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(A) For $HCl$,$pH = 1$ implies $[H^+] = 10^{-pH} = 10^{-1} = 0.1 \ M$. Since $HCl$ is a monobasic acid,its normality $(N)$ is equal to its molarity $(

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$0.1$

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(A) For $HCl$,$pH = 1$ implies $[H^+] = 10^{-pH} = 10^{-1} = 0.1 \ M$. Since $HCl$ is a monobasic acid,its normality $(N)$ is equal to its molarity $(M)$,so $N_{HCl} = 0.1 \ N$. For $H_2SO_4$ to have the same $pH$,it must have the same concentration of $H^+$ ions,which is $[H^+] = 0.1 \ M$. Normality is defined as the concentration of $H^+$ ions in the solution. Therefore,the normality of the $H_2SO_4$ solution must be $0.1 \ N$.

For a solution of $HCl$ assuming complete ionization,the $pH = 1$. Find the normality of a $H_2SO_4$ solution having the same $pH$.

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