A solid weak acid is weighed, dissolved in water and dilutedto exactly 50.0 ml.25.00ml of the solution is taken out and is titrated to aneutral endpoint with 0.10 M NaOH. The titrated portion isthen mixed with the remaining untitrated portion and the pH ofthe mixture is measured.
Mass of acid weighed out (grams) 0.633
Volume of NaOH required to reach endpoint: (ml) 19.1
pH of the mixture (half neutralized solution) 3.26
Calculate the following
1) What is the pKa of the acid?I know that I'll need to find Ka whichis = ([H+][[A-])/ [HA] but other than that i'm not sure how tostart
2) What is the molarity ofthe original acid solution
3) What is the molecular weight of the acid?