The Kb value for pyridine, C5H5N is 1.7×10−9.
The Kb of pyridine (C5H5N) is 1.70×10-9.
It generally describes the degree of ionization of an acid or base and is a true indicator of acid or base strength since the addition of water to a solution does not change the equilibrium constant. Therefore, it determines the pH value of a 0.2 M pyridine solution of 9.24.
In pyrrole, the electron pair is part of the aromatic system. As a result, pyrrole is a very weak base. Pyridine is a weaker base than saturated amines of similar structure because its electron pair is in an sp2 hybridized orbital and the electron pair is more tightly held by the atom.
Pyridine is a Lewis base that donates its electron pair to a Lewis acid. Its Lewis base properties are discussed in the ECW model.
The pH of a 0.10 M solution of pyridine (C5H5N; Kb = 1.7 × 10– 9) is 9.12.
Pyridine is a heterocyclic compound that is a colorless to yellow liquid with the chemical formula C5H5N. The basicity of amines is due to the availability of a lone pair of electrons on nitrogen.
0.25 M solution of pyridine chloride C5H6N^ + Cl^ – has a pH of 2.699.
1. An explanation of the basic character of piperidine, pyridine and pyrrole (pKb= 2.9, pKb= 8.8 and pKb= 13.6 respectively) by Saurav K.
Pyrrole is a much weaker base than pyridine (see above). This is because the lone pair of electrons on the N atom is already involved in the aromatic arrangement of the p electrons. Protonation leads to loss of aromaticity and is therefore unfavorable.
This lone pair of electrons is available to form a new bond with a proton or Lewis acid. <br> Pyridine is less basic than triethylamine because the lone nitrogen pair is delocalized in pyridine. Step-by-step solution provided by experts to help you clarify & Achieve excellent grades in exams.
13.6 (pKa 0.4 for CA)
The best way to quantify the basicity of an amine is by examining the pKa of its conjugate acid. The higher the pKa of the conjugate acid, the stronger the base.