How does ammonia behave as a Bronsted base: $"(i) "NH_3(g) + 7/2O_2(g) rarr 2NO_2(g) + 3H_2O$ $"(ii) "2NH_3(g) rarr NH_4^+ +NH_2^(-) $ $"(iii) "NH_3(g) + H_3CBr(g) rarr H_3CBr(g) + HBr(g)$ $"(iv) "NH_3(aq) +H_2O(l) rarr NH_4^+ + HO^-$?

Md Ariful Islam

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Md Ariful Islam

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Ammonia is a Bronsted base:

$NH_3(aq) + H_2O(l) rightleftharpoons NH_4^+ + OH^-$ $pK_b = 4.75$

I am not going to solve this equation using $pK_b$, but most of the ammonia is present as $NH_3$, the free base.

For AS/A2 level; ammonia is a very water like . In pure ammonia another acid/base equilibrium operates, that is comparable to the $H_3O^+; OH^-$ equilibrium in water.

$2NH_3(l) rightleftharpoons NH_2^(-) + NH_4^+$

THIS ONLY OPERATES IN LIQUID AMMONIA; IT DOES NOT OPERATE IN WATER. The amide ion, $NH_2^-$, does not exist in water.

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