Question

# From the following reactions identify each of an Arrhenius acid or base, Bronsted - Lowry acid or base, Lewis acid or base.A. $\text{NaOH, in NaOH }\to \text{ N}{{\text{a}}^{+}}\text{ + O}{{\text{H}}^{-}}$B. $\text{HCl, in HCl }\to \text{ }{{\text{H}}^{+}}\text{ + C}{{\text{l}}^{-}}$C. $\text{N}{{\text{H}}_{3}}\text{, in N}{{\text{H}}_{3}}\text{ }\to \text{ }{{\text{H}}^{+}}\text{ + NH}_{4}^{+}$D. $\text{NH}_{4}^{+}\text{, in NH}_{4}^{+}\text{ }\to \text{ N}{{\text{H}}_{3}}\text{ + }{{\text{H}}^{+}}$E. ${{\text{(C}{{\text{H}}_{3}}\text{)}}_{3}}\text{N:, in (C}{{\text{H}}_{3}}{{\text{)}}_{3}}\text{N: + B}{{\text{F}}_{3}}\text{ }\to \text{ (C}{{\text{H}}_{3}}{{\text{)}}_{3}}\text{N}:\text{B}{{\text{F}}_{3}}$

-In the fifth option, ${{\text{(C}{{\text{H}}_{3}}\text{)}}_{3}}\text{N:}$ is considered as the Lewis base because according to the reaction it is donating a pair of the electron to boron to full fill its octet.