Which of the following will decrease the pH o | vedclass

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(A) The initial $pH$ of $0.01 \ M \ HCl$ is $-\log(0.01) = 2$. To decrease the $pH$, the concentration of $H^+$ ions must increase. Option $A$: Adding

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addition of $5 \ mL$ of $1 \ M \ HCl$

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(A) The initial $pH$ of $0.01 \ M \ HCl$ is $-\log(0.01) = 2$. To decrease the $pH$, the concentration of $H^+$ ions must increase. Option $A$: Adding $5 \ mL$ of $1 \ M \ HCl$ adds $5 \ mmol$ of $H^+$ to the existing $0.5 \ mmol$. The new concentration becomes $\frac{5.5 \ mmol}{55 \ mL} = 0.1 \ M$. The new $pH$ is $-\log(0.1) = 1$. Since $1 Option $B$: Adding $50 \ mL$ of $0.01 \ M \ HCl$ results in the same concentration $(0.01 \ M)$, so the $pH$ remains $2$. Option $C$: Adding $50 \ mL$ of $0.002 \ M \ HCl$ dilutes the solution, decreasing the $H^+$ concentration and increasing the $pH$. Option $D$: Adding $Mg$ reacts with $HCl$ to consume $H^+$ ions, increasing the $pH$.

Which of the following will decrease the $pH$ of a $50 \ mL$ solution of $0.01 \ M \ HCl$?

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