Answer :
Final answer:
The pH of a 0.023 M Ba(OH)2 solution at 25°C is 12.66.
Explanation:
The pH of a solution can be calculated by using the formula pH = -log[H+]. However, in the case of Ba(OH)2, which is a strong base, it will dissociate completely in water to form 2 moles of OH- ions. The concentration of OH- ions in the solution will thus be 2 * 0.023 M = 0.046 M. We can then calculate the pOH of the solution using the formula pOH = -log[OH-]. Therefore, pOH = -log(0.046) = 1.34. At 25°C, the sum of pH and pOH is equal to 14, so the pH of the 0.023 M Ba(OH)2 solution is 14 - 1.34 = 12.66.
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