AIIMS 2017 Chemistry Hydrolysis MCQ Question

Option B correctly calculates the value of $h$ using the hydrolysis constant $K_h$. The formula $h = \frac{\sqrt{K_h}}{1 + \sqrt{K_h}}$ is applied here, where $K_h$ is derived from the provided values, resulting in $h \approx 0.51$.

Option A miscalculates $K_h$ by not correctly applying the values, leading to an incorrect result. Option C uses an inaccurate $pK_a$ and misapplies logarithmic properties, resulting in an incorrect pH calculation. Understanding hydrolysis constants and their relationship to equilibrium concentrations is crucial for accurately determining $h$ and pH in aqueous solutions.