Question

Do you expect different products in solution when aluminium(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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Answer 1

$\huge\pink{\sf Answer}$

(1) $\sf AlCl_3$ is a weak salt base $\sf Al(OH)_3$ and strong acid HCl . it undergoes Hydrolysis in normal water.

$\sf\bullet \: AlCl_3 + 3H_2O \dashrightarrow Al(OH)_3 +3H^+ + 3Cl-$

Thus, its aqueous solution is acidic in Nature.

$\rule{130}{1.5}$

(ii) In acidified water, H+ reacts with $\sf Al(OH)_3$ to produce $\sf {Al_3}^+$ ion and $\sf H_2O$. Therefore,in acidified water $\sf {AlCl}_3$ exists In the form of $\sf {Al_3}^{+}$ and $\sf Cl^-$ ions.

(iii) In Alkaline water $\sf AlCl_3$ produce the following products.

$\bullet \sf \: AlCl3 \dashrightarrow {Al(OH)_4}^{-} + 3Cl^-$

$\bullet\sf \: {Al(OH)_4}^{-} \dashrightarrow {AlO_2}^{-} + 2H_2O$

$\rule{130}{1.5}$

»» So now talking about KCl. We know that it is the salt of a strong acid HCL and strong base KOH. And so this makes it such that it doesn't undergo hydrolysis in Normal Water.

»» It only dissociate in water to produce $\sf K^+$ and $\sf Cl ^ - ion$.

»» So we may conclude that KCl is a Neutral salt and that it doesn't show any reaction.

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