Jul 8, 2015
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What is the molarity of a solution of H2SO4 if 100 ml of this solution requires 25 mL of 2 M NaOH for complete neutralization?

Isn't this N1V1=N2V2?

I thought it was 1.0 M but its .25 M
 
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510586

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Dec 24, 2014
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You can do it this way because NaOH is a strong base, so you can assume it dissociates 100%.
H2SO4 is a strong acid you have to assume the it also dissociates 100% twice.
You still do 2 N but I'm not sure if it dissociates 100% the second time.
 

510586

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Yeah, in the real world you know the second H doesn't dissociate 100% but i guess in terms of the DAT you would have to assume it does.
Oh ok just checking thanks. On a pH problem they could potentially ask it like that right? Then we would treat the second H as not a complete [H+] right?
 

clutchfans

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Feb 28, 2014
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Oh ok just checking thanks. On a pH problem they could potentially ask it like that right? Then we would treat the second H as not a complete [H+] right?
That's a really good question. I think if its a strong acid, you can assume this. If it isn't a strong acid you can't assume this.
If you have a specific question, I think it would be best to ask Dr. Romano.
Also, if they don't give you any pKa's or Ka's, your going to have to assume it dissociates twice.
 

510586

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Dec 24, 2014
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If you have DAT destroyer, I'm sure there are a few questions like this.
I do, but I don't recall a question involving the pH of a diprotic other than like Ba(OH)2. But I think they treated it as a total OH. Should be the same type of approach though right?
 
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