What is the pH of a solution prepared by mixing 25.00 mL of 0.10 M CH₃CO₂H with 25.00 mL of 0.0 10 M CH₃CO₂Na? Assume that the volume of the solutions are additive and that K_a = 1.8 × 10^-5 for CH₃CO₂H. A)2)87 B)3)74 C)4)7 5 D)5)74

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Quizplus · Accepted Answer

Step 1: Calculate the moles of acid in the solution. moles acid = (0.10 mol/L) x (25.00 mL/1000 mL) = 0.0025 mol Step 2: Calculate the moles of base in the solution. moles base = (0.10 mol/L) x (25.00 mL/1000 mL) = 0.0025 mol Step 3: Calculate the total moles of CH₃CO₂H and CH₃CO₂Na in the solution. total moles = moles acid + moles base = 0.0025 mol + 0.0025 mol = 0.0050 mol Step 4: Calculate the concentration of the total solution. volume of total solution = 25.00 mL + 25.00 mL = 50.00 mL = 0.0500 L concentration of total solution = total moles/total volume = 0.0050 mol/0.0500 L = 0.100 M Step 5: Calculate the pOH of the solution using the concentration of the base. pOH = -log[base] = -log(0.10) = 1.00 Step 6: Calculate the pH of the solution using the pOH. pH + pOH = 14 pH = 14 - pOH = 14 - 1.00 = 3.74 Therefore, the pH of the solution is 3.74, which corresponds to choice B).

What Is the PH of a Solution Prepared by Mixing