Chapter 16 Lecture 2

Chapter 16 Lecture 2 - Chapter 16 Lecture 2 Another way to...

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Chapter 16 Lecture 2 Another way to look at solubility Precipitation: If the ions of an insoluble compound find each other they will precipitate. You can predict what the ion concentrations have to be for precipitation to occur. What [CrO 4 2─ ] must be present in 0.0015 M AgNO 3 to just cause Ag 2 CrO 4 to precipitate? Ksp = 1.1 X10 ─12
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The Ksp indicates what ion minimum ion concentrations are need for precipitation. The idea of Qip Qip < Ksp no precipitate Qip > Ksp precipitate will form Qip= Ksp when precipitation has finished. Assume 1 L of solution. Add 4.0 X 10 ─7 mol K 2 CrO 4 [CrO 4 2─ ] If [Ag + ] = 0.0015 Find Qip Another shot 4.0 X 10 ─7 mol K 2 CrO 4 [CrO 4 2─ ] 8.0 X 10 ─7 Find Qip Ksp for Ag 2 CrO 4 = 1.1 X 10 ─12
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silver will precipitate out. Will a precipitate from when: 230 mL if 0.0020 M MgCl 2 is mixed with 50.0 mL of 0.0050 M NaF? Ksp MgF
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This note was uploaded on 04/16/2008 for the course CHEM 1123 taught by Professor Paul during the Fall '06 term at Arkansas.

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Chapter 16 Lecture 2 - Chapter 16 Lecture 2 Another way to...

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