![]() Two factors determine the stability of an acid's conjugate base. If deprotonation of the acid gives a very stable conjugate base then deprotonation of the acid will be more favorable. 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. This leads to the third major factor that should be considered when thinking about acid strength. 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. ![]()
0 Comments
Leave a Reply. |
AuthorWrite something about yourself. No need to be fancy, just an overview. ArchivesCategories |