Asked by Schanee
Calculate the pH of a solution that is 2.00 M HF, 1.00 M NaOH, and 0.704 M NaF. (Ka = 7.2 E -4)
Answers
Answered by
DrBob222
You have two problems in one here.
First, the NaOH will neutralize part of the HF. Do that first and see how much HF is left. Then you will have a solution of NaCl, HF, and NaF. The NaCl is neutral and will not change the pH. The HF/NaF mixture is a buffered solution. Use the Henderson-Hasselbalch equation to solve for the pH. Post your work if you get stuck.
First, the NaOH will neutralize part of the HF. Do that first and see how much HF is left. Then you will have a solution of NaCl, HF, and NaF. The NaCl is neutral and will not change the pH. The HF/NaF mixture is a buffered solution. Use the Henderson-Hasselbalch equation to solve for the pH. Post your work if you get stuck.
There are no AI answers yet. The ability to request AI answers is coming soon!
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.