Calculate the pH of a solution that is 0.20M NH₃(aq) and 0.35 M NH₄Cl(aq).(K_b(NH₃) = 1.8 x 10^-5)

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The correct answer is A because the pH of a solution that is 0.20M NH3(aq) and 0.35 M NH4Cl(aq) is 9.01. This can be calculated using the Henderson-Hasselbalch equation: pH = pKa + log([A-]/[HA]), where pKa is the dissociation constant of the weak acid, [A-] is the concentration of the conjugate base, and [HA] is the concentration of the weak acid. In this case, the weak acid is NH4+ and the conjugate base is NH3. The pKa of NH4+ is 9.25, so the pH of the solution is 9.01.

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