Konstanta disocijacije kiseline

Acetic acid, CH3COOH, is composed of a methyl group, CH3, bound chemically to a carboxylate group, COOH. The carboxylate group can lose a proton and donate it to a water molecule, H20, leaving behind an acetate anion CH3COO- and creating a hydronium cation H3O. This is an equilibrium reaction, so the reverse process can also take place.
Sirćetna kiselina, slaba kiselina, donira proton (vodonični jon, označen u zelenom) vodi u ravnotežnoj reakciji čime nastaje acetatni jon i hidronijum jon.
Kiseline i baze
Konstanta disocijacije kiseline
Kiselo-bazna ekstrakcija
Teorije kiselina i baza
Kiselo-bazna titracija
Konstanta disocijacije
Funkcija kiselosti
Puferi
pH
Protonski afinitet
Autojonizacija vode
Jačina kiseline
Tipovi kiselina
Brensted •Luis •Mineralne
Organske •Jake
Superkiseline •Slabe
Tipovi baza
Brensted •Luis •Organske
Jake •Superbaze
Nenukleofilne •Slabe

Konstanta disocijacije kiselina, Ka, (kiselinska konstanta, konstanta jonizacije kiseline) je kvantitativna mera jačine kiseline u rastvoru. To je konstanta ravnoteže hemijske reakcije poznate kao disocijacija u kontekstu kiselo-baznih reakcija.[1][2] Ravnoteža se može simbolički zapisati kao:

HA u ekvilibrujumu sa A− + H+,

gde je HA generička kiselina. Ona se disocira u A−, koji je poznat kao konjugovana baza kiseline, i vodonični jon ili proton, H+, koji u slučaju vodenih rastvora, postoji kao solvatisani hidronijumski jon. U primeru prikazanom na slici, HA je sirćetna kiselina, a A− je acetatni jon. Hemijske grupe HA, A− i H+ su u ravnoteži kad se njihove koncentracije ne menjaju u funkciji vremena. Konstanta disocijacije se obično zapisuje kao količnik ravnotežnih koncentracija (u mol/L), obleleženih sa [HA], [A−] i [H+][3]:

Pošto Ka vrednosti pokrivaju opseg sa znatnim brojem redova veličina, logaritamska mera konstante disocijacije kiseline se normalno koristi u praksi.

Što je veća pKa vrednost, to je manji stepen disocijacije. Slabe kiseline imaju pKa vrednosti u aproksimativnom opsegu −2 do 12 u vodi. Kiseline sa pKa vrednošću manjom od oko −2 se smatraju jakim kiselinama. Jaka kiselina je skoro potpuno disocirana u vodenom rastvoru, t. j. do te mere da koncentracija nedisocirane kiseline postaje zanemarljiva. pKa vrednosti jakih kiselina se mogu, međutim, proceniti teorijskim putem ili ekstrapolacijom iz merenja u nevodenim rastvaračima u kojima je konstanta disocijacije manja, poput acetonitrila i dimetil sulfoksida.[4]

Reference

  1. ↑ Skoog D.A., West, D.M.; Holler, J.F.; Crouch, S.R. (2004). Fundamentals of Analytical Chemistry (8th izd.). Thomson Brooks/Cole. ISBN 0-03-035523-0. 
  2. ↑ Rajković M. B. i saradnici (1993). Analitička hemija. Beograd: Savremena administracija. 
  3. ↑ Peter Atkins, Julio de Paula (2001). Physical Chemistry (7th edition izd.). W. H. Freeman. ISBN 0716735393. 
  4. ↑ Reichardt C. (2003). Solvents and Solvent Effects in Organic Chemistry (3rd izd.). Wiley-VCH. ISBN 3-527-30618-8. 

Literatura

  • Albert A., Serjeant, E.P. (1971). The Determination of Ionization Constants: A Laboratory Manual. Chapman & Hall. ISBN 0412103001.  (Previous edition published as Ionization constants of acids and bases. London (UK): Methuen. 1962. )
  • Atkins P.W., Jones, L. (2008). Chemical Principles: The Quest for Insight (4th izd.). W.H. Freeman. ISBN 1-4292-0965-8. 
  • Housecroft C. E., Sharpe A. G. (2008). Inorganic Chemistry (3rd izd.). Prentice Hall. ISBN 978-0-13-175553-6.  (Non-aqueous solvents)
  • Hulanicki A. (1987). Reactions of Acids and Bases in Analytical Chemistry. Horwood. ISBN 0853123306.  (translation editor: Mary R. Masson)
  • Perrin D.D., Dempsey, B., Serjeant, E.P. (1981). pKa Prediction for Organic Acids and Bases. Chapman & Hall. ISBN 041222190x. 
  • Skoog D.A., West, D.M.; Holler, J.F.; Crouch, S.R. (2004). Fundamentals of Analytical Chemistry (8th izd.). Thomson Brooks/Cole. ISBN 0-03-035523-0. 
  • Reichardt C. (2003). Solvents and Solvent Effects in Organic Chemistry (3rd izd.). Wiley-VCH. ISBN 3-527-30618-8. 

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