Final answer:
To find the pH of the solution, calculate the hydronium ion concentration by using the ion-product constant of water and then take the negative logarithm of that concentration. Given that the hydroxide concentration is significantly higher than normal, it indicates a basic solution, but exact pH value calculation requires logarithmic computation.
We find the solution to be basic.
Step-by-step explanation:
To calculate the pH of a solution with a given hydroxide ion concentration ([OH-]), we must first understand the relationship between hydroxide ions and hydronium ions ([H3O+]) in solution. The concentrations of these ions are related through the equation:
Kw = [H3O+][OH-] = 1.0 × 10-14 at 25°C
Given that [OH-] = 3.7 × 10-3 M, we can solve for [H3O+] as follows:
[H3O+] = Kw / [OH-] = (1.0 × 10-14) / (3.7 × 10-3)
Now we find the pH:
pH = -log[H3O+]
Using the calculated [H3O+] we can determine the pH. If the pH is less than 7, the solution is considered acidic; if it is greater than 7, it is considered basic; if it is exactly 7, it is neutral.
In this case, since the [OH-] concentration is significantly higher than 1 × 10-7 M, we can expect the solution to be basic.