Molecular, ionic, and net ionic equations for ammonium chloride + potassium sulfate. Also what is the observation.
Is it 2NH2Cl + Na2SO4 = (NH4)2SO4 + 2NaCl????
Please help!
Not quite.
ammonium chloride is NH4Cl.
potassium sulfate is K2SO4.
Is this a trick question. There is no reaction, just a mixing of the ions. Is this an aqueous solution?
If solids:
NH4Cl(s) + K2SO4(s) ==> No reaction
If aqueous solutions:
NH4Cl(aq) + K2SO4(aq) ==>NH4^+(aq) + Cl^-(aq) + 2K^+(aq) + SO4^2-(aq)
The latter is the ionic as well as the net ionic equation if the salts are in aqueous solution.
The correct balanced molecular equation for the reaction between ammonium chloride (NH4Cl) and potassium sulfate (K2SO4) is:
2NH4Cl + K2SO4 → (NH4)2SO4 + 2KCl
In this reaction, ammonium chloride and potassium sulfate react to form ammonium sulfate and potassium chloride.
To write the ionic equation, we need to dissociate the soluble ionic compounds into their respective ions:
2NH4Cl(aq) + K2SO4(aq) → (NH4)2SO4(aq) + 2KCl(aq)
Now, to write the net ionic equation, we remove the spectator ions (ions that appear on both sides of the equation without undergoing a change):
Net ionic equation:
2NH4+(aq) + SO42-(aq) → (NH4)2SO4(aq)
The observation for this reaction will be the formation of a white solid, which is the ammonium sulfate (NH4)2SO4 precipitate.
To determine the molecular, ionic, and net ionic equations for the reaction between ammonium chloride (NH4Cl) and potassium sulfate (K2SO4), we need to understand the nature of the compounds involved.
Ammonium chloride (NH4Cl) is a salt composed of ammonium ions (NH4+) and chloride ions (Cl-). Potassium sulfate (K2SO4) is also a salt composed of potassium ions (K+) and sulfate ions (SO4^2-).
The balanced molecular equation for the reaction can be written as:
NH4Cl + K2SO4 → (NH4)2SO4 + 2KCl
To obtain the ionic equation, we must first dissociate the ionic compounds into their constituent ions. In water, NH4Cl dissociates into NH4+ and Cl- ions, while K2SO4 dissociates into 2K+ and SO4^2- ions. Thus, the ionic equation is:
2NH4+ + 2Cl- + 2K+ + SO4^2- → (NH4)2SO4 + 2K+ + 2Cl-
Next, we need to identify the spectator ions, which are ions that appear on both sides of the equation and do not participate in the overall reaction. In this case, the spectator ions are K+ and Cl-.
Therefore, the net ionic equation, which includes only the species involved in the reaction, is:
2NH4+ + SO4^2- → (NH4)2SO4
The observation during this reaction would be the formation of a white precipitate, as (NH4)2SO4 is insoluble in water and will appear as a solid.
Overall, the correct equation is:
NH4Cl + K2SO4 → (NH4)2SO4 + 2KCl