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I have a question that reads, "What is the pH of a 0.01M (10mM) solution of arginine that has a net charge of -.65?"

I tried using the henderson hasselbach equation, since I know the pka of arginine is 12.48.

So I got pH=12.48+log(b/a)

Since the net charge was -.65, I thought the concentration of base was therefore .65 (and since a+b=1), the acid concentration was .35.

My final answer was 12.75, but I'm not sure if my steps/reasoning are correct.

  • Chemistry -

    Your answer is correct.

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