Titrating an unkown acid with NaOH
info needed: NaOH molarity = 0.1 M
Volume of unkown acid being titrated = 25
Volume of NaOH needed to reach Equivalence point = 23.93 ml
the estimated value based on the color to reach the end point = 0.09792 M
The graph for the 1/4, 1/2, 3/4 is attached
I know that this is all the info needed for the problem, if you have questions leave them as a comment specifically.
I will thumbs up any answers.
Calculate the initial concentration of the unknown acid based on the volume of standardized NaOH to reach the equivalence point. Compare to the estimated value based on the color end point. Calculate Ka for the weak acid based on the pH when the acid is ¼, ½, and ¾ neutralized (ie, the ¼, ½, and the ¾ equivalence points). Average these three values and report the average Ka.