Chemistry

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I keep getting the last part of this question wrong.

Strong base is dissolved in 765 mL of 0.200 M weak acid (Ka = 4.63 x 10^-5) to make a buffer with a pH of 4.18. Assume that the volume remains constant when the base is added. HA(aq) + OH-(aq) -. H2O(l) + A-(aq). I found that the pKa of the acid = 4.33 and the number of moles of acid initially present is 0.153 mol HA. [A-]/[HA] = 0.71 which are correct but i can't find how many moles of strong base were initially added!

(x/0.153-x) = .71 ----> 0.128 mol of OH is incorrect

and 0.153 [which i really thought would be correct] is incorrect as well!
y = 0.71(0.153 mol - y)
y = 0.153 mol

PLEASE help me!! this problem is frustrating me

  • Chemistry -

    You're on the right track; you're using the wrong signals.
    ...........HA + OH^- ==> A^- + H2O
    initial..0.153..0.........0......0
    added...........x..................
    change.....-x...-x........x.......x
    equil...0.153-x..0.........x
    4.18 = 4.33 + log(x/153-x)
    Solve for x. I get about 0.06 but you need to do it more accurately. That makes
    acid left = 0.153-0.06 and base = 0.06.
    Check it by substituting base and acid numbers into the HH equation and make sure you get 4.18.
    Now that I look over your work again, I agree with what you've done except I used 0.708 instead of 0.71. I think you just made a math error because
    (x/0.153-x) = 0.708 is right to that point. It's the 128 that isn't right.

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