Final answer:ThepOHof a 0.0085 M KOH solution is 2.07. This is computed using the formula pOH = -log[OH-], where [OH-] is the hydroxide ion concentration in the solution.Explanation:To solve for the pOH of a 0.0085 M KOH solution, you first need toacknowledgethat KOH is a strong base that dissociates completely in water to produce hydroxide ions (OH-) and potassium ions (K+). As such, the hydroxide ion concentration in this solution equals the initial concentration of KOH, which is 0.0085 M.Next, compute for pOH using the formula pOH = -log[OH-], where [OH-] is the hydroxide ion concentration. Upon substituting 0.0085 for [OH-], you get:pOH = - log(0.0085) = 2.07Hence, out of the given options, the correct answer is A) 2.07.Learn more about pOH calculation here:brainly.com/question/23227189#SPJ11...

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