A 10.0-mL solution of 0.300 M NH3 is titrated with a 0.100 M HCl solution. Calculate the pH after the following additions of the HCl solution:
a) 0.00 mL
b) 10.0 mL
c) 20.0 mL
c) 30.0 mL
d) 40.0 mL
**I know how to solve the problem but I keep getting answers that are exactly one away from the correct answer.
2 answers
Actually I figured out a, b, c, and d but I can't figure out e. What do you do if HCl is in excess?
If HCl is in excess, calculate how much excess in mols, divide by the TOTAL volume at that point to obtain (HCl) in mols/L; ie., M, then pH = -log(HCl) since HCl is a strong acid and ionizes 100%.
1 answer