# 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.

• 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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