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March 29, 2017

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What is the pH of a solution that results from adding 0.054 mol Ca(OH)2 to 1.76 L of a buffer comprised of 0.33 M CH3COOH and 0.33 M CH3COONa?

I'm not sure how to start this. Thanks!

  • Chemistry - ,

    mols CH3COOH (HAc) = M x L = 0.581
    mols CH3COONa (NaAc) = 0.581

    .......HAc + OH^- ==> Ac^- + H2O
    I......0.581..0......0.581........
    add.........2*0.054...............
    C.....-1.08..-1.08..+1.08
    E.....0.499..0.......1.66

    Substitute the E line into the Henderson-Hasselbalch equation and solve for pH.

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