Lecture 19

Lecture 19 - 3/1/10 A solution contains 0.050 M NaCl and...

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1 1 A solution contains 0.050 M NaCl and 0.050 M NaI. Can Cl - and I - be separated as silver salts? If so, at what [Ag + ]? K sp (AgCl) = 1.8 ! 10 -10 and K sp (AgI) = 8.5 ! 10 -17 . Find the [Ag + ] that causes each to precipitate (when Q > K sp ) AgCl : AgI : Q = [Ag + ](0.050M) > K sp Q = [Ag + ](0.050M) > K sp Therefore: 1.7 ! 10 -15 M < [Ag + ] < 3.6 ! 10 -9 M Only AgI precipitates Nothing precipitates Both AgI,AgCl precipitate 2 What is [I - ] when AgCl begins to precipitate? Know [Ag + ] when AgCl begins to precipitate. Therefore [I ! ] = K sp (AgI) [Ag + ] = 8.5 ! 10 " 17 3.6 ! 10 " 9 = 2.4 ! 10 " 8 3 Try textbook problems: 19.74, 19.103 [Solutions available] Also, try: 19.77, 19.104 [Answers posted with Assignment #2] Read textbook Sections 19.4, 23.1 Unit 3: Coordination Chemistry (Chapter 23) 1. Transition Metals (T.M.) - elements in d-block and f-block 4 -know names of first two rows -will not cover metallic state 5 Many transition metal compounds are - highly coloured (absorb visible light) - paramagnetic (unpaired electrons, interact with magnet) January February March April May June July August September October November December What’s your Birth Stone? Garnet
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Lecture 19 - 3/1/10 A solution contains 0.050 M NaCl and...

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