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Consider the titration of 100.0 mL of 0.110 M NaOH with 1.00 M HBr. Find the pH at the following volumes of acid added and make a graph of pH versus Va:Va = 0,2,5,8,10,10.1,11,11.1, and 12mL. Compute Ve, first.

  • Analy Chem -

    Find mols NaOH, subtract mols HBr.
    If mols NaOH are greater then pOH = -log(OH^-) and convert to pH by
    pH + pOH = pKw = 14.
    If mols HBr are in excess, pH = -log(H^+).
    Those three steps will do all of the points except for the equivalence point. That one is done by the hydrolysis of the salt, NaBr, which is 7 at the equivalence point.

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