<p>Suppose that .1 liter of .5 molar HCl is added to .04L of the buffer( .5M HCH3COO, .5M CH3COO-) Compute the hydrogen ion concetration.</p>
<p>Man, my A.P. Chemistry class is just getting to acid-bases and equilibrium stuff. I'd help you out but I guess I need to self-study a little bit ahead. Sorry! Eh, I'm sure there are people on here who will answer your Q.</p>
<p>come on anyone?</p>
<p>I am not in AP chem so this is quite possibly wrong. I would do:
(.1L)(.5M HCL)= .05 mol H+ + .05 mol Cl-
(.04L)(.5 M CH3COO-)= .02 mol CH3COO-
.05-.02=.03 mol H+
(.03 mol)/(.14 L of solution)= .214 M</p>
<p>anyone, please feel free to tell me i am wrong.</p>
<p>I don't think that's right, but I could be wrong. Since it's a buffer there are some things you'll have to do which I don't really remember. Although maybe you did do them and I'm insane.</p>
<p>I worked through the problem and found 0.214M, similar to stevezilla1088.</p>
<p>One thing I find strange about the problem is the amount of HCl used. It somewhat defeats the purpose of a buffer, in my opinion.</p>
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Although maybe you did do them and I'm insane.
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<p>That's great lol.</p>