A resistor and a 295-mH inductor are connected in series

GEN CHEM II EXAM 2 – STUDY GUIDE Chapter 15 – Chemical Equilibrium  Equilibrium  Reaction proceeds simultaneously in both directions (dynamic equilibrium).  Forward rate = Reverse rate  Denoted by a double arrow  Equilibrium Constant in terms of concentration in M (K ): HCl H + Cl - + − c  = [ ][ ] [] [ ][ ]  = [] For all non-equilibrium concentrations.  If Q > K, shift to left  If Q < K, shift to right  If Q = K, equilibrium  If K ic a big number  more products If K is a small number  more reactants c  General: aA bB  = [] , coefficients are exponents in equilibrium constant [] expression.  K oc reverse = 1/K ofcforward.  Equilibrium concentrations of liquid and solid reactants or products is considered to be 1.  Equilibrium Constant in terms of pressure (K p  K =pK (RTc delta n o, delta n of gas = final (products) gas moles – initial (reactants) gas moles.  Used for reactions in gas phase (can also use K )c  All others rules same as that of K . c  Calculating K c ex. H2(g) + I2(g) 2HI(g), [H2] initial = 0.100 M [2 ] = 0.100 M [2 ] eq = 0.0200 M  RICE Table: Reaction H2 I2 2HI Initial 0.100 0.100 0 Change -x -x 2x Equilibrium 0.100+x 0.100-x = 0.0200 2x 0.100-x = 0.0200  x = 0.08, 2x = 0.16 []2 (0.16) 2 = = = 64 2 ]2 (0.0200)(0.0200)  RICE table can also be used to calculate concentration, given K c  Can also be used for K ppressure). Chapter 16 – Acids, Bases and Salts  Bronsted Acids and Bases  Acid/base reaction – proton transfer.  Acid – proton donor.  Base – proton acceptor.  Conjugate base – what remains of the acid after it donates a proton.  Conjugate acid – species formed when the base accepts a proton.  Properties of water  Amphoteric – can act as either an acid or base.  Auto ionization – water can ionize by itself. -14 o + -  K (won product constant for water) = 1.0 x 10 at 25 C, K w [H ][OH ]  The pH scale + + -  pH = -log[H ] or –log[H ], pOH = -log[OH ]  pH < 7, acidic; pH = 7, neutral (water); pH > 7, basic  pH + pOH = pK = 14w  Strong Acids and Bases  Ionize or disassociate 100%  More ionization = stronger acid/base  Oxoacids: has atleast one oxygen, hydrogen, and a central nonmetal X  Same number of oxygen, different X  Electronegativity inc.  strength of acid inc.  Carboxylic acid (contains R group)  Electronegativity of R inc.  strength of acid inc.  Same X, different number of oxygen  Number of O inc.  electronegativity inc.  strength inc.  Different X, different number of oxygen  Stronger acid  weaker the conjugate base  Binary Acid: one H and one nonmetal  Nonmetal X  Left to right across periodic table  stronger acid  Top to bottom down periodic table  stronger acid  Weak acids: ionize only to a certain extent  Depends on concentration of acid and equilibrium constant for ionization (K ). a + -  HA(aq) + H O(l2 H 3 (aq) + A (aq) +][ ]  []  Larger K astronger acid  pK a -logK a  Weak bases: similar treatment as for weak acids - +  K hbs [OH ] instead of [H ]  Conjugate Acid-Base pairs  K Ka= b w  pK + aK = pKb= 14 aw 25 C o  As K geta larger, K getb smaller – stronger the acid, weaker the conjugate base! AND VICE-VERSA  Calculating K andaK usingbRICE table: make approximation (x = 0) only if [HA]initial/K =agreater than 1000  Diprotic and Polyprotic Acids + + +  K >>a1 [H ]a2 total [H ] 1st+ [H ] 2nd [H ] 1st> [H ]+ 2nd [H ] total [H ]1st  Acid- Base Properties of Salts: salts dissociate into cations and anions in solution  Cations +  Conjugate acid of weak base  weak acid, ex. NH 4 Hydrated metals act like weak acids Group IA and IIA metals except Be – non acids(charge density too low) Charge inc.  metal size dec.  acidity inc.  Anions  Conjugate bases of weak acids  weak bases  If both anion and cation are acids/bases  pH depends on relative strength of conjugate acid and base  When K > b , tha solution is basic  When K < b , tha solution is acidic  When K = b , tha solution is neutral  Acid-base properties of oxides  Alkali metal oxides and alkali earth metal oxides (except BeO) are basic.  Nonmetal oxides tend to be acidic  Be(OH) , Al2OH) , Sn(3H) , Pb(OH2 , Cr(OH)2, Cu(OH) ,3Zn(OH) , a2d Cd(OH) ,2are 2 amphoteric and insoluble in water.  React with acids and bases  Lewis Acids and Bases  Lewis base: electron pair donor  Must contain one or more lone pairs of e -  Lewis acid: electron pair acceptor  Contains incomplete valence shell or multiple bonds that can shift to make room for lone pair.  Lewis acid-base reaction: transfer of electron pair (formation of coordinate covalent bond)  Lewis concepts include all Arrhenius and Bronsted acids/bases