Suppose that 50.0 mL of 0.25 M CH3NH2(aq) is titrated with 0.35 M HCl(aq).
(a) What is the initial pH of the 0.25 M CH3NH2(aq)?
(b) What is the pH after the addition of 15.0 mL of 0.35 M HCl(aq)?
(c) What volume of 0.35 M HCl(aq) is required to reach halfway to the stoichiometric point?
mL
(d) Calculate the pH at the half stoichiometric point.
(e) What volume of 0.35 M HCl(aq) is required to reach the stoichiometric point?
mL
(f) Calculate the pH at the stoichiometric point.
1 answer
You work this th same way as the C6H5COOH problem EXCEPT this one is a base and not an acid. That makes the hydrolysis equation slight different.
2 answers