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What is the Ka for C3H6O3 in a titration with NaOH?
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[QUOTE="epenguin, post: 5051772, member: 106258"] I agree the question sounds garbled. However at pH 8 you [I]do[/I] know the concentration of H[SUP]+[/SUP]. The concentration of C[SUB]3[/SUB]H[SUB]6[/SUB]O[SUB]3[/SUB][SUP]-[/SUP] is for all practical purposes equal to that of Na[SUP]+[/SUP] and this is an important principle that will come up in all such calculations, surely explained in your textbook, that you will need to mentally fix. o_O If the question feels to any student weird and uncomfortable they may not be wrong as the equivalence point is a stupid place to determine a pK - the pH is changing wildly there with added base, so extremely (unnecessary!) good accuracy is being presumed here. As this all sounded screwy I calculated (check my calcs.) using [I]accurate[/I] atomic masses that 0.7993 mMoles acid were initially present, and 0.7875 mMoles of Na[SUP]+[/SUP] which is given to 4 figures, added. And is 1.5% short of equivalence. Just about makes sense. :bugeye: Actually that last figure tells me that the pK should be in the ballpark of a bit above 6. And then again with the given formula there are not many options for a structure with acid group and I do not know any hydroxyacid with pK in that ballpark. :wideeyed: [/QUOTE]
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What is the Ka for C3H6O3 in a titration with NaOH?
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