[skibum143]

0.03 moles of NaOH are added to a 1.0L solution of 0.1M HF. Aftre the solution comes to equilibrium, what is the pH?

Since this is a weak acid titrated with a strong base, at equilibrium the moles of base added should equal the original moles of acid. And I think I should find the molarity of the base using an ICE table, but I can't figure out what the reaction is?

NaOH + HF -> NaF + H2O?

How do I find the pH?
thanks

[TheUnfocusedOne]

0.03 moles of NaOH are added to a 1.0L solution of 0.1M HF. Aftre the solution comes to equilibrium, what is the pH?

Since this is a weak acid titrated with a strong base, at equilibrium the moles of base added should equal the original moles of acid. And I think I should find the molarity of the base using an ICE table, but I can't figure out what the reaction is?

NaOH + HF -> NaF + H2O?

How do I find the pH?
thanks

That reaction is right, just do the normal procedure with the ICE table.

[skibum143]

but don't i need either the concentration of [OH-] or [H3O+] in order to get the pH?

[Borek]

Buffer. Henderson-Hasselbalch equation.