Post a New Question

organic chemistry

posted by .

A solution of acetic acid (CH3COOH; Ka = 1.74 x 10-5) was titrated to a final pH of 4.76 by using NaOH solution. What % of acetic acid is converted to sodium acetate (CH3COO-Na+)? Show your method

  • organic chemistry -

    If this were a real organic question I probably could not answer it; however, it looks like a good analytical question to me.
    Use the Henderson-Hasselbalch equation.
    pH = pKa + log (base/acid)
    pKa = -log(Ka) = 4.76
    4.76 = 4.76 + log (base/acid)
    Solve for (base/acid). You should get 1 which means the acid was half neutralized.
    You can prove this by writing the equation and assuming a number for acetic acid.
    CH3COOH + NaOH ==>CH3COONa + H2O
    Start with 10 mmoles CH3COOH
    Add 5 mmols NaOH.

    CH3COOH left = 10-5= 5 mmoles
    NaOH left = 0
    CH3COONa formed = 5 mmoles
    H2O formed = 5 mmoles

    You started with 10 mmoles CH3COOH and you have formed 5 mmoles CH3COONa.
    %CH3COONa formed = 5/10*100 = 50%

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

More Related Questions

Post a New Question