CH3NH2 is a weak base (Kb = 5.0 × 10–4) and so the salt,
CH3NH3NO3, acts as a weak acid. What is the pH of a solution that
is 0.0490 M in CH3NH3NO3 at 25 °C?
In the titration of a 25.00 mL of 0.245 M weak base (Kb= 1.0
*10^-4) being titrated by 0.365 M HCl determinethe initial pH, the
pH after 12.3 mL of HCl has been added, the pH at equivalence
point, and the pH after 22.4 mL of HCl has been reached.
Please explain! I'm having a hard time with these type of
questions.
Consider the titration of 60.0 mL of 0.0400 M C6H5NH2 (a weak
base; Kb = 4.30e-10) with 0.100 M HCl. Calculate the pH after the
following volumes of titrant have been added: a) 45.6 mL