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. ${{\text{(C}{{\text{H}}_{3}}\text{)}}_{3}}\text{N:, in (C}{{\text{H}}_{3}}{{\text{)}}_{3}}\text{N: + B}{{\text{F}}_{3}}\text{ }\to \text{ (C}{{\text{H}}_{3}}{{\text{)}}_{3}}\text{N}:\text{B}{{\text{F}}_{3}}$

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. ${{\text{(C}{{\text{H}}_{3}}\text{)}}_{3}}\text{N:, in (C}{{\text{H}}_{3}}{{\text{)}}_{3}}\text{N: + B}{{\text{F}}_{3}}\text{ }\to \text{ (C}{{\text{H}}_{3}}{{\text{)}}_{3}}\text{N}:\text{B}{{\text{F}}_{3}}$

Vedantu Content Team · Accepted Answer

Hint:  Arrhenius base can release the hydroxyl ion whereas Arrhenius acid can release the hydrogen ion from the compound. Bronsted- Lowry acid donates hydrogen ion whereas Bronsted-Lowry base accepts hydrogen ion. Lewis acid is the species which can accept a pair of electrons whereas Lewis base can donate the pair of electrons.Complete answer: -In the given question we have to identify the Arrhenius base and acid, Bronsted Lowry acid and base & 	Lewis acid or base.-In the first reaction, we can see that sodium hydroxide releases sodium ion and hydroxyl ion and as we know that only base can release the hydroxyl ion.-Also, we can say that sodium hydroxide is Arrhenius base because they are those species which can release the hydroxyl ion.-Now, in the second option, we can see that hydrogen ion is released by hydrochloric acid so it will be considered as the Arrhenius acid.-Because Arrhenius acid is the species which can easily release hydrogen ions.-In the third option, ammonia is both Bronsted base and Lewis base because it can accept the hydrogen ion and forms ammonium ion as well as it can donate the electron pair to the nitrogen.-In the fourth option, ammonium ion is the Bronsted acid because it releases hydrogen ion to give ammonia.-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.Note: Conjugate base is the species in which one hydrogen atom is absent from the molecule whereas in conjugate acids are the species in which one extra hydrogen atom is present.

From the following reactions identify each of an Arrhenius acid or base, Bronsted - Lowry acid or base, Lewis acid or base.A. NaOH, in NaOH → Na+ + OH−B. HCl, in HCl → H+ + Cl−C. NH3, in NH3 → H+ + NH4+D. NH4+, in NH4+ → NH3 + H+E. (CH3)3N:, in (CH3)3N: + BF3 → (CH3)3N:BF3

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