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    What is the approximate pH of a buffer solution containing 0.20 mol of a weak acid, HA,(pKa = 4.8) and 0.20 mol of the sodium salt of the acid, NaA, in a total volume of 1 dm3of solution?

    I tried solving it by using logs, pH= log[H+]But then I was told to use the ICE methodSo my question is how do I know when to use the ICE method?
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    (Original post by Adorable98)
    Like for instance for this question,
    What is the approximate pH of a buffer solution containing 0.20 mol of a weak acid, HA,(pKa = 4.8) and 0.20 mol of the sodium salt of the acid, NaA, in a total volume of 1 dm3of solution?

    I tried solving it by using logs, pH= log[H+]But then I was told to use the ICE methodSo my question is how do I know when to use the ICE method?
    ICE is for equilibrium, this is a buffers question.

    Use ka = [H+][A-]/[HA]
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    (Original post by charco)
    ICE is for equilibrium, this is a buffers question.

    Use ka = [H+][A-]/[HA]
    I see.. Thaanks
 
 
 
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