreases.

6. Option E, pure water. Due to common ion effect , solubility is less in remaining solutions.

7. Option C, since it doesn't form buffer solution since it is formed by strong acid and strong base.

8. Option E, due to common ion effect of iodide in more concentration.