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# Do you expect different products in solution when aluminium(III) chloride and potassium chloride treated separately with(i)normal water(ii)acidified

9.34  Do you expect different products in solution when aluminum (III) chloride and potassium chloride treated separately with (i) normal water (ii) acidified water, and (iii) alkaline water? Write equations wherever necessary.

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• KCl is salt of KOH(strong base) and HCl(strong acid). So it does not hydrolyze in normal water because it is neutral in nature. It just simply ionizes in water.

$KCl\rightarrow K^{+}+Cl^{-}$ In acidified and alkaline water they do not dissociate into ions and remains the same.

• $AlCl_{3}$ is the salt of a weak base  $Al(OH)_{3}$ and HCl( strong acid).So it hydrolyzes in normal water.

$AlCl_{3}+H_{2}O\rightarrow Al(OH)_{3}+HCl$

In acidic water, there are  $H^{+}$ ions which react with $Al(OH)_{3}$ and form water molecule and give $Al^{3+}$ ions. In alkaline water,  $OH^{-}$ ions react with $Al(OH)_{3}$  and form $[Al(OH)_{4}]^{-}$and water molecules.

$Al(OH)_{3}+OH^{-}\rightarrow [Al(OH)_{4}]^{-}+H_{2}O$

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