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Unformatted text preview: 1 Last Time Measurement of Ka pH Indicators Buffers HendersonHasselbach equation Solubility Product Characterizes salt equilibria and solubility Just like heterogeneous equilibrium from Chapter 13 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 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 3 (aq) [Ag(NH 3 ) 2 ] + K f = Salt solubility increases due to complex formation [Ag(NH 3 ) 2 ] + [Ag][NH 3 ] 2 2 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...
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