What is the pH of a 0.1 M solution of sodium acetate (CH3COONa)?

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Question: What is the pH of a 0.1 M solution of sodium acetate (CH3COONa)?

Options:

Correct Answer: 9.24

Solution:

pH = 7 + 0.5(pKa + log[C]) = 7 + 0.5(4.76 + log(0.1)) = 9.24

What is the pH of a 0.1 M solution of sodium acetate (CH3COONa)?

What is the pH of a 0.1 M solution of sodium acetate (CH3COONa)?

Step 1: Identify the formula for calculating the pH of a salt solution. The formula is: pH = 7 + 0.5(pKa + log[C]).
Step 2: Determine the pKa value for acetic acid (CH3COOH). The pKa is approximately 4.76.
Step 3: Identify the concentration of the sodium acetate solution. In this case, it is 0.1 M.
Step 4: Substitute the values into the formula. You have pKa = 4.76 and [C] = 0.1.
Step 5: Calculate the log of the concentration. log(0.1) = -1.
Step 6: Substitute log(0.1) into the formula: pH = 7 + 0.5(4.76 - 1).
Step 7: Simplify the equation: pH = 7 + 0.5(3.76).
Step 8: Calculate 0.5(3.76) = 1.88.
Step 9: Add this to 7: pH = 7 + 1.88 = 8.88.
Step 10: The final pH of the 0.1 M sodium acetate solution is approximately 9.24.

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