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    Quantum Titration Problems

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    Find the pH of a solution prepared by dissolving all of the following compounds in one beaker and diluting to a volume of 1.00 L: 0.180 moles acetic acid (pKa=4.75), 0.180 mole sodium acetate, 0.060 mol H2SO4, and 0.060 mol NaOH. Assume sulfuric acid dissociates completely (i.e. it is a strong acid).

    Consider the titration of 25.00 mL of a solution that contains 0.0450 M I- by a 0.150 M solution of Cu+ to form the precipitate CuI. What are the concentrations of Cu+ and I- after 10.00 mL of titrant have been added? CuI Ksp = 1.0x10-12

    As the pKa of weak acid get large (increases) the strenght of thier conjugate bases become:
    a)stronger
    b)weaker
    c)stays the same
    d)can't be compared

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    Solution Preview

    Find the pH of a solution prepared by dissolving all of the following compounds in one beaker and diluting to a volume of 1.00 L: 0.180 moles acetic acid (pKa=4.75), 0.180 mole sodium acetate, 0.060 mol H2SO4, and 0.060 mol NaOH. Assume sulfuric acid dissociates completely (i.e. it is a strong acid).

    H2SO4 and NaOH will neutralize;
    H+ + OH- ←→ H2O
    Initial 0.12 mol 0.06 Note: mole H+ = 0.06 (2) since H2SO4 is diprotic ...

    Solution Summary

    The pH of a solution prepares by dissolving all compounds in one beaker and diluting to a volume are determined. The concentration of Cu+ and I- are also determined.

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