Part of a question I did involved comparing the acidity of NH4+ vs. HF. I reasoned that:
NH4+ -----> yields a conjugate base: NH3
HF-------> yields a conjugate base: F-
Based on the fact that F- has a charge, whereas NH3 does not, I thought that F- would be considered a stronger, more reactive base. The negative charge would destabilize the base, making it more reactive. Thus, HF would be a weaker acid than NH4+. However, this was incorrect. What is wrong with this reasoning?
The correct...
Acid base reasoning
NH4+ -----> yields a conjugate base: NH3
HF-------> yields a conjugate base: F-
Based on the fact that F- has a charge, whereas NH3 does not, I thought that F- would be considered a stronger, more reactive base. The negative charge would destabilize the base, making it more reactive. Thus, HF would be a weaker acid than NH4+. However, this was incorrect. What is wrong with this reasoning?
The correct...
Acid base reasoning