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Kelvi

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Acidity of diprotic acids in aqueous solutions increases in the order

easy

Equilibrium

2014

chemistry

$H_2S < H_2Se < H_2Te$

$H_2Se < H_2S < H_2Te$

$H_2Te < H_2S < H_2Se$

$H_2Se < H_2Te < H_2S$

Explanation

To determine the acidity order of diprotic acids $(H_2S, H_2Se, H_2Te)$

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in aqueous solutions,

\\

we need to consider the trend in acidity down the group in the periodic table.

\\

• These acids belong to Group 16 (chalcogens) and their acidity is influenced by the

\\

bond strength between hydrogen and the chalcogen.

\\

• As we move down the group from sulfur (S) to tellurium (Te), the size of the chalcogen

\\

atom increases, leading to weaker H-X bonds.

\\

• Weaker H-X bonds result in easier release of

H^+

ions, thus increasing acidity.

\\

Therefore, the acidity order is determined by the ease of dissociation of the H-X bond:

\\

H

_2

S

<

H

_2

Se

<

H

_2

Te

\\

This corresponds to Option 1.

\\

In summary, the correct order of acidity is:

\\

H

_2

S

<

H

_2

Se

<

H

_2

Te

\\

This is because the bond strength decreases as the size of the chalcogen increases,

\\

making it easier for the acid to donate

H^+

ions.