Which of the following solutions will have pH | vedclass

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Question

(A) The $pH$ of a solution is calculated using the formula $pH = -\log[H^+]$.For $pH = 2$,the concentration of hydrogen ions $[H^+]$ must be $10^{-2}

Vedclass · Accepted Answer

$0.01 \, M \, HCl$

Vedclass · Answer

(A) The $pH$ of a solution is calculated using the formula $pH = -\log[H^+]$.For $pH = 2$,the concentration of hydrogen ions $[H^+]$ must be $10^{-2} \, M = 0.01 \, M$.$(A)$ $0.01 \, M \, HCl$: $HCl$ is a strong monoprotic acid,so $[H^+] = 0.01 \, M$. Thus,$pH = -\log(0.01) = 2$.$(B)$ $0.02 \, M \, HCl$: $[H^+] = 0.02 \, M$,so $pH = -\log(0.02) \approx 1.7$.$(C)$ $0.01 \, M \, H_2SO_4$: $H_2SO_4$ is a strong diprotic acid,so $[H^+] = 2 	imes 0.01 = 0.02 \, M$. Thus,$pH = -\log(0.02) \approx 1.7$.$(D)$ $0.02 \, M \, H_2SO_4$: $[H^+] = 2 	imes 0.02 = 0.04 \, M$,so $pH = -\log(0.04) \approx 1.4$.Therefore,the correct option is $A$.

Which of the following solutions will have $pH = 2$?

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