Hey there! My professor wrote this vague problem on the boardand I can't figure out how to solve it so --- I apologize inadvance for any lack of clarity.
50.0 mL of 0.03M of Cysteine is titrated by 0.06M of NaOH
pKa 2= 8.37
pKa 1 = 1.92
What is the pH of the solution.....
1) Before any titrant is added
2) 12.5 mL of NaOH
3) 25.0 mL of NaOH
4) 37.5 mL of NaOH
5) 50.0 mL of NaOH
6) 60.0 mL of NaOH
I really want to understand this type of problem for exams inthe future so any explanation to go along with your work would besuper appreciated. Thank you!!
