(Photo of the analyte at what was meant to be the equivalence point, but we put in too much NaOH)
(Photo of the setup/materials of the lab)
The procedure of this lab was to fill up the burette with NaOH, and then drop the NaOH slowly into a flask that had a magnetic stir bar inside of it (we activated it by using the hot plate's stir function, it was cool), as well as 6-8mL of vinegar with 3-5 drops of phenolphthalein dispersed in it. The reason why we did this was to see if we could reach the equivalence point. If we couldn't, we'd have to do the procedure over again. We never got the exact molarity, which was 0.83M, from the lab in any of our three trials, but the last one was the closest, at a solid 0.85M. The percent ionization was found by dividing our average H3O+ concentration, which was 0.81M, by the average concentration for NaOH, which was 0.04M. This resulted in a .49% ionization, and the reson this number is so low is because acetic acid is a weak acid, so they don't ionize because they don't disassociate well.
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