Why does NaF form a basic solution while sulfate and carbonate form acidic ones?

[MotoPayton]

I know that when a salt such as NaF is dissolved in water will dissociate and form HF creating a basic condition.

So why when you you have an ion such as sulfate or carbonate they react to form H2SO4 and H2CO3 they form a acidic solution.

These ideas seem to conflict? In both reactions you have a base absorbing hydrogens but only only in the first reaction a basic solution is formed.

Does this have something to do with the diprotic acid?

 

[Borek]

You are confusing something.

F^- + H₂O -> HF + OH^-

yields a basic solution.

CO₃^2- + H₂O -> HCO₃^- + OH^-

yields a basic solution as well.

It can even go further:

CO₃^2- + 2H₂O -> H₂CO₃ + 2OH^-

but this is a multistage equilibrium, with carbonic acid easily decomposing to water and carbon dioxide, so it is better to not treat this equation too seriously.

In the case of sulfates reaction

SO₄^2- + H₂O -> HSO₄^- + OH^-

also takes place (and can increase the pH), although to much lesser extent, as HSO₄^- is a relatively strong acid (alternatively SO₄^2- is a weak base).

 

[MotoPayton]

Okay, I must have misinterpreted something I read.

thanks for helping me out with all my dumb questions, appreciate it