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 0 answersPost by Maimouna Louche on July 21, 2012We didn't see the other type of solution-heterogenous. 3 answersLast reply by: Zachary McCoySun Jan 5, 2014 6:18 PMPost by priyanka thapa on October 13, 2011am i mistaken, isnt the molarity of solution at the example solution concentration suppose to be 2.22 M ? 0 answersPost by Zak Roeser on December 14, 2010Correct me if I am wrong, but I believe on the "Dilution of Solutions" portion of the lecture the answer should be 8.00mL of water due to sig. figs. in the problem.

### Solutions, Henry's Law, Concentration Equations

• Solutions: every phase in every other; solutions in liquids most important

• Saturation solubility: no more solute will dissolve in solvent; an equilibrium phenomenon

• Henry’s Law for gases in liquids: s = KP; effects shown in carbonated liquids; divers and the “bends”

• Concentration expressions: % by mass; molarity = mol. solute/L soln.; molality = mol. solute/ kg solvent

• Do examples of interconverting solubility expressions for particular solutions

• Dilution MV = const

• Temperature effects: gases, always lower S as T increases; solids varying effects

• Entropy means mixed-upness, chaos; temperature effects on S can be explained by enthalpy and entropy effects

### Solutions, Henry's Law, Concentration Equations

Lecture Slides are screen-captured images of important points in the lecture. Students can download and print out these lecture slide images to do practice problems as well as take notes while watching the lecture.