chem notes 2
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| Amphoteric | can act as an acid or a base; H2O
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| If we want the conjugate Base, then | H2O acting as an acid (proton donor); H20--> H+ + OH- (CB)
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| If we want the conjugate Acid, then | H2O is acting as a base( proton acceptor) H20--> H3O+ (CA)
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| Strong ACIDS::: 7 of them | HCl; HBr; HI; H2SO4; HNO3; HCLO4; HCLO3
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| Strong BASES:: 8 of them | LiOH; NAOH; KOH; RbOH; CsOH; ---> Group 1 & then Ca(OH)2; Sr(OH)2; Ba(OH)2 ----> Group 2
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| Ba(OH)2 | Barium Hydroxide
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| Oxyacidic Trend: | More OXYGEN= more Acidic for Oxyacid i.e. HCLO<HCLO2
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| Oxyacidic Trend: | More ELECTRONEGATIVE the element= more Acidic ( stronger) ....NOT including H or O......I.e. HCLO3 > HBrO3
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| More acidic | more stable; larger; weaker conjugate base
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| Kw of water= | 1X 10 ^-14
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| Kw= | [H+] [OH-]
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| Ka*Kb= | Kw
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| pH= | -log[H+]
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| pOH= | -log[OH-]
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| [H+]*[OH-]= | 1X 10^-14
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| pH+ pOH= | 14
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| H+= | 10^-pH
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| OH- = | 10^-pH
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| As -OH goes up (inc)....pOH goes ______? | DOWN (Dec)
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| 1M HCL will have a pH of ?? | 0
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| 10 M HCL will have a pH of ??? and a pOH of ?? | pH= -1 and pOh= 15
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| weak acid _____ dissociated; Strong acid _____ dissociates | weak acid= partially dissociates; strong acids= fully dissociates
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| Shortcut to find weak acid pH:: when Ka is given | [H3O+] = sqrt Ka*HA
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| Shortcut to find weak base pOH:: when Kb is given | [OH-] = sqrt Kb*A-
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| Moles and pH are ______ proportional | inversely
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| Dissociation of a weak base | A- + H20= OH- + HA
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| Dissociation of a weak acid | HA+ H20= H30 + A-
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| HF + CL- ---> HCL + F- | HF= weak acid; CL- = weak conjugate base; HCL= strong acid; F- = strong conjugate base
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| Equilibrium favors the ______ side in a dissociation rxn ??? | weaker side (side with weaker acid/ or base)
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| INCREASE Ka= _____ pKa? | DECREASE ----> stronger acid
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| INCREASE Kb= ______ pKb? | DECREASE ----> stronger base
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| Cations (+)- neutral salt...8 conjugate acids | conjugate acid of strong bases....Li+, K+, Na+, Rb+, Cs+, Ca 2+, Sr 2+, Ba 2+
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| Anion (-) - neutral salt......7 conjugate bases | conjugate base of strong acid.....Cl-, Br-, I-, NO3-, CLO4-, CLO3-, HSO4-
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| Anions | usually BASES w/ exception to the 7 conjugate bases of the strong acids
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| Cations | usually ACIDS w/ exception to the 8 neutral conjugate acids of the strong bases
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| More positively charged= the better the _____ | acid ( cation)
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| To find out if a salt is acid or base...i.e. CsF | Cs is a neutral cation ( so its crossed out), and the F has a charge of -1 on table...so its basic ( anion)
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| NaNO3 ( Sodium Nitrate) has a pH of?? | pH= close to 7 because both Na and NO3- are neutral species.
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| Resists change in pH | buffer
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| Buffer is a combination of.... | weak acid and its conjugate base.......OR.......weak base and its conjugate acid; BOTH needed in equal amounts
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| Buffer can be _____ or ____ away from pH value... | +1, -1
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| Acid/ base pH is scaled based on powers of _____ | 10; i.e. pH of 2 is 1000 more acidic than pH of 5
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| For a Buffer pH equation use :: | Henderson Hasselbach ::: pH= pKa+ log (A-)/ (HA)
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| 10x more acid than base = | drop one unit from pKa value
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| 100x more acid than base = | drop 2 unit from pKa value
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| 10x more base than acid= | RAISE 1 unit from pKa value
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| 100x more base than acid= | RAISE 2 unit from pKa value
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| First Law of Thermodynamics | Energy can NOT be created nor destroyed
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| Second Law of Thermodynamics | For a spontaneous process, ΔS universe> 0; ΔS system + Δ S surroundings > 0
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| Third Law of Thermodynamics | A perfect crystal at 0 K has ZERO entropy
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| Change in work energy | ΔE= q + w ; q= change in heat energy & w= change in work energy
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| System looses heat if q= | negative (-)
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| System absorbes heat if q= | positive (+)
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| System does work if w= | negative (-)
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| System has work done on it if w= | positive (+)
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| Gas expands then w= | negative (-)
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| Gas compressed then w= | positive (+)
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| w= | - PΔV
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| locked piston = | constant volume
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| As heat (Temp) increases, then ... | Pressure increase (P and T are directly related)
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| Cool= | expanding gas
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| Heat | compressing gas
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| Isobaric | constant pressure; ΔP= 0
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| Isochoric | ΔV=0 & w= 0...think v0w isochoric
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| Isothermal | constant temp; ΔT= 0, then ΔE=0
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| Adiabatic | NO heat allowed in or out; q=0
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| Altitude Change= State function= | doesnt matter the path taken ( independent) just matters start and finish
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| Everything are State Functions EXCEPT: 2 of them | q and w ; Even though ΔE= state fx
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| Path Dependent | q and w
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| Solids have the _____ Entropy ( disorder) ΔS | Least amount out of a s,l,g
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| Gasses have the ____ Entropy ( disorder) ΔS | MOST amount
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| S--> L---> G ΔS=? | postitive
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| G--->L---->S ΔS=? | negavite
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| More moles of gas= ____ entropy | more
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| in a rxn if we go left to right according to the number of moles of gas ( more moles of gas on right then left) | Δ S= positive
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| If products + reactants have the same # of moles of gas ...then Entropy= | close to 0 or very small
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| Enthalpy ΔH= | q x p
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| ΔH<0 | Exothermic ( release heat)
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| ΔH>0 | Endothermic ( absorb heat)
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| if the soln is cold .... | endothermic rxn occuring
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| if the soln if warm.... | exothermic rxn occuring
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| Bond Enthalpy (D) | Amnt of energy needed to break a bond
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| break bond= | ENDO ( energy needed in system)
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| Make bond= | EXO ( release energy in a system)
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| ΔH= | bonds broken- bonds formed
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| Enthalpies of formation ΔHf= | products- reactants
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| ΔHf for any element in it's standard state = | 0 ... i.e. Cl2
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| ΔHf= forms exactly ____ moles of any product & forms elements in their standard state | 1 M
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| Hess's law: | Change in ΔH is same regardless of path taken
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| Gibb's free energy (ΔG) | Energy that is free to do work
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| ΔG<0 | Spontaneous
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| ΔG>0 | non- spontaneous
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| ΔG= 0 | equilibrium
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| ΔG= | products- reactants
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| ΔG= | ΔH-TΔS ; Get High Test Scores
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| Room temp = | 25 degrees C standard conditions
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| ΔH= - .......ΔS= + | Spontaneous for all temp
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| ΔH= + .......ΔS= - | Non spontaneous for all temp
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| ΔH= - .......ΔS= - | Spontaneous at low temp
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| ΔH= + .......ΔS= + | Spontaneous at High temp
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| Oxidation State Rules...Get their typical oxidation states | #1 Group 1 or 2 Metals ; #2 H+ is +1 except when bonded to a metal; #3 More electronegative elements get their typical oxidation states
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| Permangenate | MnO4-
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| Iodide | I-
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| SOdium Azide | NaN3
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| In Redox Reactions... if #e- is on the product side | oxidation
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| In Redox Reactions... if #e- is on the reactant side | reduction ( think reactant reduction RR)
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| In finding E for the reduction potential rxns... | dont worry about coefficients, just change sign if reverse is needed
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| The standard electrode reduction potential E for H= | 0v
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| shift right= E cell Increases= | spontaneous
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| shift left= E cell dencreasses= | non spontaneous
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| E cell= cell potential or | EMF
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| for E cell shifting... only ____ matter not s or L | aq
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| add more reactant, shift to the | left
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| add more product , shift to the | right
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| add more solid or Liquid, shift to the | NO shift because s and L are not counted
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| Increase pH ( loosing H+ and becomes more basic) , shift to the | the side with more H+ ions
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| Decrease pH ( adding H+ and becomes more acidic), shift to the | the side with less H+ ions
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| Nerst :: | E= E - [.0592/ n] log Q ; where n= number of moles transfered in rxn; and Q= products/ reactant
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| strongest oxidizing agent= gets reduced | most positive v
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| strongest reducing agent = gets oxidized | most negative v ( think RAN....reducing agent negative)
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| In a redox rxn if sum = NEGATIVE ...then rxn is | not spontaneous
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| In a redox rxn if sum = POSITIVE ...then rxn is | spontaneous
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| For Spontaneous rxns;; ΔG=___; Ecell = ____; Q___K | negative; positive; Q<K If one is true then all is true
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| Electrolysis= | Destruction of electricity; consumes electricity; have to have moving ions;
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| molten electrolysis= | melt salt
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| NaBr (liguid)= | molten b/c its a liquid
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| Grams made by electrolysis:: | (AMPS) ( t in seconds) ( mw) / ( n) ( Faraday= 96,000)
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| Reductant= | gets oxidized
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| Oxidant= | gets reduced
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| Galvanic/ Voltaic Cells | Spontaneous
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| Cell potential/ EMF= E>0; ΔG<0 | Galvanic/ Voltaic Cells
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| Produces electricity | Galvanic/ Voltaic Cells
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| RED CAT & AN OX | Galvanic/ Voltaic Cells
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| e- go from ANODE ---> CATHODE | Galvanic/ Voltaic Cells
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| ions float in and out of bridge; keep solns neutral; necessary for battery; | SALT bridge
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| In a salt bridge....anions go to _____ & cations go to _____ | anode; cathode
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| NON- spontaneous/ consumes energy | ELectrolytic cell
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| E<0 ; ΔG>0 for _____ cells | Electrolytic cell
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| In a electrolytic cell, anode is ____ & cathode is ____ | +; -
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| In a electrolytic cell electrons move from | ANODE (-)----> Cathode (+)
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