Calculate the pOH of a 0.01 text{ M} monobasi | vedclass

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(B) Step $1$: Since the monobasic acid is completely dissociated, the concentration of hydrogen ions is $[H^+] = 0.01 	ext{ M} = 10^{-2} 	ext{ M}$.S

Vedclass · Accepted Answer

$12$

Vedclass · Answer

(B) Step $1$: Since the monobasic acid is completely dissociated, the concentration of hydrogen ions is $[H^+] = 0.01 	ext{ M} = 10^{-2} 	ext{ M}$.Step $2$: Calculate the $pH$ using the formula $pH = -\log[H^+]$. Thus, $pH = -\log(10^{-2}) = 2$.Step $3$: At $298 	ext{ K}$, the relationship between $pH$ and $pOH$ is $pH + pOH = 14$.Step $4$: Substitute the value of $pH$: $2 + pOH = 14$, which gives $pOH = 12$.

Calculate the $pOH$ of a $0.01 \text{ M}$ monobasic acid solution that is completely dissociated at $298 \text{ K}$.

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