Question
Calculate the pH of the solution that results from the mixture. 170 mL of 0.12 M C2H5NH2 with 285.0 mL of 0.22 M C2H5NH3Cl.
Answers
This is a buffer problem. Use the Henderson-Hasselbalch equation. C2H4NH2 is the base.
wha are the relative numbers of h3o+ and oh ions in an acidic, a basic, and a neutral solution?
Related Questions
Calculate the pH of each of the following buffered solutions:
a. 0.10M C2H5NH2/0.25M C2H5NH3Cl
b....
Calculate the pH of a solution that is 0.124 M C2H5NH2 and 0.124 M C2H5NH3Cl. (Assume that the solut...
A buffered solution is made by adding 48.6 g C2H5NH3Cl to 1.00 L of a 0.77 M solution of C2H5NH2. Ca...
Calculate the pH of a 50.0 mL solution 0.0120 M ethylaminium chloride (C2H5NH3Cl ) and 0.0360 M ethy...