lec25 - 1 Last Time • Measurement of Ka • pH Indicators...

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Unformatted text preview: 1 Last Time • Measurement of Ka • pH Indicators • Buffers – Henderson–Hasselbach 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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lec25 - 1 Last Time • Measurement of Ka • pH Indicators...

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