At 298 K,the pH of a NaCl solution is 7. If | vedclass

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(A) The dissociation of water is an endothermic process: $H_2O(l) \rightleftharpoons H^+(aq) + OH^-(aq)$.As temperature increases,the equilibrium cons

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$pH$ will decrease

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(A) The dissociation of water is an endothermic process: $H_2O(l) \rightleftharpoons H^+(aq) + OH^-(aq)$.As temperature increases,the equilibrium constant for the dissociation of water $(K_w)$ increases.At $298 \ K$,$K_w = 10^{-14}$,so $pH = 7$.At $320 \ K$,$K_w > 10^{-14}$,which means $[H^+]$ and $[OH^-]$ both increase.Since $pH = -\log[H^+]$,an increase in $[H^+]$ leads to a decrease in $pH$.Similarly,$pOH = -\log[OH^-]$,so an increase in $[OH^-]$ leads to a decrease in $pOH$.Therefore,the $pH$ of the neutral solution decreases at higher temperatures.

At $298 \ K$,the $pH$ of a $NaCl$ solution is $7$. If the solution is heated to $320 \ K$,which of the following statements is correct?

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