Final answer:
The [OH-] of the solution is 1.02 x 10^-2 M, the pOH is 2, and the pH is 12. These values are calculated using the ion-product constant for water (Kw) and the known concentration of H+ ions in the solution.
Step-by-step explanation:
To determine the hydroxide ion concentration ([OH-]), pH, and pOH of a solution with [H+] of 9.8 × 10⁻¹³ M at 25 °C, we can use the ion-product constant for water (Kw) at this temperature, which is 1.0 × 10⁻. First, calculate the [OH-] using the following formula:
Kw = [H+][OH-]
The hydroxide ion concentration is:
[OH-] = Kw / [H+] = (1.0 × 10⁻) / (9.8 × 10⁻) = 1.02 × 10⁻² M
Next, calculate the pOH and the pH using the formulas:
pOH = -log [OH-]
pH = 14.00 - pOH
By substituting the calculated [OH-], we get:
pOH = -log (1.02 × 10⁻²) = 2
pH = 14.00 - pOH = 14.00 - 2 = 12
Note that we approximate pOH and pH to two significant figures based on the provided concentration of H+.