The correct order of increasing $[H_{3} O^{+}]$ in the following aqueous solution is

0.01 M H_{2} S < 0.01 M H_{2} S O_{4} < 0.01 M N a C l < 0.01 M N a N O_{2}

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0.01 M N a C l < 0.01 M N a N O_{2} < 0.01 M H_{2} S < 0.01 M H_{2} S O_{4}

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0.01 M N a N O_{2} < 0.01 M N a C l < 0.01 M H_{2} S < 0.01 M H_{2} S O_{4}

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0.01 M H_{2} S < 0.01 M N a N O_{2} < 0.01 M N a C l < 0.01 M H_{2} S O_{4}

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Solution

The correct option is C $0.01 M N a N O_{2} < 0.01 M N a C l < 0.01 M H_{2} S < 0.01 M H_{2} S O_{4}$
The correct order of increasing $[H_{3} O^{+}]$ in the following aqueous solution is $0.01 M N a N O_{2} < 0.01 M N a C l < 0.01 M H_{2} S < 0.01 M H_{2} S O_{4}$
The molarity of all the four compounds is same.
Sulphuric acid is a strong acid and hydrogen sulphide has weak acidic behaviour. NaCl is a neutral compound (as it is salt of strong acid HCl and strong base NaOH and it does not undergo hydrolysis in water). Sodium nitrite is basic in nature (it is salt of weak acid nitrous acid and strong base NaOH).

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[H_{3} O^{+}]

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