what is the result of using 75g of dihydronoxybutanedioric acid in one liter of H2O in a titration?
I do not have a answer.
I don't know what this compound is and google doesn't either. Check for typos.
2,3-Dihydroxybutanedioic is tartaric acid
HOOCCH(OH)CH(OH)COOH
MOL WT> 150.09
What is the result of using 75g of this tartaric acid in one liter as a titration.
I am not told what the one liter solution is for the titration.
Not much to go on. No details about titrating what. The only quick thing that comes to mind is that tartaric acid is a diprotic acid which means it will take TWO mols of base to neutralize it instead of just one.
Also, when I typed your second post (without the typo with the extra n) google did tell me it was tartaric acid.
To determine the result of using 75g of dihydronoxybutanedioric acid in one liter of H2O in a titration, we need some additional information. Specifically, we need the concentration of the acid solution and the titrant being used in the titration.
Once we have the concentration of the acid solution and the titrant, we can calculate the amount of titrant required to reach the equivalence point. This can be done using the stoichiometry of the reaction involved in the titration.
However, without knowing the specific titrant and its concentration, it is not possible to determine the result of the titration. I would recommend providing more information about the titration setup to get a more accurate answer.