Chem Ii Study Guide

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Multiple Choice: (42 points)

Chapter 15: Principles of Chemical Equilibrium

dynamic equilibriumequilibrium constantreversibility
LeChâtelier’s PrincipleICE tableQ and Keq
major speciesminor species
Keq,f vs Keq,rrate constant vs. equilibrium expressions
significance of magnitude of Keqequilibrium shift with concentration changes
equilibrium shift with temperature changesequilibrium shift with volume changes

Chapter 16: Acid-Base Euilibrium

Brønsted-Lowry acidBrønsted-Lowry baseamphoteric
water equilibrium constantpHpOHpH scale
weak acidKa and pKaweak baseKb and pKb
oxyacidscarboxylic acidspolyprotic acids
aminesconjugate acidconjugate base
pH of acidic salt solutionspH of basic salt solutionsrelate Ka and Kb
acid strength (binary acids)acid strength (oxyacids)Lewis acidLewis base

Chapter 17: Additional Aspects of Aqueous Equilibria

common ion effect effect of buffercomposition of buffer preparation of buffersHenderson-Hasselbach equationbuffer capacity
buffer rangeSA/SB titration curveWA/SB titration curve
equivalence pointpH at equivalence ptbuffer region
pH at midpointsolubility product constantinsoluble Ksp slightly soluble Kspsoluble Ksp
Short problems: (about 45 points)
1.Calculate [H3O+] and [OH-] for a KOH solution with pH = 9.36.


[H3O+] =[OH-] =

2.A container initially has 0.500 atm NO2. At equilibrium, the NO2 pressure is 0.186 atm. Calculate the value of Kp.


Kp =

3.Determine the Ka or Kb for each of the following...
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