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CHEM 112

by: Jessica Lee
Jessica Lee

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About this Document

Chapter 12 & 14
General Chemistry
Dr. Stec
Class Notes
25 ?




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This 3 page Class Notes was uploaded by Jessica Lee on Friday July 22, 2016. The Class Notes belongs to CHEM 112 at University of Illinois at Chicago taught by Dr. Stec in Fall 2015. Since its upload, it has received 9 views. For similar materials see General Chemistry in Chemistry at University of Illinois at Chicago.


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Date Created: 07/22/16
Chapter 12, 14 Lecture Notes Homogeneous Mixtures  A mixture of 2+ substances  Composition vary from 1 sample to another Solutions  Solvent: majority component of solution  Solute: minority component of solution  Solutions form in part of intramolecular forces Solubility:  Soluble: solute dissolves in solvent  Insoluble: 1 substance doesn’t dissolve Solubility & Saturation:  Solubility: defined as amount of compound that dissolves in certain amount of liquid; additional solute added -> not dissolve  Saturated solution: holds max amt of solute under solution conditions  Unsaturated solution: holds less than max amt of solute; additional solute added -> dissolve  Supersaturated solution: Solubility:  Other factors affect ability solute to dissolve o Temp o Pressure o Ratio of amt of solute & solvent  Intermolecular forces o Dispersion o Dipole-dipole o Hydrogen bond o Ion-dipole Mixing & the Entropy of Solution Formation  Entropy: measure of system’s disorder or dispersal of particles throughout a system  Energy: drive to disperse throughout the system  Solution formation may/not lower potential energy Solute Solubility Temperature & Pressure:  Increase in temp -> increase in solubility  Solubility of solids increase as temp increases, or change of H solution is endothermic  Solubility of gases decrease as temp increases, change of H solution is exothermic Solubility of Gases in Water: Pressure Dependence  Henry’s Law: higher pressure, higher the solubility  greater partial pressure of gas -> more soluble gas  Sgas= k H gas  Sgas = concentration  kH= Henry’s law constant Mole Fraction PPM = amt of solute/amt of solution * 10^6 Ptotal P soluteP solvent T FPm T bp= FP solventFPsolution Van’t Hoff Factor (i) = ratio of moles of solute particles to moles of formula units 2 Osmosis = flow of solvent from solution of low concentration into solution of high concentration  = MRT equilibrium shifts away from side w/ added 3


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