1. a .1276 g sample of a monprotic acid, molar mass 1.10 x 10^2, was dissolved in 25 mL of water and titrated with .0633 M NaOH. After 10 mL if base had been added the pH was determined to be 5.27. What is the Ka for the acid?
2. calculate the ph at the equivilance point for the following titration: .20 M HCl versus .20 M methylamine. Ka of methylammonium is 2.3 x 10^-11
3. 30 mL if .10 M Ba(NO3)2 is added to 10 mL of .10 M Na2CO3 and resulting concentration in solution of Ba is .075 M CO3 is .025 M. What is the value of the reaction quotient?