How can we identify strong acid and strong base?

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Solution

Strong Acids:-
Strong acids completely dissociate in water, forming H+ and an anion. There are six strong acids. The others are considered to be weak acids. You should commit the strong acids to memory:

HCl - hydrochloric acid
HNO3 - nitric acid
H2SO4 - sulfuric acid
HBr - hydrobromic acid
HI - hydroiodic acid
HClO4 - perchloric acid

If the acid is 100% dissociated in solutions of 1.0 M or less, it is called strong. Sulfuric acid is considered strong only in its first dissociation step; 100% dissociation isn't true as solutions become more concentrated.
H2SO4 → H+ + HSO4

Strong Bases:-
Strong bases dissociate 100% into the cation and OH- (hydroxide ion).
The hydroxides of the Group I and Group II metals usually are considered to be strong bases.

LiOH - lithium hydroxide
NaOH - sodium hydroxide
KOH - potassium hydroxide
RbOH - rubidium hydroxide
CsOH - cesium hydroxide
Ca(OH)2 - calcium hydroxide
Sr(OH)2 - strontium hydroxide
Ba(OH)2 - barium hydroxide
* These bases completely

dissociate in solutions of 0.01 M or less.

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S F_{4}

can act as Lewis acid in the presence of strong Lewis base and as Lewis base in the presence strong Lewis acid.

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