Statement A: pH of a buffer increases with in | vedclass

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(B) The dissociation of water is an endothermic process. Therefore,as temperature increases,the ionic product of water $(K_W)$ increases. Conversely,a

Vedclass · Accepted Answer

Both $A$ and $B$ are correct.

Vedclass · Answer

(B) The dissociation of water is an endothermic process. Therefore,as temperature increases,the ionic product of water $(K_W)$ increases. Conversely,as temperature decreases,$K_W$ decreases. Thus,Statement $B$ is correct.For a buffer solution,the $pH$ is given by the Henderson-Hasselbalch equation: $pH = pK_a + \log(\frac{[Salt]}{[Acid]})$. As temperature increases,the $pK_a$ value generally decreases,leading to an increase in the $pH$ of the buffer solution. Thus,Statement $A$ is also correct.

Statement $A$: $pH$ of a buffer increases with increasing temperature. Statement $B$: The value of $K_W$ of water decreases with decreasing temperature.

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