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“pH Measurement and Titration.”
Author(s) -
Pratt P. F.
Publication year - 1962
Publication title -
agronomy journal
Language(s) - English
Resource type - Journals
SCImago Journal Rank - 0.752
H-Index - 131
eISSN - 1435-0645
pISSN - 0002-1962
DOI - 10.2134/agronj1962.00021962005400030040x
Subject(s) - citation , library science , titration , mathematics , computer science , chemistry , inorganic chemistry
pH is a measure of the acidity of a solution. It is defined as the –log[H3O]. H3O (protonated water) is the strongest acid that can exist in water. Any stronger acids, such as HCl, completely dissociate in water to form H3O and an anion (Cl in the case of HCl). Weak acids do not completely dissociate when dissolved in water. The measure of the strength of a weak acid is its dissociation constant (Ka); the smaller the acid dissociation constant, the weaker the acid and the smaller its extent of dissociation in water. More basic conditions are required to remove the protons from weaker acids. The pKa, which is defined as the –log Ka, is pH at which the concentration of the weak acid and base conjugate pairs are equal.