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Equilibrium

Short Answer Type

221.

How does Lewis concept account for the acidic character of carbon dioxide?

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222.

What are the limitations of Lewis concept of acids and bases ?

406 Views

Long Answer Type

223.
Justify the statement: All Bronsted bases are Lewis bases, but all Bronsted acids are not Lewis acids.

(i) All Bronsted bases are also Lewis bases: According to Bronsted concept, the base is a substance which accepts a proton. According to Lewis concept, a base is a substance which can donate a pair of electron. Any substance which can donate a pair of an electron can easily accept a proton.

Thus all Bronsted bases are all Lewis bases.

(ii) All Bronsted acids are not Lewis acids: According to Bronsted concept, an acid is a substance that can donate a proton (H⁺). According to Lewis concept, an acid is any substance (molecule or ion) which can accept a pair of electrons from another substance to form a coordinate bond. HCl, H₂SO₄ are Bronsted acids because they can donate protons, but they cannot accept a pair of electrons to form a coordinate bond, therefore, they are not Lewis acids. Thus all Bronsted acids are not Lewis acids.

377 Views

Short Answer Type

224.

Out of Lowry Bronsted concept and Lewis concept, which is regarded as better and why?

168 Views

Long Answer Type

225.

What do you understand by ionic product of water?

101 Views

Short Answer Type

226. What is the effect of temperature on (ionic product of water)?

714 Views

227.

The ionic product of water is 0·11 × 10^–14 at 273 K; 1·0 × 10^–14 at 298K and 51 × 10^–14 at 373K. Deduce from this data whether the ionisation of water into hydrogen and hydroxide ion is exothermic or endothermic.

108 Views

Long Answer Type

228.

Comment on the statement: An acidic solution contains OH^– ions and even a basic solution contains H₃O⁺ ions.
Or
How the values of K_w, [H₃O⁺] and [OH^–] are affected if acid or base is added to pure water at 298K?