Write the ionic equation for dissolution and the solubility product (Ksp) expression for each of the following slightly soluble ionic compounds: (a) PbCl2 (b) Ag2S (c) Sr3(PO4)2 (d) SrSO4

8.Write the ionic equation for dissolution and the solubility product (Ksp) expression for each of the following slightly soluble ionic compounds: (a) PbCl2 (b) Ag2S (c) Sr3(PO4)2 (d) SrSO4

14.Assuming that no equilibria other than dissolution are involved, calculate the molar solubility of each of the following from its solubility product:
(a) Ag2SO4
(b) PbBr2
(c) AgI
(d) CaC2O4∙H2O
28. The following concentrations are found in mixtures of ions in equilibrium with slightly soluble solids. From the concentrations given, calculate Ksp for each of the slightly soluble solids indicated:
(a) AgBr: [Ag+] = 5.7 × 10–7 M, [Br–] = 5.7 × 10–7 M
(b) CaCO3: [Ca2+] = 5.3 × 10–3 M, [CO3 2−] = 9.0 × 10–7 M
(c) PbF2: [Pb2+] = 2.1 × 10–3 M, [F–] = 4.2 × 10–3 M
(d) Ag2CrO4: [Ag+] = 5.3 × 10–5 M, 3.2 × 10–3 M
(e) InF3: [In3+] = 2.3 × 10–3 M, [F–] = 7.0 × 10–3 M

54. Calculate the molar solubility of AgBr in 0.035 M NaBr (Ksp = 5 × 10–13).
CHAPTER 16
4.A helium-filled balloon spontaneously deflates overnight as He atoms diffuse through the wall of the balloon. Describe the redistribution of matter and/or energy that accompanies this process.

12.Arrange the following sets of systems in order of increasing entropy. Assume one mole of each substance and the same temperature for each member of a set.
(a) H2(g), HBrO4(g), HBr(g)
(b) H2O(l), H2O(g), H2O(s)
(c) He(g), Cl2(g), P4(g)

16.Predict the sign of the entropy change for the following processes.
(a) An ice cube is warmed to near its melting point.
(b) Exhaled breath forms fog on a cold morning.
(c) Snow melts

16.Predict the sign of the entropy change for the following processes.
(a) An ice cube is warmed to near its melting point.
(b) Exhaled breath forms fog on a cold morning.
(c) Snow melts

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