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2014 Acid Base Equilibrium Chemistry Acid Base Equilibrium Advanced Placement 2014 2 Ar Kr 10 18 36 54 86 Xe He Ne Rn (222) 83.80 4.0026 20.179 39.948 131.29 I 9 F Cl At Br 17 35 53 85 Lr 71 Lu 103 (210) 19.00 79.90 (260) 35.453 126.91 174.97 8 S O Te 16 34 52 84 Se Po 70 Yb No 102 (209) 16.00 32.06 78.96 (259) 127.60 173.04 7 P N Bi 15 33 51 83 As Sb 69 Md Tm 101 74.92 (258) 14.007 30.974 121.75 208.98 168.93 6 C Si 8.71 14 32 50 82 Sn Pb Er Ge 68 Fm 100 28.09 72.59 207.2 (257) 12.011 11 167.26 11 §Not yet named 5 B Tl In Al 4.82 13 31 49 81 67 99 Es Ga Ho (252) 26.98 69.72 10.8 11 204.38 164.93 2 § 30 48 80 Zn Cd Hg Cf 66 98 Dy 11 (277) 65.39 (251) 112.41 200.59 162.50 § 29 47 79 Ag Au Cu 65 97 Tb Bk 111 (272) 63.55 (247) 107.87 196.97 158.93 0 § Ni Pt 28 46 78 Pd 64 96 Gd 11 Cm (269) (247) 58.69 106.42 195.08 157.25 Ir 27 45 77 Mt Co Rh 63 95 Eu 109 Am ble of the Elements (266) 58.93 192.2 (243) 102.91 151.97 Ta 26 44 76 Fe Hs Ru Os 62 94 Pu 108 Sm (265) 55.85 101.1 190.2 (244) 150.4 Tc 25 43 75 61 93 Bh Re Np Mn Pm 107 (98) Periodic (262) (145) 54.938 186.21 237.05 U W Cr 24 42 74 Sg 60 92 Mo Nd 106 (263) 52.00 93.94 183.85 144.24 238.03 V Pr Ta 23 41 73 59 91 Pa Nb Db 105 (262) 50.94 92.91 180.95 140.91 231.04 Ti Zr Hf Rf 22 40 72 58 90 Th Ce 104 (261) 47.90 91.22 178.49 140.12 232.04 Y 21 39 57 89 La Sc Ac * † 44.96 88.91 138.91 227.03 4 Sr 12 20 38 56 88 Be Ba Ca Ra Mg 9.012 24.30 40.08 87.62 137.33 226.02 †Actinide Series: 1 3 K H Li Fr 11 19 37 55 87 *Lanthanide Series: Cs Na Rb (223) 6.941 22.99 39.10 85.47 1.0079 132.91 ADVANCEDADVANCED PLACEMENTPLACEMENT CHEMISTRYCHEMISTRY EQUATIONSEQUATIONS ANDAND CONSTANTSCONSTANTS ThroughoutThroughout thethe testtest thethe followingfollowing symbolssymbols havehave ththee definitionsdefinitions specifiedspecified unlessunless otherwiseotherwise noted.noted. L,L, mLmL == liter(s),liter(s), milliliter(s)milliliter(s) mmmm HgHg == millimetersmillimeters ofof mercurymercury gg == gram(s)gram(s) J,J, kJkJ == joule(s),joule(s), kilojoule(s)kilojoule(s) nmnm == nanometer(s)nanometer(s) VV == volt(s)volt(s) atmatm == atmosphere(s)atmosphere(s) molmol == mole(s)mole(s) ATOMICATOMIC STRUCTURESTRUCTURE EE == energyenergy EE == hhνν νν == frequencyfrequency cc == λνλν λλ == wavelengthwavelength Planck’sPlanck’s constant,constant, hh == 6.6266.626 × × 1010−−3434 JJ s s SpeedSpeed ofof light,light, cc == 2.9982.998 ×× 101088 msms−−11 Avogadro’sAvogadro’s nnumberumber == 6.0226.022 ×× 10102323 molmol−−11 ElectronElectron charge,charge, e e == −−1.1.602602 ××1010−−1919 coulombcoulomb EQUILIBRIUMEQUILIBRIUM [C][C]cdcd [D] [D] KKcc == ,, wherewhere aa AA ++ bb BB RR cc CC ++ dd DD EquilibriumEquilibrium Constants Constants [A][A]abab [B] [B] cdcd KKcc (molar(molar concentrations)concentrations) ((PPPPCC )( )(DD ) ) KKpp == abab KKpp (gas(gas pressures)pressures) ((PPPPABAB )( )( ) ) KKaa (weak(weak acid)acid) [H[H+-+- ][A ][A ] ] KK == K (weak base) aa [HA][HA] Kbb (weak base) KK (water)(water) [OH-+-+ ][HB ] ww KK == [OH ][HB ] bb [B][B] ++ −− −−1414 KKww == [H[H ][OH][OH ]] == 1.01.0 ××1010 atat 2525°°CC == KKaa ×× KKbb pHpH == −−loglog[H[H++]] , , pOHpOH == −−log[OHlog[OH−−]] 1414 == pHpH ++ pOHpOH -- pHpH == ppKK ++ loglog[A[A ] ] aa [HA][HA] ppKKaa == −−loglogKKaa,, ppKKbb == −−loglogKKbb KINETICSKINETICS ln[A]ln[A] −− ln[A]ln[A] == −−ktkt tt 00 kk == raterate constantconstant 1111 tt == timetime -- == ktkt AAAA [][]tt [][]00 tt½½ == half-lifehalf-life tt == 0.6930.693 ½½ kk GASES, LIQUIDS, AND SOLUTIONS P = pressure V = volume PV = nRT T = temperature moles A n = number of moles PA = Ptotal × XA, where XA = total moles m = mass M = molar mass Ptotal = PA + PB + PC + . D = density n = m KE = kinetic energy M Ã = velocity K = °C + 273 A = absorbance a = molarabsorptivity m D = b = path length V c = concentration KE per molecule = 1 mv2 2 Gas constant, R = 8.314 J mol--11 K Molarity, M = moles of solute per liter of solution --11 = 0.08206 L atm mol K --11 A = abc = 62.36 L torr mol K 1atm= 760 mm Hg = 760 torr STP= 0.00D C and 1.000 atm THERMOCHEMISTRY/ ELECTROCHEMISTRY q = heat m = mass q= mcD T c = specific heat capacity T temperature DSSDD= ÂÂ products- S D reactants = SD = standard entropy DD D DDHH= ÂÂproducts- D Hf reactants f HD = standard enthalpy DD D GD standard free energy DDGG= ÂÂf products- D Gf reactants = n = number of moles D DDGD = HDD - TS D E = standard reduction potential I = current (amperes) = -RTln K q = charge (coulombs) t = time (seconds) = -nFED q Faraday’s constant , F = 96,485 coulombs per mole I ϭ t of electrons 1 joule 1volt = 1coulomb ACID – BASE EQUILIBRIUM Ka, Kb, and Salt Hydrolysis What I Absolutely Have to Know to Survive the AP Exam The following might indicate the question deals with acid – base equilibrium: + − pH, pOH, [H3O ], [OH ], strong and weak, salt hydrolysis, solubility product, Ka, Kb, acid or base dissociation constant, percent ionized, Bronsted-Lowry, Arrhenius, hydronium ion, etc… Acids and Bases: By Definition! Arrhenius • Acids: Hydrogen ion, H+, donors • Bases: Hydroxide ion, OH− donors HCl → H+ + Cl− NaOH → Na+ + OH− Bronsted-Lowry • Acids: proton donors (lose H+) Bases: proton acceptors (gain H+) • + − HNO3 + H2O → H3O + NO3 + − NH3 + H2O ⇌ NH4 + OH Hydrogen Ion, Hydronium Ion, Which is it!!!? Hydronium − H+ riding piggy-back on a water molecule; water is polar and the + charge of the naked proton is greatly attracted to “Mickey's chin” (i.e. the oxygen atom) + • H3O “Anthony” • H+ “Tony” + • Often used interchangeably in problems; if H3O is used be sure water is in the equation! Bronsted−Lowry and Conjugate Acids and Bases: What a Pair! Acid and conjugate base pairs differ by the presence of one H+ ion. + − HC2H3O2 + H2O → H3O + C2H3O2 − + • HC2H3O2 is the acid; thus C2H3O2 is its conjugate base (what remains after the H has been donated to the H2O molecule) • H2O behaves as a base in this reaction. The hydronium ion is its conjugate acid (what is formed after the H2O accepts the H+ ion) + − NH3 + H2O → NH4 + OH + + • NH3 is the base; thus NH4 is it’s conjugate acid (what is formed after the NH3 accepts the H ion) + • H2O behaves as an acid in this reaction. The hydroxide ion is its conjugate base (what remains after the H has been donated to NH3) Understanding conjugate acid/base pairs is very important in understanding acid-base chemistry; this concepts allows for the understanding of many complex situations (buffers, titrations, etc…) Important Notes… Amphiprotic/amphoteric--molecules or ions that can behave as EITHER acids or bases; water, some anions of weak acids, etc… fit this bill. Monoprotic − acids donating one H+ Diprotic − acids donating two H+ Polyprotic − acids donating 3+ H+ Regardless, always remember: ACIDS ONLY DONATE ONE PROTON AT A TIME!!! Copyright © 2014 National Math + Science Initiative, Dallas, Texas. All Rights Reserved. Visit us online at www.nms.org Page 1 Acid – Base Equilibrium Ionization: That’s What it’s All About! Relative Strengths A strong acid or base ionizes completely in aqueous solution (100% ionized [or very darn close to it!]) • The equilibrium position lies far, far to the right (favors products)… + − • Since a strong acid/base dissociates into the ions, the concentration of the H3O /OH ion is equal to the original concentration of the acid/base respectively. • They are strong electrolytes. • Do Not confuse concentration (M or mol/L) with strength! • Strong Acids • Hydrohalic acids: HCl, HBr, HI; Nitric: HNO3; Sulfuric: H2SO4; Perchloric: HClO4 • Oxyacids! More oxygen atoms present, the stronger the acid WITHIN that group. The H+ that is “donated” is bonded to an oxygen atom. The oxygen atoms are highly electronegative and are pulling the bonded pair of electrons AWAY from the site where the H+ is bonded, “polarizing it”, which makes it easier [i.e. requires less energy] to remove − thus the stronger the acid! O HO Br < HO Br O < HO Br O • Strong Bases • Group IA and IIA (1 and 2) metal hydroxides; be cautious as the poor solubility of Be(OH)2 and Mg(OH)2 limits the effectiveness of these 2 strong bases. − • IT’S A 2 for 1 SALE with the Group 2 (IIA) ions), i.e. 0.10M Ca(OH)2 is 0.20M OH Where the fun begins… A weak acid or base does not completely ionize (usually < 10%) • They are weak electrolytes. • The equilibrium position lies far to the left (favors reactants)… • [H+] is much less than the acid concentration − thus to calculate this amount and the resulting pH you must return to the world of EQUILIBRIUM Chemistry! • The vast majority of acid/bases are weak. Remember, ionization not concentration!!!! • Acids and Bases ionize one proton (or H+) at a time! + − • For weak acid reactions: HA + H2O → H3O + A [H O+ ][A- ] K = 3 where K is typically much less than 1 a [HA] a + − • For weak base reactions: B + H2O → HB + OH [HB+ ][OH- ] K = where K is typically much less than 1 b [B] b Copyright © 2014 National Math + Science Initiative, Dallas, Texas.
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