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(D) For $(a)$,$HCl$ is a strong acid. $[H^+] = 0.01 \, M = 10^{-2} \, M$. Thus,$pH = -\log(10^{-2}) = 2$.For $(b)$,$H_2SO_4$ is a strong acid. $[H^+]

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$(a)$ and $(c)$ both

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(D) For $(a)$,$HCl$ is a strong acid. $[H^+] = 0.01 \, M = 10^{-2} \, M$. Thus,$pH = -\log(10^{-2}) = 2$.For $(b)$,$H_2SO_4$ is a strong acid. $[H^+] = 2 	imes 0.01 \, M = 0.02 \, M$. Thus,$pH = -\log(0.02) \approx 1.7$.For $(c)$,$moles \, of \, H_2SO_4 = 0.02 \, M 	imes 0.050 \, L = 0.001 \, mol$. $moles \, of \, H^+ = 2 	imes 0.001 = 0.002 \, mol$.$moles \, of \, NaOH = 0.02 \, M 	imes 0.050 \, L = 0.001 \, mol$. $moles \, of \, OH^- = 0.001 \, mol$.$Net \, moles \, of \, H^+ = 0.002 - 0.001 = 0.001 \, mol$.$Total \, volume = 50 \, mL + 50 \, mL = 100 \, mL = 0.1 \, L$.$[H^+] = \frac{0.001 \, mol}{0.1 \, L} = 0.01 \, M = 10^{-2} \, M$.Thus,$pH = -\log(10^{-2}) = 2$.Since $(a)$ and $(c)$ both result in a $pH$ of $2$,the correct option is $(d)$.

Assuming complete dissociation,which of the following aqueous solutions will have the same $pH$ value?

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