jazzie14
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#1
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In this practical you are titrating an equilibrium mixture of acid+base=salt+water (sulphuric acid catalyst) with NaOH. Basically, say you calculated the moles of NaOH needed to neutralize all of the acid in the equilibrium mixture to be .006. Why is the moles of NaOH also equal to the moles of H+ ions in the of equilibrium mixture? Equilibrium mixture is acid+alcohol=ester+water, with sulphuric acid catalyst. so there's more than 1 acid. Also, in this situation, am i correct in assuming that the MOLES of H+ ions is not the same thing as the concentration of them.
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Borek
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#2
Report 7 years ago
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(Original post by jazzie14)
In this practical you are titrating an equilibrium mixture of acid+base=salt+water (sulphuric acid catalyst)
Equilibrium mixture is acid+alcohol=ester+water, with sulphuric acid catalyst.
So, what is titrated, and what is the question again?
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