Assuming complete ionisation,the pH of 0.1 M | vedclass

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(A) The correct option is $A$. The $pH$ of $0.1 \ M \ HCl$ is $1$,which means the concentration of hydrogen ions $[H^{+}]$ is $0.1 \ M$.For $H_2SO_4$,

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$0.05$

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(A) The correct option is $A$. The $pH$ of $0.1 \ M \ HCl$ is $1$,which means the concentration of hydrogen ions $[H^{+}]$ is $0.1 \ M$.For $H_2SO_4$,the dissociation reaction is: $H_2SO_4 \rightarrow 2H^{+} + SO_4^{2-}$.Since $1 \ mole$ of $H_2SO_4$ produces $2 \ moles$ of $H^{+}$ ions,the molarity of $H_2SO_4$ required to produce $0.1 \ M \ H^{+}$ ions is calculated as:$[H_2SO_4] = \frac{[H^{+}]}{2} = \frac{0.1 \ M}{2} = 0.05 \ M$.

Assuming complete ionisation,the $pH$ of $0.1 \ M \ HCl$ is $1$. The molarity of $H_2SO_4$ with the same $pH$ is (in $M$)

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