Calculate the pH of a 1.00 L solution of 0.100 M NH₃(aq) after the addition of 0.010 mol NH₄Cl(s). For NH₃, pKb = 4.74. A) 10.26 B) 9.26 C) 8.26 D) 11.56

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Quizplus · Accepted Answer

The addition of NH4Cl to NH3 will form a buffer solution. The pH of the buffer can be calculated using the Henderson-Hasselbalch equation:pH = pKb + log([NH3]/[NH4+])We know that pKb = 4.74 and [NH3] = 0.100 M. We can calculate [NH4+] using the following equation:[NH4+] = [NH4Cl] / Vwhere [NH4Cl] is the concentration of NH4Cl in moles per liter and V is the volume of the solution in liters. In this case, [NH4Cl] = 0.010 mol / 1.00 L = 0.010 M. Therefore, [NH4+] = 0.010 M.Now we can plug these values into the Henderson-Hasselbalch equation to calculate the pH:pH = 4.74 + log(0.100 / 0.010) = 10.26Therefore, the correct answer is A.

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