What is the pOH of a 0.125 M solution of hydroxylamine? The K_b value for hydroxylamine is 1.1 $\times$ 10^-8.

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Quizplus · Accepted Answer

The pOH of a solution can be calculated using the formula:pOH = -log[OH-]where [OH-] is the hydroxide ion concentration in moles per liter.The hydroxide ion concentration can be calculated using the Kb value for the base and the concentration of the base:Kb = [OH-]^2 / [B]where Kb is the base dissociation constant, [OH-] is the hydroxide ion concentration, and [B] is the base concentration.For hydroxylamine, Kb = 1.1 x 10^-8 and [B] = 0.125 M. Substituting these values into the equation, we get:1.1 x 10^-8 = [OH-]^2 / 0.125Solving for [OH-], we get:[OH-] = 1.05 x 10^-4 MNow we can calculate the pOH:pOH = -log[OH-] = -log(1.05 x 10^-4) = 3.98Therefore, the pOH of a 0.125 M solution of hydroxylamine is 3.98, which is closest to choice A, 4.43.

What Is the POH of a 0 ×\times× 10-8

What Is the POH of a 0 $\times$ 10^-8