What it is that gets hydrolyzed in soap? Isn't soap made by hydrolyzing fats, so technically there should be nothing left for hydrolyzing?
Where does the information about different results of titration in water and ethanol come from? I am not saying it is wrong, but good source should explain why it is so. It can be a matter of kinetics.
Hello Borek, thanks for the reply.
I am not a chemist, so take my "technical terms" with a spoon of salt. By hydrolysis of soap via addition of acid in a water solution (as part of the titration process) I meant:
-as I add (citric) acid for the neutralization of any free potassium hydroxide (which is caustic and therefore unwanted in the finished product) in soap until the indicator endpoint in an AQUAEOUS solution, the endpoint never really comes because the (citric) acid also "breaks" the soap (in this case the Potassium Cocoate bond) and keeps "moving" the endpoint due to the potassium hydroxide being continually made available by separation from the lauric acid.
Essentially in a water solution I keep "breaking" the soap until the presence of enough fatty acids lowers the pH enough that the phenolphtalein ceases to indicate pink/alkalinity. Meanwhile the productitself becomes a useless oily mess.
On the other hand, when doing it (adding citric acid) in an ethanol solution, (example 2g of soap dissolved in 50g of ethanol), no free fatty acids are liberated from their potassium bonds when I reach the endpoint, but rather only the free unbonded alkali is reacted into potassium citrate.
Learned from: ASTM procedures; D 460-91, as well as a "dumbed down" version from Scientific Soapmaking (Kevin Dunn)
I would like to understand why this is; predominantly to understand if and how I am making a safe product with no free caustic alkali in it.