Do you expect different products in solution when aluminium (III) chloride and potassium chloride treated separately with

(i) alkaline water

(ii) acidified water, and

(iii) normal water. Write equations wherever necessary.

Asked by Abhisek | 1 year ago |  149

##### Solution :-

Potassium chloride (KCl) is the salt of a strong acid (HCl) and strong base (KOH). Hence, it is neutral in nature and does not undergo hydrolysis in normal water. It dissociates into ions as follows:

$$KCl_{(g)}\rightarrow K^{+}_{(aq)}+Cl^{-}_{(aq)}$$

In acidified and alkaline water, the ions do not react and remain as such. Aluminium (III) chloride is the salt of a strong acid (HCl) and weak base [Al(OH)3]. Hence, it undergoes hydrolysis in normal water.

$$AlCl_{3(g)}+3H_{2}O_{(l)}\rightarrow Al(OH)_{3(s)}+3H^{+}_{(aq)}+3Cl^{-}_{aq}$$

In acidified water, H+ ions react with Al(OH)3 forming water and giving Al3+ ions. Hence, in acidified water, AlCl3 will exist as

$$Al^{3+}_{(aq)}​$$ and $$Cl^{-}_{(aq)}$$

Answered by Pragya Singh | 1 year ago

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