Write the ionic equation for dissolution and the solubility product (Ksp) expression for each of the following slightly soluble ionic compounds:
Ch. 15 (pages 889-894): 8, 14, 28, 54
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1. Â Â Â Â Â Â Â 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
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2. Â Â Â Â Â Â Â 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
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3. Â Â Â Â Â Â Â 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
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4. Calculate the molar solubility of AgBr in 0.035 M NaBr (Ksp = 5 × 10-13)
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