Question

The correct statements among the following:
A) Ionic product of pure water is $1\times {10}^{-14}{M}^2$ at any temperature.
B) All Bronsted bases are Lewis bases.
C) Ionisation of acetic acid is suppressed in $C{H}_{3}COONa$.
D) All Lewis acids are Arrhenius acids.

• A. All are correct
• B. A and B are correct
• C. B and C are correct
• D. B, C and D are correct

Answer 1

The correct option is C B and C are correct

Ionic product of water is ${10}^{-14}{M}^2$ only at 25 degrees Celcius.

Lewis acids are those which can accept electron lone pairs whereas Bronsted acids are $H^{+}$ donors. All lewis bases can't be said as Bronsted acids.

Bronsted bases are $H^{+}$ acceptors and lewis bases are electron lone pair donors. All Bronsted bases can thus be said to be lewis bases.

$C{H}_{3}COOH\to C{H}_{3}CO{O}^{-}+H^{+}$.

In presence of $C{H}_{3}CO{O}^{-}$ the equilibrium is shifted towards the left-hand side and the dissociation decreases.

All Lewis acids are not Arrhenius acids. Example: $B{F}_3$.