Question

The correct order of acidic nature is:

A. ${\text{HCl}}{{\text{O}}_{\text{4}}}\,{\text{ > }}\,{{\text{H}}_{\text{2}}}{\text{S}}{{\text{O}}_{\text{4}}}\,{\text{ > }}\,{\text{HP}}{{\text{O}}_4}$
B. ${\text{HCl}}{{\text{O}}_{\text{4}}}\,\,{\text{ > }}\,{\text{HP}}{{\text{O}}_4}{\text{ > }}\,{{\text{H}}_{\text{2}}}{\text{S}}{{\text{O}}_{\text{4}}}$
C. ${{\text{H}}_{\text{2}}}{\text{S}}{{\text{O}}_{\text{4}}}{\text{ > }}\,{\text{HCl}}{{\text{O}}_{\text{4}}}\,{\text{ > }}\,{\text{HP}}{{\text{O}}_4}$
D. \[{{\text{H}}_{\text{2}}}{\text{S}}{{\text{O}}_{\text{4}}}\,{\text{ > }}\,\,{\text{HP}}{{\text{O}}_4}\,{\text{ > }}\,{\text{HCl}}{{\text{O}}_{\text{4}}}\,\]

Answer 1

Hint: To determine the answer we should know what are acids and the factors on which the acidic strength depends. The species which accepts electrons are known as acids. The accepting power depends upon the deficiency of electrons. So, we will determine the most electron deficient molecule.


Complete solution:
As acids accept electrons so if there any factor which increases the electrons accepting power will increase the acidic nature.
We will draw the structure of the given molecules as follows:

Just by looking at the structure, we cannot say anything about the acidic nature of acids so, we will compare the oxidation states. A high oxidation state means, the high positive charge on the atom means more electron-deficient central atom so it will attract the electrons easily.
High positive charge means a high effective nuclear charge of an atom so an atom having a high oxidation state will attract more electron density hence will have high acidic nature.
Now we will determine the oxidation state of the central atom of each acid.
The oxidation of chlorine atoms in \[{\text{HCl}}{{\text{O}}_{\text{4}}}\,\]is as follows:
The oxidation state of oxygen is $ - 2$ and hydrogen is $ + 1$.
$\left( { + 1} \right)\, + \,( - 2 \times 4)\, + x\, = \,0$
$x\, = \, + 7$
So, the oxidation state of chlorine is $ + 7$.
The oxidation of sulphur atoms in \[{{\text{H}}_{\text{2}}}{\text{S}}{{\text{O}}_{\text{4}}}\]is as follows:
The oxidation state of oxygen is $ - 2$ and hydrogen is $ + 1$.
$\left( { + 1 \times 2} \right)\, + \,( - 2 \times 4)\, + x\, = \,0$
$x\, = \, + 6$
So, the oxidation state of sulphur is$ + 6$.
The oxidation of sulphur atoms in \[{\text{HP}}{{\text{O}}_4}\]is as follows:
The oxidation state of oxygen is $ - 2$ and hydrogen is $ + 1$.
$\left( { + 1 \times 3} \right)\, + \,( - 2 \times 4)\, + x\, = \,0$
$x\, = \, + 5$
So, the oxidation state of sulphur is$ + 5$.
As we know high oxidation state means high acidity so, the correct order of acidic nature will be, ${\text{HCl}}{{\text{O}}_{\text{4}}}\,{\text{ > }}\,{{\text{H}}_{\text{2}}}{\text{S}}{{\text{O}}_{\text{4}}}\,{\text{ > }}\,{\text{HP}}{{\text{O}}_4}$

Therefore, option (C) is correct.


Note: According to Arrhenius and Bronsted acids are proton donors and according to Lewis acids are electron acceptors. The electrons deficient species accepts electrons so, electrons deficient species behave as acids such as aluminium trichloride which behaves as Lewis acid. Acidic nature is directly proportional to the oxidation state, effective nuclear charge, the small size of the central atom, high polarizing power of the cation, presence of an electron-withdrawing group, etc.