Question

At 22°C, an excess amount of generic metal hydroxide M(OH)2 is mixed with pure water. The resulting equilibrium solution has a pH of 10.26. What is the concentration of hydroxide ions (OH⁻) in the solution?

Answer 1

The concentration of hydroxide ions in a solution at pH 10.26 is approximately 1.82 × 10-4 M, calculated through the inverse exponential function of the pOH, which was found by subtracting the pH from 14.

Step-by-step explanation:

To determine the concentration of hydroxide ions (OH-) at a pH of 10.26, we first need to calculate the pOH. The pH and pOH of a solution add up to 14.00. Therefore, we calculate the pOH as:

pOH = 14.00 - pH = 14.00 - 10.26 = 3.74

Now, using the relationship between pOH and the hydroxide ion concentration, which is pOH = -log[OH-], we can find the OH- concentration:

[OH-] = 10-pOH = 10-3.74

Thus, the concentration of hydroxide ions is:

[OH-] ≈ 1.82 × 10-4 M.