lec25 - 3 (aq) [Ag(NH 3 ) 2 ] + K f = Salt solubility...

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1 Announcements Office hours today 11 –12, 159 Chemistry Last Time • Measurement of Ka • pH Indicators • Buffers – Henderson–Hasselbach equation Solubility Product • Characterizes salt equilibria and solubility • Just like heterogeneous equilibrium in gases M n X m (s) nM m+ (aq ) + mX n– (aq) K sp = [M] n [X] m • K sp >> 1, very soluble : K sp << 1, insoluble
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2 Example Calculate the molar solubility S for Fe(OH) 3 given that K sp = 2.0 x 10 –39 . Using K sp M n X m (s) nM m+ (aq ) + mX n– (aq) • Common ion effect – like Le Chatelier • Predict precipitation – compare to Q sp • Qualitative analysis – unknown solutions – selective precipitation – complex formation Complex Formation • Consider AgCl(s): AgCl(s) Ag + (aq) + Cl (aq) Ag + (aq) + 2NH
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Unformatted text preview: 3 (aq) [Ag(NH 3 ) 2 ] + K f = Salt solubility increases due to complex formation [Ag(NH 3 ) 2 ] + [Ag][NH 3 ] 2 3 Ionic Strength Total ionic concentration in solution Affects the apparent charge on a cation or anion changes Ksp and pH of salt solutions from that expected on the basis of concentration tabulated activity coefficients, Replace concentrations with activities [M] [M] M called an activity A M = [M] M Example What is the concentration of F anions in a solution saturated with CaF 2 and containing enough MgSO 4 to make the ionic strength 0.05 M? Ca = 0.485 F = 0.81 K sp = 3.9 x 10 11...
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lec25 - 3 (aq) [Ag(NH 3 ) 2 ] + K f = Salt solubility...

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