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The Ionic Product of Water, \({K_{\rm{w}}}\) , is the equilibrium constant for the reaction in which water undergoes an acid-base reaction with itself.

\({K_{\rm{w}}} = \left[ {{H_3}{O^ + }_{(aq)}} \right]\left[ {O{H^ - }_{(aq)}} \right] = {10^{ - 14}}at25{}^oC\)

The value of \({K_{\rm{w}}}\) increases almost 75 times when temperature is increased from 0°C to 100°C .
If the \({K_{\rm{w}}}\) is  \(0.11 \times {10^{ - 14}}mo{l^2}d{m^{ - 6}}\) at 0°C . What would be the value of \({K_{\rm{w}}}\) at 100°C?

Explanation

As the value of \({K_{\rm{w}}}\) increases almost 75 times when temperature is increased from 0°C to 100°C. If value of \(K_{\mathrm{w}}\) is \(0.11 \times 10^{-14} \mathrm{~mol}^{2} d m^{-6}\) at 0°C, it would be \(0.11 \times 10^{-14} \times 75\)when temperature is increased 75 times i.e, at 100°C.
Supplement: \(0.11 \times \$75 \sim \$ 8.25\)

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