The correct increasing order of the acidity of $C O_{2}, H_{2} O$ and $H_{2} O_{2}$ is:

C O_{2} < H_{2} O_{2} < H_{2} O

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H_{2} O < H_{2} O_{2} > C O_{2}

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H_{2} O < H_{2} O_{2} < C O_{2}

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H_{2} O_{2} < H_{2} O < C O_{2}

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Solution

The correct option is C $H_{2} O < H_{2} O_{2} < C O_{2}$
An acid is a proton (hydrogen ion), donor.
A base is a proton (hydrogen ion), the acceptor.
$H_{2} O_{2}$ gives $2$ hydrogen ions in aqueous solution whereas water gives $1$ hydrogen ion. As $H_{2} O_{2}$ protonates to a larger extent than water in aqueous solution, hence, it has a larger Ka(acid dissociation constant), thus making it a stronger Bronsted-Lowry acid than water.
Hydrogen peroxide has a pH rating between $1$ to $5$ whereas carbon dioxide has a pH rating of $6$ . Therefore hydrogen peroxide is slightly more acidic than carbon dioxide.
The correct increasing order stands as $H_{2} O < H_{2} O_{2} < C O_{2}$ .

$H e n c e t h e c o r r e c t a n s w e r i s o p t i o n (C)$ .

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