Question

Explain The concept of BRONSTED -LOWRYS CONCEPT OF ACIDS AND BASES how we can identify whether the acids or bases are examples of bronsted lowrys

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Answer 1

Explanation:

Bronsted lowry acid is one that can produce H+ by any form- even by accepting OH-

eg B(OH)3 + H2O = B(OH)4- + H+

Brownsted base can produce OH- by any means

NH3 + H2O = NH4+ + OH-

You will have to remember some common examples

Generally Alkali and alkaline metal hydroxide and halgon acids are not brownsted.

Mostly p block elements form brownsted acid and base.

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Answer 2

Answer :-

This theory was given by a Danish chemist, Bronsted and an english chemist Lowry in 1923.

According to this theory -

An acid is a substance that has tendency to release proton and base is a substance which has tendency to accept the proton.

Bronsted and Lowry theory is also known as proton donar and proton acceptor theory.

To determine whether a substance is a acid or base, check the number of hydrogen of a substance on both side. If a subtance has more hydrogen on reactant side than on the product side, than the subtance is acid ( Proton donar ).

If the number of a hydrogen of a substance on product side is more than reactant side, than the subtance is base ( Proton acceptor ).

For eg :-

$\sf HCl + H_2O \leftrightharpoons H_3O^+ + Cl^-$

Here, HCl is donating a proton to water. So, HCl is acid and water is accepting a proton, so water is base.

More examples :-

$\sf NH_3 + H_2O \leftrightharpoons NH_4^+ + OH^-$

Here, water is donating a proton, so water is acting as a acid and NH₃ is accepting the proton and hence acting as a base.

$\sf CH_3COOH + H_2O \leftrightharpoons H_3O^+ + CH_3COO^-$

Here, CH₃COOH is donating a proton and acting as a acid and water is accepting a proton and acting as base.

Note :- The species like H₂O , NH₃ , CH₃COOH which can act as both acid and base are called amphiprotic.

Also, according to the theory, a base when accepts the proton changes to an acid known as conjugate acid.

Also, an acid on losing a proton changes to base known as conjugate base.

$\bf CH_3COOH + H_2O \leftrightharpoons H_3O^+ + CH_3COO^-$

$\sf CH_3COOH \: loses\: H^+ \:and\: form \:CH_3COO^-$

$\sf H_2O \:accepts \:H^+\: and\: form \:H_3O^+$

Here,

$\sf CH_3OO^- \: ion\: is \:conjugate \:base \:of \:CH_3COOH$

$\sf H_3O^+ \:ion\: is \:conjugate\: acid \:of \:H_2O$