Answer :
Final answer:
The pH of a 1.69 M Ba(OH)2 solution is 13.228.
Explanation:
The pH of a solution can be calculated using the following formula: pH = 14.00 - pOH. In the case of a 1.69 M Ba(OH)2 solution, the pOH can be determined by taking the negative logarithm of the hydroxide ion concentration. In this case, the hydroxide ion concentration is 1.69 M, so pOH = -log(1.69) = 0.771.
Substituting the value of pOH into the pH formula, we get pH = 14.00 - 0.771 = 13.229. Rounded to three decimal places, the pH of the solution is 13.228.
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