Question
Find the $\mathrm{pH}$ of a buffer that consists of $0.25 \mathrm{M} \mathrm{NH}_{3}$ and $0.15 M \mathrm{NH}_{4} \mathrm{Cl}\left(\mathrm{p} K_{\mathrm{b}}\right.$ of $\left.\mathrm{NH}_{3}=4.75\right)$
Step 1
The concentrations of the base and the conjugate acid are given as $0.25 \mathrm{M}$ and $0.15 \mathrm{M}$ respectively. The $pK_{b}$ of the base is given as $4.75$. Show more…
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A buffer is prepared containing $0.25 \mathrm{M} \mathrm{NH}_{3}$ and $0.45 \mathrm{M} \mathrm{NH}_{4}+.$ Calculate the $\mathrm{pH}$ of the buffer using the $K_{\mathrm{b}}$ for $\mathrm{NH}_{3}$
Find the pH of a buffer that consists of 0.25$M \mathrm{NH}_{3}$ and 0.15$M \mathrm{NH}_{4} \mathrm{Cl}\left(\mathrm{p} K_{\mathrm{b}} \text { of } \mathrm{NH}_{3}=4.75\right) .$
A buffer is prepared containing $0.25 \mathrm{MNH}_{3}$ and $0.45 \mathrm{M}$ $\mathrm{NH}_{4}^{+} .$ Calculate the $\mathrm{pH}$ of the buffer using the $K_{\mathrm{b}}$ for $\mathrm{NH}_{3}$.
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