If the ionic product of water (K_w) is 1.96 t | vedclass

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(C) The auto-ionization of water, $H_2O_{(l)} \rightleftharpoons H^+_{(aq)} + OH^-_{(aq)}$, is an endothermic process $(\Delta H > 0)$.
According

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$2.95 	imes 10^{-15}$

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(C) The auto-ionization of water, $H_2O_{(l)} ightleftharpoons H^+_{(aq)} + OH^-_{(aq)}$, is an endothermic process $(\Delta H > 0)$.
According to Le Chatelier's principle, an increase in temperature shifts the equilibrium to the right, increasing the value of the ionic product $(K_w)$.
Conversely, a decrease in temperature shifts the equilibrium to the left, decreasing the value of $K_w$.
Since the temperature is decreased from $35^{\circ} C$ to $10^{\circ} C$, the value of $K_w$ must be less than $1.96 	imes 10^{-14}$.
Among the given options, $2.95 	imes 10^{-15}$ is the only value smaller than $1.96 	imes 10^{-14}$.

If the ionic product of water $(K_w)$ is $1.96 \times 10^{-14}$ at $35^{\circ} C$, what is its value at $10^{\circ} C$?

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