The ionic product of water is at 25°C. Assuming the density of water independent from change in temp — Ionic Equilibrium Chemistry Question

💡 Solution & Explanation

The self-ionization of water is an endothermic process. As the temperature increases from 25°C to 50°C, the equilibrium shifts forward, which increases the ionic product ($K_w$). Therefore, $K_w$ must be greater than $1.0 \times 10^{-14}$. Among the given options, only $5.9 \times 10^{-14}$ represents a biologically and chemically realistic increase in $K_w$ for this temperature shift.