What is the pH of a 0.01 M solution of sodium acetate (CH3COONa)?

What is the pH of a 0.01 M solution of sodium acetate (CH3COONa)?

Correct Answer: 9.24

Step 1: Identify the components of sodium acetate (CH3COONa). It is made from acetic acid (a weak acid) and sodium hydroxide (a strong base).
Step 2: Understand that when sodium acetate dissolves in water, it will create a basic solution because it comes from a weak acid and a strong base.
Step 3: Find the pKa value of acetic acid, which is 4.76.
Step 4: Use the formula to calculate the pH: pH = 7 + 0.5(pKa - log[C]). Here, C is the concentration of the sodium acetate solution, which is 0.01 M.
Step 5: Calculate log[C]: log[0.01] = -2.
Step 6: Substitute the values into the formula: pH = 7 + 0.5(4.76 - (-2)).
Step 7: Simplify the equation: pH = 7 + 0.5(4.76 + 2) = 7 + 0.5(6.76) = 7 + 3.38.
Step 8: Final calculation gives pH = 10.38.

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