(C) At $37^{\circ}C$,the ionic product of water $(K_w)$ is approximately $2.4 \times 10^{-14}$.$pH = -\log[H^+]$.For a neutral solution,$[H^+] = \sqrt

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(C) At $37^{\circ}C$,the ionic product of water $(K_w)$ is approximately $2.4 \times 10^{-14}$.$pH = -\log[H^+]$.For a neutral solution,$[H^+] = \sqrt{K_w} = \sqrt{2.4 \times 10^{-14}} \approx 1.55 \times 10^{-7}$.$pH = -\log(1.55 \times 10^{-7}) \approx 6.8$.Therefore,the $pH$ of a neutral solution at human body temperature is $6.8$.