Chemistry

posted by Shana

A 30.00mL sample of 0.150M KOH is titrated with 0.125M HClO4 solution. Calculate the pH after the following volumes of acid have been added: 30.0 mL, 35.0 mL, 36.0 mL, 37.0 mL, 40.0 mL

  1. DrBob222

    This is a strong acid/strong base titration so the pH at the equivalence point will be 7.00. The first thing to do is to calculate where the equivalence point is.The following will do that.
    mL acid x M acid = mL base x M base
    mL acid x 0.125 = 30.00 x 0.150
    mL acid = ?

    Then set up an ICE chart for each addition of acid to the base. We start with how many moles of KOH? That is M x L = 0.150 x 0.0300 = .0045
    Additions of HClO4 are
    30.00 x 0.125 = 0.00375
    35.00 --- you can fill
    36.00 --- you can fill
    40.00 --- you can fill.

    ..........KOH + HClO4 ==>KClO4 + H2O
    initial..0.0045..0.........0......0
    add 30..........0.00375............
    change.-0.00375 -0.00375..+0.00375..etc
    equil....0.00075..0...0.00375..0.00375

    The ICE chart tells you what you have at this point in the titration which for 30.00 mL is a solution of KOH and KClO4 in a volume of 60.00 mL (30.00 acid _ 30.00 base).
    M KOH = moles/L = 0.00075/0.0600 = 0.0125M KOH. Then pOH = ? and obtain pH from pH + pOH = pKw = 14.
    Everything up to equilvanece point is done this way. The equivalence point, as I pointed out above has a pH of 7.00, and everything after the equivalence point done the same way EXCEPT you should note that for those points its the HClO4 in excess. Post your work if you get stuck.

  2. hannah

    I am doing similar homeowrk and I was wondering how you calculate the ph after the equivalence point?

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