ln9s09 - Lecture 9: Getting Quantitative About Solubility...

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Lecture 9: Getting Quantitative About Solubility Our first lecture on “simple” equilibria concerns what happens when you throw a salt that can dissociate into water and try to assign some numbers to the concentration of material that dissolves. We will be using concepts from Lectures 5 and 6 in which the R ICE expression was introduced. We will also see be introduced to strategies for simplifying the equilibrium problem -- making approximations that reduce cubics and quartics to quadratics and first order expressions that permit simple r calculation s. Also, athough we will spend just a single lecture on solubility calculations, it will be instructive to relate what you learn here to the month-long introduction to acid/base equilibria that will follow--it will really help reinforce your general understanding of dissociation equilibria if you can see the parallels between solubility equilibria and acid-base equilibria. Throwing salts in water— the qualitative background developed in high school chemistry and in CH301 . You may not know it, bu have been introduced to two qualitative strategies for explaining solubility: 1. The solubility rules. These include facts such as: CO 3 2- , S 2- , OH - , PO 4 -3 don’t dissolve K + , Na + , NO 3 - , NH 4 + do dissolve So lubility rules predict the chemistry we see in the laboratory , like the classic reaction to yield lead chromate, a yellow precipitate.
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2. Concepts from p hysical e quilibria in Lecture 3 : the physical reasons for why things dissolve multiply charged salts have a high heat of hydration and therefore are less soluble in water “like dissolves like” because of intermolecular force arguments so polar dissolves polar, non-polar dissolves non-polar For example, le t’s look at “Like dissolves like” again and predict
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This note was uploaded on 04/07/2009 for the course CH 302 taught by Professor Holcombe during the Spring '07 term at University of Texas at Austin.

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ln9s09 - Lecture 9: Getting Quantitative About Solubility...

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