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Analytical Chemistry

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Need help with question. Calculate the pH of a buffer prepared by adding 100mL of 0.0500M NaOH to 100mL of 0.175M CH3COOH.

so far I have calculated mols of
CH3COOH---->H+ + CH3OO-

Not sure were to go from here, or if the above is right

  • Analytical Chemistry - ,

    Millimoles is a little easier to work with in these problems; it keeps all those leading zeros out of the way.
    100 mL x 0.175M CH3COOH = 17.5 mmoles.
    100 mL x 0.05M NaOH = 5 mmoles.

    .......NaOH + CH3COOH ==> CH3COONa + H2O

    So you have CH3COOH and CH3COONa (a weak acid and its salt which gives you a buffer). Use the Henderson-Hasselbalch equation to solve for pH. I get about 4.3 or so but you need to do it more accurately.
    pH = pKa + log[(acetate)/(acid)]

  • Analytical Chemistry - ,

    How do i solve if i am not aloud to use henderson-hasselbach?

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