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by: Dana Hawkins

Chapter14LeChatelier.pdf CHEM 135

Marketplace > Kansas > Chemistry > CHEM 135 > Chapter14LeChatelier pdf
Dana Hawkins
GPA 2.9
General Chemistry II
Sheelu Panikkatu

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Chapter 14 Le Chatelier Chapter 15 Acids and Bases Chapter 16 Aqueous Ionic Equilibrium
General Chemistry II
Sheelu Panikkatu
Study Guide
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This 5 page Study Guide was uploaded by Dana Hawkins on Tuesday March 31, 2015. The Study Guide belongs to CHEM 135 at Kansas taught by Sheelu Panikkatu in Spring2015. Since its upload, it has received 133 views. For similar materials see General Chemistry II in Chemistry at Kansas.


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Date Created: 03/31/15
Chapter 14 Le Chatelier39s Principal When a chemical system at equilibrium is disturbed the equilibrium shifts in the direction which minimizes the disturbance How does this effect concentration t effects equilibrium by either pushing it make more product or more reactant N204 yields 2N02 It39ll shift to the right to make more reactant To remove reactants it39ll shift to the left 0 How does temperature effect equilibrium o In Endothermic rxn Heat is required to reactants When heat is removed equilibrium will shift to the left to make more heat When heat is added equilibrium will shift to the right where heat will be consumed o In a Exothermic rxn Heat is on the product side When heat is removed equilibrium will shift the right where more can be produced When heat is added equilibrium will shift the left to be consumed How does Pressure effect equilibrium 0 Pressure and volume are inversely related As pressure increases volume decreases As pressure decreases volume increases N23H2 0 When pressure increases equilibrium will shift to the side with fewer mos 0 When pressure decreases equilibrium will shift to the side more mos Chapter 15 Acids and Bases Equations to consider HZ Z Z H30jv logi pHZ logi pOHz log OH pHp0H14 PKaZ logika D same for pkb HZ a H30jvg percent ionization Z Acids and Bases 0 Acid Arrhenius de nition a substance that H ions in an aq equation 0 Acid BronstedLowry de nition the proton H donor 0 Base Arrhenius de nition a substance that produces OH ions in an aq solution 0 Base BronstedLowry de nition is the proton acceptor What is a conjugate acidbase o Conjugate acid is a base where the proton H has been added 0 Conjugate base is an acid where the proton H has been removed I i i Horaq H250 gt IIaq H301an acid base Conjugate Conjugate base acid i l i NH3aq HZOU lt2 N H4aq OHaq base acid Conjugate Con ugate acid base Liat39 Hf strong acids Lis39l39 of s39j39r39rng hinges ilyti1tznishlul39ii acid HUI Lithium 1 Wd11i3f1393 Lii Hl liyLlj IMJIliinic acid NET Sodium hydroxide Haq li Hiy y j di amid Hi I ljotassium l1yt l139mritle IiLiI I aul urc acid HEEUJ j Strontium i39f 1quotIitflc Small1 nitric acid 1WD I Calcium 11 3rtlrrcartirle CMUH pem m c acid HCECIJ Barium hydroxide Haf l l h Characteristics of a strong and weak acid or base 0 Strong acidweak base Completely disassociates in water Weak bond strength Large amount of ions left after disassociation Contains more oxygen atoms More acidic or the more products formed 0 Weak acid strong base Partially disassociates in water Depicted by the equilibrium arrows Strong bond strength Small number of ions left pH of a weak acid can be determined through the ICE Table AcidBase properties of salts and ions 0 Anion Acids If an anion is a conjugate base of a weak acid it39s a weak base If an anion is a conjugate base of a strong acid it39s a strong base with a neutral pH Always H o Cations bases If a cation is a conjugate acid of a weak base it39s a weak acid If a cation is a conjugate acid of a strong base it s a strong acid with a neutral pH Always Acids with more than one ionizable H polyprotic Polyorotio acids Acids with more than one ionizable proton H3803 Ego H803 H o Kai 16 r 102 H80 Ego e 305 Hgo Ea 64L w JiU E Kill 1 Kn Stepwise function like above Ka1gtKa2 because the negative charge on the reactant side in the second step means an electron has been added and is going to stay Chapter 16 Aqueous ionic equilibrium 2 Ka Kb Kw 10 x 103914 pH PKa10gi ACidi HH equation for buffers pH logiKai10giACidi Henderson Hasselbach equation Calculating pH change in a buffer solution 0 A buffer solution resists change in pH when small amounts of an acid or base is added 0 Because buffers contain an excess of weak acidsbases and salt of conjugates the added acid is neutralized by the base Same for added bases 0 Buffer capacity is when the max amount of a strong acid or base that can be added before a signi cant pH change occurs 0 The more disassociated acids the higher the pH Acid ease titrations rrortoo in tho Slow addition of ono oointion of a known oonoontrn tion onliod n titrnnt to n known trolnlno of another oolntion of nn tnown tf i i until tltuo roootion ronoilroo nontrrrlinntion Typoo of ti trntiono Enninnlonoo noint Strong noiti l Strong hnoo pH 7 Wonk noirl Strong hooo pH 1 4 7 Strong onitl Wonk boon pH r 7 Polyprotio noicl Strong rinse Mtiltipilzo oquivnlonoo points


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