Boric acid is basically a monobasic acid and a lewis acid, so what happens when Boric Acid is subjected to Ammonia in presence of ethanol?

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Solution

$A s t h e a c i d i s a L e w i s a c i d, i t a c c e p t s t h e e l e c t r o n f r o m t h e b a s e a m m o n i a . B (O H)_{3} + N H_{3} \overset{C_{2} H_{5} O H}{\to} B (O H {)_{4}}^{-} N {H_{2}}^{+}$

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Boric acid is polymeric due to
(a) its acidic nature (b) the presence of hydrogen bonds
(c) its monobasic nature (d) its geometry

	Column - I		Column - II
(A)	Hypo phosphoric acid	(p)	All hydrogen are ionizable in water
(B)	Pyro phosphoric acid	(q)	Lewis acid
(C)	Boric acid	(r)	Monobasic in water
(D)	Hypo phosphorus acid	(s)	$s p^{3}$ hybridized central atom

B (O H)_{3}

H^{+}

B (O H)_{3} + H_{2} O ⇌ [B (O H)_{4}]^{-} + H^{+}, K_{a} = 5.9 \times 10^{- 10}

P^{H}

0.025 M

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