Explain Arrhenius’ concept of acid and base. Arrhenius’ concept of acid and base -: In 1887, Arrhenius put forward the theory of electrolytic dissociation, which resulted in a revision of the hydrogen concept of acid.
This blog is one of my students Ritika Rathor B.Sc Written by a first-year student. Thanks, Ritika
Explain Arrhenius’s concept of acid and base.
According to Arrhenius’ theory, acids were substances that gave hydroxyl ions in water solutions.
HCl + H2O }——-> (H+) + (Cl-)
Alkali -: NaOH + H2O }———->(Na+) + OH-
Hydrogen ions and hydroxyl ions combine to give water molecules. The process is known as neutralization.
(H+) + (OH-) ——-> H2O
Other examples of Arrhenius acids include sulfuric acid (H2SO4), hydrobromic acid (HBr), and nitric acid (HNO3). Examples of Arrhenius bases include sodium hydroxide (NaOH) and potassium hydroxide (KOH).
utility -:
It was helpful in understanding the catalytic properties of acids.
Limitations:-
1) This concept could not explain the acidic nature of some substances like AlCl3 in aqueous solution
2) It can only be applied to an aqueous solution, thus dry HCl will not act as an acid.
3) This concept fails to give an account of the behaviour of acids and bases in solvents other than water, such as non-aqueous solutions.
