may22
Well-Known Member
- Joined
- Jun 15, 2021
- Messages
- 498
- Gender
- Female
- HSC
- 2022
Hey everyone,
I just worked out a question that needed me to calculate the pH of a buffer solution. I used the Henderson-Hasselbalch equation (pH = pKa+ log([A-]/[HA]) ) and got 4.89. I checked the solutions, and it was worked out by using the Ka expression, and then using pH = -log[H+], which led to pH = 4.61.
I've cross-checked my response, and the solutions, for any mathematical errors but have found none. My question is...what happens if this is the case in an exam? Are both solutions technically correct based on working out? If not, then which method is more reliable to use in exams?
I just worked out a question that needed me to calculate the pH of a buffer solution. I used the Henderson-Hasselbalch equation (pH = pKa+ log([A-]/[HA]) ) and got 4.89. I checked the solutions, and it was worked out by using the Ka expression, and then using pH = -log[H+], which led to pH = 4.61.
I've cross-checked my response, and the solutions, for any mathematical errors but have found none. My question is...what happens if this is the case in an exam? Are both solutions technically correct based on working out? If not, then which method is more reliable to use in exams?