Question

I have to finish a lab report in which we conducted an experiment with NaOH and an unknown acid. Essentially we added varying amounts of NaOH (from 2.5mL up to 30.00mL and a certain amount of deionized water) to an unchanging volume of unknown acid (10mL). While doing these reactions we calculated the change in temperature from before and after the reaction. I'm confused as to how to determine if the acid is monoprotic or diprotic from this information. Online I was only able to find how to determine with pH not temperature.

Answer 1

As per your description, I understand that you took a const. volume of acid and you were adding NaOH while calculatoroing the conductance. Let HA is our unknown aced : HA + Naohs Natt tiot A-. Thus the more conducting Ht is consumed to farm water, so, un conductance decreases tul and pornt. And beyond end point the conductance increasis due to excess oH In case of a deprotonie acid, one of proton is strongly acidic anottier is weally acidic Wan when the more acdic proton is removed, the conductance decreases due to the previous explanation but when it gets completed, less acedic proton is removed, and due to La-chatevers principle the more less acidic proton get ionised due to the consumtion and the conductance increases in a very slow rate. After end point the conductance aleruptly increases due to excess of from the plot we can clearly make them dyferent.

for monobasic acid, the plot will be End point . and far no. of drops of Noor dibasic acid : I SA mo. of drops of Noot.