Asked by Reen
what mass of sodium acetate should be dissolved in 1.00L of acetic acid, 0.150M concentration, in order to produce a buffer with pH = 4.5?. Ka of CH3COOH = 1.8x10^-5
Answers
Answered by
DrBob222
Use the Henderson-Hasselbalch equation.
pH = pKa + log (base/acid)
Plug in pH needed, pKa for acetic acid, (HAc) for acid in the log term, and solve for base (acetate). That will be the concn of sodium acetate. For 1 L in the problem, that = moles and mols = grams/molar mass. Solve for grams.
pH = pKa + log (base/acid)
Plug in pH needed, pKa for acetic acid, (HAc) for acid in the log term, and solve for base (acetate). That will be the concn of sodium acetate. For 1 L in the problem, that = moles and mols = grams/molar mass. Solve for grams.
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