What is the pH of a buffer solution that is 0.295 mol L^-1 in hypochlorous acid (HClO)and 0.373 mol L^-1 in sodium hypochlorite (NaClO)? The $K _ { a }$ of hypochlorous acid is 3.8 × $10 ^ { - 8 }$ . A)13.04 B)8.38 C)7.32 D)6.48 E)7.52

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The pH of a buffer solution can be calculated using the Henderson-Hasselbalch equation:$$pH = pK_a + log\frac{[A^-]}{[HA]}$$where $pK_a$ is the negative logarithm of the acid dissociation constant, [A^-] is the concentration of the conjugate base, and [HA] is the concentration of the acid.In this case, the acid is hypochlorous acid (HClO) and the conjugate base is sodium hypochlorite (NaClO). The $pK_a$ of hypochlorous acid is 3.8 × $10 ^ { - 8 }$.Substituting the given concentrations into the Henderson-Hasselbalch equation, we get:$$pH = 3.8 + log\frac{0.373}{0.295} = 7.52$$Therefore, the pH of the buffer solution is 7.52.

What Is the PH of a Buffer Solution That Is KaK _ { a }Ka​

What Is the PH of a Buffer Solution That Is $K _ { a }$