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When do I use the ICE method?

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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 method:s-smilie:So my question is how do I know when to use the ICE method?:smile:
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 method:s-smilie:So my question is how do I know when to use the ICE method?:smile:


ICE is for equilibrium, this is a buffers question.

Use ka = [H+][A-]/[HA]
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Adorable98
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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:h:

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