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(C) To find the $pH$ of each solution:$(1) 0.005 \, M \, H_2SO_4$: Since $H_2SO_4$ is a strong diprotic acid,$[H^+] = 2 	imes 0.005 = 0.01 \, M = 10^

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$1, 4$

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(C) To find the $pH$ of each solution:$(1) 0.005 \, M \, H_2SO_4$: Since $H_2SO_4$ is a strong diprotic acid,$[H^+] = 2 	imes 0.005 = 0.01 \, M = 10^{-2} \, M$. Thus,$pH = -\log(10^{-2}) = 2$.$(2) 0.1 \, M \, Na_2SO_4$: This is a salt of a strong acid and a strong base,so it is neutral. $pH = 7$.$(3) 10^{-2} \, M \, NaOH$: Since $NaOH$ is a strong base,$[OH^-] = 10^{-2} \, M$. Thus,$pOH = -\log(10^{-2}) = 2$,and $pH = 14 - 2 = 12$.$(4) 0.01 \, M \, HCl$: Since $HCl$ is a strong monoprotic acid,$[H^+] = 0.01 \, M = 10^{-2} \, M$. Thus,$pH = -\log(10^{-2}) = 2$.Comparing the $pH$ values,solutions $(1)$ and $(4)$ have the same $pH$ of $2$.

Select the correct option that has the same $pH$ value.
$(1) 0.005 \, M \, H_2SO_4$
$(2) 0.1 \, M \, Na_2SO_4$
$(3) 10^{-2} \, M \, NaOH$
$(4) 0.01 \, M \, HCl$

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Select the correct option that has the same $pH$ value.$(1) 0.005 \, M \, H_2SO_4$$(2) 0.1 \, M \, Na_2SO_4$$(3) 10^{-2} \, M \, NaOH$$(4) 0.01 \, M \, HCl$