SODIUM BIFLUORIDE NaHF2

Properties of sodium bifluoride NaHF2:

White, decomposes when heated. Stable in dry air. Moderately soluble in water, the anion is partially decomposed, and due to protolysis of HF creates an acidic environment. Crystalline hydrates do not form. Decomposed by concentrated acids, neutralized by alkalis.


Obtaining sodium bifluoride NaHF2:

NaOH + HF (diluted) = NaF + H2O

NaOH + 2 HF (conc.) = NaHF2 + H2O.

Na2CO3 + 2 HF (diluted) = 2 NaF + H2O + CO2↑

Na2CO3 + 4 HF(conc.) = 2 NaHF2 + CO2↑ + H2O.

NaF + HF (conc.) = NaHF2

NaF + nHF(liquid) = NaF·nHF↓, or Na[F(HF)n] (n = 1 / 4).


Reactions with sodium bifluoride NaNF2:

NaHF2 = NaF + HF (270 - 400° C).

NaHF2 (diluted) + 4H2O = [Na(H2O)4](+) + HF2(-)

HF2(-) ↔ HF + F(-)

HF + H2O ↔ F(-) + H3O(+); pKк = 3,18.

2 NaHF2 + H2SO4 (conc.) = Na2SO4 + 4HF↑ (boiling)

NaHF2 + NаOH (conc.) = 2 NaF + H2O

NaHF2 + Ca(ОН)2 (saturated) = NaOH + H2O + CaF2↓.

 

Did you know?

Although oxygen gas is colorless, the liquid and solid forms of oxygen are blue.