Calculate the pH of a 5.0 M solution of aniline (C₆H₅NH₂; K_b = 3.8 × 10^-10). A) 9.64 B) 9.30 C) 4.36 D) -0.070 E) none of these

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The correct answer is A because the pH of a 5.0 M solution of aniline can be calculated using the Kb value of aniline and the following equation:pH = 14 - pOH = 14 - (1/2)pKb - (1/2)log[B]where [B] is the concentration of the base (aniline) in moles per liter. Substituting the given values into this equation, we get:pH = 14 - (1/2)pKb - (1/2)log[5.0 M] = 14 - (1/2)(9.64) - (1/2)(0.70) = 9.64

Calculate the PH of a 5