Acid bases Buffers calculation help please
Predict then calculate the pH of a buffer containing
0.1M HF and 0.12M NaF? (Ka = 3.5 x 10-4)
0.1M HF and 0.1M NaF, when 0.02M HCl is added to the solution?
Part a is easy, in part b, should I just add the conc of HCl to HF and plug it in the same Henderson hasselbalch equation ?
0.1M HF and 0.12M NaF? (Ka = 3.5 x 10-4)
0.1M HF and 0.1M NaF, when 0.02M HCl is added to the solution?
Part a is easy, in part b, should I just add the conc of HCl to HF and plug it in the same Henderson hasselbalch equation ?
Original post by JanaALEVEL
Predict then calculate the pH of a buffer containing
0.1M HF and 0.12M NaF? (Ka = 3.5 x 10-4)
0.1M HF and 0.1M NaF, when 0.02M HCl is added to the solution?
Part a is easy, in part b, should I just add the conc of HCl to HF and plug it in the same Henderson hasselbalch equation ?
0.1M HF and 0.12M NaF? (Ka = 3.5 x 10-4)
0.1M HF and 0.1M NaF, when 0.02M HCl is added to the solution?
Part a is easy, in part b, should I just add the conc of HCl to HF and plug it in the same Henderson hasselbalch equation ?
b) No, you can't do that.
Remember that an acidic buffer works by absorbing "extra" acid using the reservoir of conjugate base ions - in this case the fluoride ions.
H+ + F- ==> HF
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