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What happens when
(a) Borax is heated strongly,
(b) Boric acid is added to water
(c) Aluminium is treated with dilute \(\mathrm{NaOH}\)
(d) \(\mathrm{BF}_3\) is reacted with ammonia?
(a) Borax is heated strongly,
(b) Boric acid is added to water
(c) Aluminium is treated with dilute \(\mathrm{NaOH}\)
(d) \(\mathrm{BF}_3\) is reacted with ammonia?
Solution:
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Verified Answer
(a) 
(b) Boric acid acts as a weak Lewis acid by accepting a hydroxide ion of water and releasing a proton into the solution.
\(\mathrm{H}-\mathrm{OH}+\mathrm{B}(\mathrm{OH})_3 \longrightarrow\left[\mathrm{B}(\mathrm{OH})_4\right]^{-}+\mathrm{H}^{+}\)
(c) Aluminum reacts to sodium tetrahydroxoaluminate (III) by forming dilute \(\mathrm{NaOH}\). In this process, hydrogen gas is liberated.
\(2 \mathrm{Al}(\mathrm{s})+2 \mathrm{NaOH}(\mathrm{aq})+6 \mathrm{H}_2 \mathrm{O}(\mathrm{l}) \longrightarrow\) \(2 \mathrm{Na}^{+}\left[\mathrm{Al}(\mathrm{OH})_4\right]^{-}(\mathrm{aq})+3 \mathrm{H}_2(\mathrm{~g})\)
(d) \(\mathrm{BF}_3\) being a Lewis acid accepts a pair of electrons from \(\mathrm{NH}_3\) to form the corresponding complex.
(b) Boric acid acts as a weak Lewis acid by accepting a hydroxide ion of water and releasing a proton into the solution.
\(\mathrm{H}-\mathrm{OH}+\mathrm{B}(\mathrm{OH})_3 \longrightarrow\left[\mathrm{B}(\mathrm{OH})_4\right]^{-}+\mathrm{H}^{+}\)
(c) Aluminum reacts to sodium tetrahydroxoaluminate (III) by forming dilute \(\mathrm{NaOH}\). In this process, hydrogen gas is liberated.
\(2 \mathrm{Al}(\mathrm{s})+2 \mathrm{NaOH}(\mathrm{aq})+6 \mathrm{H}_2 \mathrm{O}(\mathrm{l}) \longrightarrow\) \(2 \mathrm{Na}^{+}\left[\mathrm{Al}(\mathrm{OH})_4\right]^{-}(\mathrm{aq})+3 \mathrm{H}_2(\mathrm{~g})\)
(d) \(\mathrm{BF}_3\) being a Lewis acid accepts a pair of electrons from \(\mathrm{NH}_3\) to form the corresponding complex.
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