![]() ![]() Notice that because hydrofluoric acid does not dissociate completely, you must represent it in molecular form. Now, the complete ionic equation looks like this - keep in mind that sodium fluoride is soluble in aqueous solution This will go on until all the molecules of acid have dissociated and all the hydrogen cations have reacted with the hydroxide anions #-># a complete neutralization took place. This will consume hydrogen cations and cause the dissociation equilibrium of hydrofluoric acid to shift to the right #-># more of the molecules of acid will dissociate. The hydroxide anions and the hydrogen cations will neutralize each other to produce water. Sodium hydroxide, on the other hand, will dissociate completely in aqueous solution to produce sodium cations, #"Na"^(+)#, and hydroxide anions, #"OH"^(-)# Instead, an equilibrium will be established between the undissociated acid and the dissociated ions Now, the important thing to remember here is that hydrofluoric acid is a weak acid, which implies that it does not dissociate completely in aqueous solution to form hydrogen cations, #"H"^(+)#, usually referred to as hydronium cations, #"H"_3"O"^(+)#, and fluoride anions, #"F"^(-)#. For our purposes, an acid is a substance that increases the concentration of hydrogen ions (H + + + start superscript, plus, end superscript) in a solution, usually by donating one of its hydrogen atoms through dissociation. #"HF"_ ((aq)) + "NaOH"_ ((aq)) -> "NaF"_ ((aq)) + "H"_ 2"O"_ ((l))# Structure, properties, spectra, suppliers and links for: Hydrofluoric acid, Hydrogen fluoride,, 1, 1, 1, 3. H + + + start superscript, plus, end superscript concentration shifts away from neutral when an acid or base is added to an aqueous (water-based) solution. Hydrofluoric acid, #"HF"#, a weak acid, will react with sodium hydroxide, #"NaOH"#, a strong base, to produce aqueous sodium fluoride, #"NaF"#, and water.
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