What is the pH of a solution with a [ ^- OH] of 1.0 *10 ^- ¹⁰ M? A) "1.0 *10 ^- ¹⁰" B) "10.0" C) "4.00" D) "-10.0" E) "-4.00"

Question

Quizplus · Accepted Answer

The given chemical formula does not provide any information about the pH of the solution. Only the concentration of each ion is given. To calculate the pH, we need to use the formula: pH = -log[H+], where [H+] is the concentration of hydrogen ions in the solution. We can calculate [H+] by using the equation for the dissociation of water: H2O ↔ H+ + OH-. At room temperature, the concentration of H+ and OH- ions in pure water is 1.0 x 10^-7 M. Since the solution given in the question is not pure water, we need to use the ion concentration to calculate the concentration of H+ ions. According to the formula given in the question, the concentration of OH- ions is 1.0 x 10^-4 M. So, [H+] = Kw / [OH-] = 1.0 x 10^-14 / 1.0 x 10^-4 = 1.0 x 10^-10 M. Therefore, pH = -log(1.0 x 10^-10) = 10 + log(1.0 x 10^-10) = 10 - 10 = 4.00. Hence, the correct answer is C.

What Is the PH of a Solution with a [