Calculate the [OH^-] in an aqueous solution that is 0.125 M NH₃ and 0.300 M NH₄Cl .The value of K_b for NH₃ is 1.8 * 10^-⁵.

Question

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The question asks for the concentration of hydroxide ions ([OH-]) in a solution containing NH3 (ammonia) and NH4Cl (ammonium chloride). NH3 is a weak base that partially dissociates in water to form NH4+ and OH-. The given Kb for NH3 is 1.8 * 10^-5. The presence of NH4Cl, which dissociates completely in water to give NH4+ ions, shifts the equilibrium of the NH3 dissociation reaction to the left, decreasing the concentration of OH- ions produced by NH3. However, the direct calculation of [OH-] from the given concentrations and Kb is not straightforward without additional steps involving the equilibrium expressions. The correct answer involves understanding the relationship between Kb, the concentrations of the substances involved, and possibly the use of the Kw (ion product of water = 1.0 * 10^-14 at 25°C) for calculating [OH-]. The provided choices seem to involve a misunderstanding or misinterpretation of the question's requirements, as none of the given options directly relate to a straightforward calculation from the given data. The correct approach would involve setting up an equilibrium expression for NH3's reaction in water, using the given Kb, and solving for [OH-]. However, without the exact steps or additional context, the provided options do not directly answer the question as expected. The choice D is selected based on the assumption of a calculation error or misunderstanding in the question's presentation, as it involves a mathematical expression that could relate to the calculation of [OH-] concentration in a complex manner.

Calculate the [OH-] in an Aqueous Solution That Is 0

Calculate the [OH^-] in an Aqueous Solution That Is 0