Re: solubility
- From: Bob <bbx107@xxxxxxxxxxxxxxx>
- Date: Sat, 25 Jun 2005 18:25:21 -0700
On Sat, 25 Jun 2005 19:01:57 GMT, "John Doe III"
<john_doeIII@xxxxxxxxx> wrote:
>
>>>A 2N concentration of H2SO4 that is completely dissolved would be expected
>
>> Because you have mis-interpreted the question. You (below) are
>> calculating the total concentration of all ions. The question asks for
>> the concentration of the sulfuric acid. That may not be explicit, but
>> it is certainly implicit from common usage. Careful about
>> over-interpreting questions!
>
>Thanks so much. I thought "completely dissolved" means all ions are
>separated.
It might mean that (assuming the solute is a strong electrolyte). But
it still does not matter.
I suppose it is basically a matter of convention that molarity (and
such) refer to the conc of the chemical you add, not to the total conc
of ions (unless the latter is clearly specified).
For example, osmotic properties depend on the total conc of
"particles". So the "osmolarity" of the given solution would indeed be
3 M (let's assume for simplicity that it is fully ionized, though the
2nd ionization undoubtedly is incomplete.)
Note that it was possible for me to focus my answer because you had so
clearly explained what you did do. And what you did was reasonable --
it just happened to not be what was wanted here, and that is as much
chemical convention as clarity.
bob
> That's why after finding the molarity of H2SO4 I found the
>molarity of the solution when all ions are separated. I definitely
>misunderstood the question.
>
.
- References:
- solubility
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- Re: solubility
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- Re: solubility
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- solubility
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