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CHM Exam 3 Study Guide

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by: Joseph Notetaker

CHM Exam 3 Study Guide 46657 - CHM 170 - 002

Joseph Notetaker

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About this Document

This is a brief overview of the material on the exam
General Chemistry 2
Mark M Richter
Study Guide
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"Killer notes! I'm stoked I can finally just pay attention in class!!!"
Jeffrey Roob

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This 3 page Study Guide was uploaded by Joseph Notetaker on Saturday March 12, 2016. The Study Guide belongs to 46657 - CHM 170 - 002 at Missouri State University taught by Mark M Richter in Spring 2016. Since its upload, it has received 96 views.


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Date Created: 03/12/16
CHM 170-002 Exam 3 Cheat Sheet +¿ ¿ H O3 ¿ + ­ [H 3 ]>[OH] then solution is acidic ¿ pH=−log¿ −¿ OH ¿ ¿ [H3O ]<[OH] ­ ¿ pOH=−log¿ then solution is basic pH+pOH=14 + ­ [H 3 ]=[OH] then solution is neutral pKa=−log? [Ka] Strong Acid: +¿ H O ¿ 3 ¿ −¿ HCl+H O2­­­­H O 3Cl        Ka= ¿     Ka is very large in this case Cl ¿ ¿ ¿ [H 3 ] = [Cl] = [HCl] in the case of strong acids due to complete ionization Weak Acid: +¿ ¿ H 3 ¿ −¿ HC 2 O3+2 O+2­­­H O +C3H O  2  3a2 ¿      Ka=1.8*10 ­5 C 2 O3 2 ¿ ¿ ¿ HA represents a weak acid + [H 3 ] ≠ [HA] in the case of weak acids due to incomplete ionization Assuming [H O3] represents a small number then:  +¿ ¿ H 3   ¿ ¿ with HA iepresenting the initial concentration  Check this value with the equation O +¿ H 3 ∗100 HA ¿ + If the answer exceeds 5% then [H 3 ] is not small If [H3O ] is large then: −¿ +¿ ¿ A¿ H 3 ¿ ¿                    or              ¿      ¿ pH=pKa+log¿ Use according to personal preference Solubility: Solubility Product (Ksp) 2+ ­ In the equation              2PbCl ­­­­­­­Pb +2Cl Ksp = [Pb ][Cl]­ 2 Ksp ≠ Molar solubility Molar solubility= n+m Ksp √n ∗m m   with n and m representing products Complex Ion formation In the equation Fe +6CN­­­­­­­­­­­Fe(CN) 6 4−¿ ¿ CN¿ 6 ¿ 2+¿ ¿ Fe ¿ 6 C N −¿¿ ¿ Fe¿ ¿ Kf =¿ Some other things to remember: BAD: Bronsted Acid Donates (+) LAA: Lewis Acid accepts (­) Use an ICE table to find stoichiometric coefficients  Strong acids and bases ionize completely  Weak acids and bases ionize incompletely The stronger the acid the weaker the conjugate base and vice versa Strong bonds lead to weak acids + Polyprotic acids (acids with more than one H ) require multiple calculations Buffers contain an acid and a conjugate base Acidity increases as you go left to right and top to bottom on the periodic table Good Luck!


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