The pK_a of a weak acid is 4.8. What should b | vedclass

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(B) The Henderson-Hasselbalch equation for an acidic buffer is given by:$pH = pK_a + \log \frac{[Salt]}{[Acid]}$Given $pH = 5.8$ and $pK_a = 4.8$,subs

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$0.1$

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(B) The Henderson-Hasselbalch equation for an acidic buffer is given by:$pH = pK_a + \log \frac{[Salt]}{[Acid]}$Given $pH = 5.8$ and $pK_a = 4.8$,substitute these values into the equation:$5.8 = 4.8 + \log \frac{[Salt]}{[Acid]}$Rearranging the equation:$\log \frac{[Salt]}{[Acid]} = 5.8 - 4.8 = 1.0$Taking the antilog on both sides:$\frac{[Salt]}{[Acid]} = 10^1 = 10$We need the ratio of $[Acid]/[Salt]$:$\frac{[Acid]}{[Salt]} = \frac{1}{10} = 0.1$

The $pK_a$ of a weak acid is $4.8$. What should be the ratio of $[Acid]/[Salt]$ of a buffer if $pH = 5.8$ is required?

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