Question

What is the pH when 20 mL of a 0.01 M solution of ethylamine (Kb = 4.3 x 10-4) has been mixed with 5 mL of a 0.02 M solution of HCl.

Answer 1

Steps on doing this:

1) Calculate moles of ethylamine & HCl.
2) Determine the new concentrations of ethylamine & its conjugate acid after some of the ethylamine will be converted to ethylamineH+ from the HCl.
3) Use Henderson hasselbalch equation to find the pH of the buffer formed.

Answer 2

how would i do step number two? that's wht i seem to be hung up on

Answer 3

is it set up an ICE chart?