Asked by Dana
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.
(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.
Answers
Answered by
DrBob222
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.
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