What is the pH of a solution that is 0.20 M CH3COOH and 0.10 M CH3COONa?
3 answers
Use the Henderson-Hasselbalch equation.
Please tell me if this is correct.
The pH of a solution: 0.20 M CH3COOH and 0.10 M CH3COONa
pH=pKa+log{[CH3COONa]/[CH3COOH]}
pH= -log(1.8x10-5)+log{0.10/0.20}
pH= 4.74+log 0.50= 4.74-0.30= 4.44
The pH of a solution: 0.20 M CH3COOH and 0.10 M CH3COONa
pH=pKa+log{[CH3COONa]/[CH3COOH]}
pH= -log(1.8x10-5)+log{0.10/0.20}
pH= 4.74+log 0.50= 4.74-0.30= 4.44
ph=pka+log[ch3coo-]\[ch3cooh]
3 answers