Chemical Forums
Chemistry Forums for Students => Analytical Chemistry Forum => Topic started by: Xenonman on April 08, 2014, 10:14:45 PM
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Hello all ;D
I just figured how annoying normality is. To get the full picture, I want to gather the names of as many solutions that have the same molarity, but different normality depending on the reaction they are used.
So far, I could think of Fe+3 ion, which could react to form either Fe+2 or Fe(s), thus having at least two normalities and one molarity. Same with copper.
The other one is H2Y-2: One could treat is as an usual acid or base (two acid/base sites per molecule), or use it for a typical complexometric titration (one complex is formed by one molecule). This gives at least two normalities and one molarity.
But I am sure there are examples I can't even think of. That's when all of you come in.
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H2SO4 (acid/base, BaSO4 precipitation).
Pb2+ (precipitation of chloride, precipitation of sulfate)
MnO4- (three different values for oxidations in acidic, neutral and basic solutions)
And so on.
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H2SO4 (acid/base, BaSO4 precipitation).
I was taught sulphuric has two acid sites, and gets its two protons removed by bases and Ba2+, so its normality should be the same for both reactions.
Pb2+ (precipitation of chloride, precipitation of sulfate)
Same thing here. Different stoichiometry, but same amount of positive charges and thus same normality.
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Xenonman:, you've made the same mistake twice in both postings. Just because sthe sulfate ion is 2-, doesn't mean it interacts twice, the same as two H+. Likewise, the Fe2+ and Fe3+ don't enter into discussions of normality and molarity.
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Back from the dead.
As far as I understand, IUPAC mentions the viability of using equivalents for solutions part of redox reactions. Here: http://goldbook.iupac.org/E02192.html (http://goldbook.iupac.org/E02192.html).
And since equivalents are viable, and normality relies on equivalents, normality for redox should be a valid and archaic way of expressing concentration.