Short Answer Type
Long Answer TypeJustify the statement:Â All Bronsted bases are Lewis bases, but all Bronsted acids are not Lewis acids.
Short Answer TypeOut of Lowry Bronsted concept and Lewis concept, which is regarded as better and why?
Long Answer TypeShort Answer TypeThe 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.
Long Answer TypeComment on the statement: An acidic solution contains OH– ions and even a basic solution contains H3O+ ions.
Or
How the values of Kw, [H3O+] and [OH–] are affected if acid or base is added to pure water at 298K?
We know, [H3O+][OH–] = Kw
For pure water, [H3O+] =[OH–]
= 1 × 10–7 mol L–1
On adding few drops of an acid (say HCl) to water, the concentration of H3O+ increases and thus concentration OH– decreases accordingly in order to maintain Kw constant.
Hence acidic solution contains both hydronium and hydroxyl ions. But 
 But on adding.Â
But on adding few drops of a base (say NaOH) to water, the concentration of OH–increases and thus the concentration of H3O+ decreases accordingly in order to maintain Kw constant.
Hence basic solution contains both hydronium and hydroxyl ions.
But [H3O+] < [OH–]
In general, in neutral solution,
[H3O+] = [OH–]
In acidic solution, [H3O+] > [OH–]
In basic solution, [H3O+] < [OH–]
Short Answer Type
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