Final answer:
The pH of a solution with [OH]- = 4.7 x 10⁻⁶ M is 8.67, indicating it is a basic solution.
Step-by-step explanation:
The question is asking to calculate the pH of a solution given its hydroxide ion concentration ([OH]-) which is 4.7 x 10⁻⁶ M. To find the pH, we first determine the pOH by taking the negative logarithm of the hydroxide ion concentration. Thus, the pOH is calculated as follows:
pOH = -log(4.7 x 10⁻⁶) ≈ 5.33
Since pH + pOH = 14 (at 25°C), we can find the pH by subtracting the pOH from 14:
pH = 14 - pOH ≈ 14 - 5.33 = 8.67
Therefore, the pH of the solution is 8.67, which indicates that the solution is basic because a pH greater than 7 is characteristic of basic solutions.