Chem: Soluble with Insoluble: Will Reaction occur?

[madgab89]

Homework Statement

Write the balanced net ionic equations for the reactions, if any that occur between:

NiS(s) & HCl(aq)

My attempt:

NiS(s) + 2HCl(aq) -> NiCl2(aq) + H2S(s)

NiS(s) + 2H + 2CL -> Ni(aq) + 2CL + H2S(s)

NiS(s) + 2H(aq) -> Ni(aq) + H2S(s)

My real question is, would NiS and HCl even react, as NiS is insoluable...

 

[Borek]

H₂S is not solid.

Ionic and net ionic reactions require that ions have actual charges.

You are missing several (aq) symbols, but equations are - at least - properly balanced in terms of atoms.

My real question is, would NiS and HCl even react, as NiS is insoluable...

This is difficult question. Just because something is insoluble doesn't meant that it will not dissolve in acid or base - for example calcium carbonate, which is insoluble, will happily dissolve in hydrochloric acid with a lot of fizzling. Similar situation happens with many sulfides - they can be dissolved in hydrochloric acid. However, NiS is unique. It has two different forms. One dissolves easily, second can be dissolved only in the presence of strong oxidizing agents. The first one forms when you precipitate NiS, the second one - if NiS precipitate is left for at least several hours for so called aging. So both answers - that it will dissolve and that it will not - are right and wrong at the same time.

 

[Blueshift5]

Based on the given information, it is likely that a reaction will occur between NiS and HCl. NiS is a solid and HCl is an aqueous solution, which means they are in different physical states and can potentially react. Additionally, HCl is a strong acid and can potentially react with the metal in NiS to form a soluble salt, NiCl2. However, it is important to note that the reaction may not be complete as NiS is insoluble and may not fully dissolve in the solution. The balanced net ionic equations provided in the attempt section show the potential reactions that may occur between NiS and HCl. Further experimentation and analysis would be needed to determine the extent of the reaction and the products formed.