When [H⁺] = 1.0 $\times$ 10^-7 M in water at 25 $\circ$ C, then ________

Question

Quizplus · Accepted Answer

The pH of the solution can be calculated using the formula: pH = -log[H+]. Since [H+] is not given in the question, we need to use the relationship: [H+][OH-] = Kw, where Kw is the ion product constant of water (1.0 x 10^-14 at 25°C). Rearranging this equation gives: [OH-] = Kw/[H+]. Substituting the given values in this equation gives: [OH-] = (1.0 x 10^-14)/((1.0 x 10^-1) x (1.0 x 10^-10)) = 1.0 x 10^-4. Taking the negative logarithm of this value gives the pOH of the solution: pOH = -log[OH-] = -log(1.0 x 10^-4) = 4. Finally, the pH can be found by subtracting the pOH from 14: pH = 14 - pOH = 10. Therefore, the correct answer is C.

When [H+] = 1 ×\times× 10-7 M in Water at 25 ∘\circ∘

When [H⁺] = 1 $\times$ 10^-7 M in Water at 25^$\circ$