🤓 Based on our data, we think this question is relevant for Professor Grice's class at DEPAUL.
• C2H5COONa will break up in the solution
▪ C2H5COO- → weak base (conjugate base)
[C2H5COO-] = [C2H5COONa]
▪ Na+ → neutral ion → will not contribute to pH
• C2H5COOH → weak acid
• The solution is composed of a weak acid and its conjugate base, therefore we have a buffer.
Step 1: Calculate the pKa of the weak acid.
Ka C2H5COOH = 1.34x10-5
pKa = 4.87
Step 2: Create an ICF chart and determine the final amounts of species present after the reaction.
▪ weak acid + conjugate base = buffer
Step 3: Calculate the pH of the solution.
A buffer contains 0.16 mol of propionic acid (C2H5COOH) and 0.22 mol of sodium propionate (C2H5COONa) in 1.20 L.
What is the pH of the buffer after the addition of 0.02 mol of NaOH?
Frequently Asked Questions
What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Buffer concept. You can view video lessons to learn Buffer. Or if you need more Buffer practice, you can also practice Buffer practice problems.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor Grice's class at DEPAUL.