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44 Cards in this Set
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1/11 =
1/12 = |
1/11 = 0.091
1/12 = 0.083 |
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1/6 =
1/7 = 1/8 = 1/9 = |
1/6 = 0.166
1/7 = 0.143 1/8 = 0.125 1/9 = 0.111 |
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Solubility Rules (5)
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1) Most +1 cation with -1 anion salts are soluble in water (Except transition metals)
2) Nitrate (NO3-) salts are mostly water-soluble. 3) Sulfate (SO4 2-) salts w +1 cations are mostly water-soluble. 4) Most salts with -2 and -3 anions are insoluble (except sulfate) 5) Most oxide (O2-) and hydroxide (OH-) anions are only slightly water-soluble. (except NaOH and KOH) |
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Acetate
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C2H3O2-
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Bicarbonate
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HCO3-
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Bisulfite (Hydrogen Sulfite)
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HSO3-
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Bisulfate (hydrogen sulfate)
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HSO4-
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Dihydrogen phosphate
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H2PO4-
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Hypochlorite
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ClO-
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Chlorite
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ClO2-
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Chlorate
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ClO3-
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Perchlorate
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ClO4-
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Cyanide
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CN-
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Superoxide
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O2-
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Nitrite
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NO2-
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Nitrate
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NO3-
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Permanganate
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MnO4-
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Carbonate
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CO3 2-
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Chromate
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CrO4 2-
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Dichromate
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Cr2O7 2-
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Hydrogen phosphate
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HPO42-
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Oxalate
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C2O4 2-
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Oxide
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O 2-
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Peroxide
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O2 2-
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Sulfite
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SO3 2-
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Sulfate
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SO4 2-
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phosphate
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PO4 3-
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Ammonium
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NH4+
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Solubility Product
MX (s) <--> M+ (aq) + X- (aq) MX2 (s) <--> M+ (aq) + 2X- (aq) |
MX (s) <--> M+ (aq) + X- (aq)
Ksp = [M+][X-] = (x)(x) MX2 (s) <--> M+ (aq) + 2X- (aq) Ksp = [M+][X-]^2 = (x)(2x)^2 |
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Arrheinius Acid
Bronsted-Lowry Acid Lewis Acid |
Arrheinius Acid : Yields H3O+ when added to H2O
Bronsted-Lowry Acid : Proton donor Lewis Acid : electron pair acceptor |
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Acid strength (up!)
Ka pKa conjugate base strength Kb pKb |
Acid strength (up!)
Ka (up!) pKa (down) conjugate base strength (down) Kb (down) pKb (up) |
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strong acid
Ka? pKa? Weak acid Ka? pKa? |
strong acid
Ka? much larger than 1 pKa? negative number Weak acid Ka? between 10^-14 and 1 pKa? between 0 and 14 |
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Haloacids and strength?
HF HCl HBr HI |
Descending --> size increases--> bond length increase --> strength decrease --> dissociation increase --> acidity increase
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Two factors to count when comparing acidity of oxyacids
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1) Excess Oxygen number (# O - # H) which corresponds to # of pi bonds. more resonance withdrawal --> stronger acid
2) Electronegativity of central atom. More electronegative ones have stronger inductive effect, thus stronger acid |
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For polyprotic acids, the pKa values of 1st and 2nd proton?
pKb? |
1st proton has much lower pKa. But know that pKa(1) + pKb(2) =14 and pKa(2) + pKb(2) = 14.
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pH of a weak acid?
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pH (weak acid) = 1/2 pKa - 1/2 log[HA]
THus know that if [HA] is ~1 M, pH is 1/2 of pKa |
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pOH of a weak base?
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pOH = 1/2 pKb - 1/2 log[A-]
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A buffer is normally made of
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a weak acid and and its weak conjugate base (both must be weak)
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Henderson-Hasselbalch eqauation--- what is it and what does it mean?
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Quantifiable verification of pH change in buffer solution.
pH = pKa + log[A-]/[HA] pH range = pKa +/- 1 As [A-] increases, buffer pH increases as well. |
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The color change range of an indicator
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pKa (indicator) +/- 1
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Best approximation scenario for the titration of a weak acid by a strong base
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1/2 pKa(HA) + 1/2 pH(titrant base) = pKa(ind) +/- 1
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Best approximation scenario for the titration of a weak base by a strong acid
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1/2 pKa(HA, conjugate acid) + 1/2 pH(titrant acid) = pKa(ind) +/- 1
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ΔG(reaction)=
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ΔG(reaction)=-nFε(cell)
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ΔG(reaction)=-nFε(cell)=ΔG*+RTlnQ |
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ε(reaction)=
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ε(reaction)=ε(reduction) + ε(oxidation)
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ε(reaction)=ε*+RT/nF lnQ |
