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

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

Options:

  1. 4.76
  2. 7.00
  3. 9.24
  4. 10.00

Correct Answer: 9.24

Solution: 

Sodium acetate is a salt of a weak acid (acetic acid) and a strong base (sodium hydroxide). The pH can be calculated using the formula pH = 7 + 0.5(pKa - log[C]), where pKa of acetic acid is 4.76.

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

Practice Questions

Q1
What is the pH of a 0.01 M solution of sodium acetate (CH3COONa)?
  1. 4.76
  2. 7.00
  3. 9.24
  4. 10.00

Questions & Step-by-Step Solutions

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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