Question

1. Write the equations for the reaction of the following Bronsted acids with water: (a) NH4 + (b) H3C6H5O7 (c) H2SO4

2. Write equations for the reactions of the following Bronsted bases with water: (a) HCO2 - (b) (CH3)2NH (c) SO4 2-

Answer 1

1. Bronsted acids lose their proton(H⁺) in water and forms its conjugate base and hydronium ion(H₃O⁺) .

(a) NH₄⁺ + H₂O ----> NH₃ + H₃O⁺

(b)  H3C6H5O7 + H₂O ----> H₃C₆H₄O₇^{-​​​​​} + H₃O⁺

(c) H₂SO₄ + H₂O ----> HSO4^- + H₃O⁺

2. Bronsted base abstracts Proton(H⁺) from water and form its conjugate acid and Hydroxide ion(OH^-).

(a)HCO₃^- + H₂O---> H₂CO₃ + OH^-

(b) (CH₃)₂NH + H₂O---> (CH₃)₂NH₂⁺+ OH^-

(c) SO₄^2- + H₂O---> HSO4^-+ OH^-