All reactions are in theory reversible, and so when considering the propensity of an acid to donate hydrogen ions, it can be helpful to look at the reverse of hydrogen ion donation, namely, protonation of the acid's conjugate base. The more stable the acid's conjugate base, the stronger the Brønsted acid. Electronegativity Effects, Especially as Seen Using the Conjugate Base Principle This leads to the third major factor that should be considered when thinking about acid strength.ģ. Polarized E-H bonds also make for stronger Brønsted acids because the resulting \(E:^-\) conjugate base is more stable.This may be seen from how the pK a values of acetic acid and its mono-, di-, and tri-chlorinated derivatives decreases with the extent of chlorination of the methyl group. \)) it is easier to cleave off the hydrogen ion from that E-H bond.
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