I started by calculating the concentrations of the KOH solution. You can get it from the reaction with H2SO4. By determining the amount of H30+ ions (in moles) in the H2SO4 solution you know how many moles (of KOH) the 14.2ml solution of KOH contains. (H2SO4 is a diprotic acid, H2SO4 -> HSO4-. HSO4- <-> SO4(2-) )
I'm not quite sure about this latter part, but here goes:
After you know the concentration and the volume of the KOH solution, you know how many moles it takes to neutralize the "unknown acid".
And this is where I probably did something wrong:
I assumed that the acid is a strong, monoprotic one. Otherwise I don't know how I would have calculated how many moles of acid there was in the solution.
Once you get how many moles of acid there was in the solution, you know
enough to calculate the molecular mass of it.
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