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The value of the ion product constant for water, \( \left(K_{w}\right) \) at \( 60^{\circ} \mathrm{C} \) is \( 9.6 \times 10^{-14} \mathrm{M}^{2} \). What is the \( \left[\mathrm{H}_{3} \mathrm{O}^{+}\right] \)of a neutral aqueous solution at \( 60^{\circ} \mathrm{C} \) and an aqueous solution with a pH \( =7.0 \) at \( 60^{\circ} \mathrm{C} \) are respectively?
(a) \( 3.1 \times 10^{-8} \), acidic
(b) \( 3.1 \times 10^{-7} \), neutral
(c) \( 3.1 \times 10^{-8} \), basic
(d) \( 3.1 \times 10^{-7} \), basic
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