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Lecture_Notes_100209b

Lecture_Notes_100209b - Lecture Note

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Solubility Equilibria y A 1.00 L solution saturated at 25 o C with calcium oxalate, CaC 2 O 4 , is evaporated to dryness giving a 0.0061 g residue of CaC 2 O 4 . Calculate the solubility and the solubility product constant for this salt at 25 o C.

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Comparing Solubilities y Need to consider K sp as well as the number of ions being produced.
Which of the following salts is the most soluble in 1.0 L of water? Mg(OH)2; Ksp = 8.9 x... Ba(OH)2; Ksp = 5.0 x ... Co(OH)2; Ksp = 2.5 x... 4% 8% 89% 1. Mg(OH) 2 ; K sp = 8.9 x 10 -12 2. Ba(OH) 2 ; K sp = 5.0 x 10 -3 3. Co(OH) 2 ; K sp = 2.5 x 10 -16

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What is the solubility of Ag 3 PO 4 in 1.0 L of water? K sp = 1.8 x 10 -18 1.8 x 10-18 M 1.3 x 10-9 M 1.6 x 10-5 M 3.7 x 10-5 M 6% 10% 73% 10% 1. 1.8 x 10 -18 M 2. 1.3 x 10 -9 M 3. 1.6 x 10 -5 M 4. 3.7 x 10 -5 M
Common Ion Effect y Calculate the molar solubility of AgBr (K sp = 5.0 x 10 -13 ) in: { Pure Water { 3.0 x 10 -2 M AgNO 3 solution

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pH and Solubility y We can shift certain solubility equilibria if we change the pH of the solution.
Precipitation y Ion product – what we use to predict if a precipitate will form. Defined the same as K sp , but with initial rather then equilibrium concentrations

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