why HCL
cannot act as
bronsted acid and Bronsted base
Answers
Hiii.
HCl IS A BRONSTED LOWRY BASE AND ACID.
The Brønsted-Lowry Theory of Acids and Bases
Brønsted-Lowry theory of acid and bases took the Arrhenius definition one step further, as a substance no longer needed to be composed of hydrogen (H+) or hydroxide (OH-) ions in order to be classified as an acid or base. For exmapl, consider the following chemical equation:
HCl(aq)+NH3(aq)→NH+4(aq)+Cl−(aq)(1)(1)HCl(aq)+NH3(aq)→NH4+(aq)+Cl−(aq)
Here, hydrochloric acid (HCl) "donates" a proton (H+) to ammonia (NH3) which "accepts" it , forming a positively charged ammonium ion (NH4+) and a negatively charged chloride ion (Cl-). Therefore, HCl is a Brønsted-Lowry acid (donates a proton) while the ammonia is a Brønsted-Lowry base (accepts a proton). Also, Cl- is called the conjugate base of the acid HCl and NH4+ is called the conjugate acid of the base NH3.
A Brønsted-Lowry acid is a proton (hydrogen ion) donor.
A Brønsted-Lowry base is a proton (hydrogen ion) acceptor.
In this theory, an acid is a substance that can release a proton (like in the Arrhenius theory) and a base is a substance that can accept a proton. A basic salt, such as Na+F-, generates OH- ions in water by taking protons from water itself (to make HF):
F−(aq)+H2O(l)⇌HF(aq)+OH−(2)(2)F(aq)−+H2O(l)⇌HF(aq)+OH−
When a Brønsted acid dissociates, it increases the concentration of hydrogen ions in the solution, [H+][H+]; conversely, Brønsted bases dissociate by taking a proton from the solvent (water) to generate [OH−][OH−]
Hope u Understood.
Thank You