When aqueous solutions of potassium fluoride and hydrochloric acid are mixed, an aqueous solution of potassium chloride and hydrofluoric acid results

Question

Write the net ionic equation for the reaction.

(Use the solubility rules provided in the OWL Preparation Page to determine the solubility of compounds.)

Use H+ for the hydronium ion.

Answer 1

It is easiest to write the compete molecular equation first, and then write the ionic and/or net ionic.

KF(aq) + HCl(aq) ===>KCl(aq) + HF(aq)

Don't know what the solubility rules in the OWL Preparation page show, but all species are soluble. This is an example of writing an net ionic when one species is a WEAK ELECTROLYTE (not a precipitate).  That species is HF which is a WEAK acid and does not dissociate completely. Thus, you have:

K⁺(aq) + F^-(aq) + H⁺(aq) + Cl^-(aq) ==> K⁺(aq) + Cl^-(aq) + HF(aq)  complete ionic equation

H⁺(aq) + F^-(aq) ===> HF(aq)  net ionic equation