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Ionization Constants of Weak Acids

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Acidities of Common Compounds at room temperature (25oC)

Acid  Ka pKa
Hydrogen Iodide, HI (strongest acid)  ~1.0 x 1010 -10.0
Hydrogen Bromide, HBr ~1.0 x 109 -9.0
Hydrogen Chloride, HCl ~1.0 x 108 -8.0
Sulfuric Acid, H2SO4 ~1.0 x 103 -3.0
Hydronium ion, H3O+ 50 -1.7
Nitric Acid, HNO3 25 -1.4
Hydrogen Fluoride, HF 6.3 x 10-4 3.2
Acetic Acid, CH3COOH 2.0 x 10 -5 4.7
Hydrogen Cyanide, HCN 6.3 x 10-10 9.2
Ammonium Ion, NH4+ 5.7 x 10-10 9.3
Methanol, CH3OH 3.2 x 10-16 15.5
Water, H2O 2.0 x 10-16 15.7
Ammonia, NH3 1.0 x 10-35 35
Methane, CH4 (weakest acid)  ~1.0 x 10-50 ~50
 
Compound Equilibrium pKa ΔHStrikeO.png /kJ·mol−1 TΔSStrikeO.png /kJ·mol−1
HA = Acetic acid HA is in equilibrium with H+ + A 4.756 −0.41 27.56
H2A+ = GlycineH+ H2A+ is in equilibrium with HA + H+ 2.351 4.00 9.419
  HA is in equilibrium with H+ + A 9.78 44.20 11.6
H2A = Maleic acid H2A is in equilibrium with HA + H+ 1.92 1.10 9.85
  HA is in equilibrium with H+ + A2− 6.27 −3.60 39.4
H3A = Citric acid H3A is in equilibrium with H2A + H+ 3.128 4.07 13.78
  H2A is in equilibrium with HA2− + H+ 4.76 2.23 24.9
  HA2− is in equilibrium with A3− + H+ 6.40 −3.38 39.9
HA = Boric acid HA is in equilibrium with H+ + A 9.237 13.80 38.92
H3A = Phosphoric acid H3A is in equilibrium with H2A + H+ 2.148 −8.00 20.26
  H2A is in equilibrium with HA2− + H+ 7.20 3.60 37.5
  HA2− is in equilibrium with A3− + H+ 12.35 16.00 54.49
HA = Hydrogen sulfate HA is in equilibrium with A2− + H+ 1.99 −22.40 33.74
H2A = Oxalic acid H2A is in equilibrium with HA + H+ 1.27 −3.90 11.15
  HA is in equilibrium with A2− + H+ 4.266 7.00 31.35

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Last Modified
10:07, 2 Oct 2013

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