Write an equation to show the dissolving of the following substance in water.
(NH4)2SO4(s)
NH42SO4 + H2O -> 2NH4 + SO4 + H^+ + OH-?
I think what they want you to do is this.
(NH4)2SO4(s) + H2O ==> 2NH4^+(aq) + SO4^-2(aq)
Isn't the equation not balanced then?
No, you're correct. The equation isn't balanced. What we normally do is to write the arrow with H2O over the arrow to show that the solid is dissolving in water. That way the H2O doesn't actually enter into the balancing. I can't do that on these boards. Something like this but the H2O goes OVER the arrow and not through it. This is what one does when showing that the sample is treated with something (such as a catalyst although this is not a catalyst type reaction) and the result is what we see on the right (in this case the solvated ions. I think the main purpose of the problem is to make sure you understand that the (s) goes into solution, the ions are formed and that they are solvated, shown as (aq).
(NH4)2SO4(s) ==H2O==> (2NH4^+(aq) + SO4^-2(aq).
I understand now, thanks for clarifying. :)
The equation you provided does not accurately represent the dissolving of (NH4)2SO4 in water. Here's the correct equation:
(NH4)2SO4(s) + H2O(l) → 2NH4+(aq) + SO4^2-(aq)
In this equation, (NH4)2SO4(s) represents solid ammonium sulfate, H2O(l) represents liquid water, NH4+(aq) represents ammonium ions in aqueous solution, and SO4^2-(aq) represents sulfate ions in aqueous solution.
To write the correct equation, we start with the solid form of ammonium sulfate, (NH4)2SO4. When it dissolves in water, the solid breaks down into its constituent ions, which means that the ammonium ions (NH4+) and sulfate ions (SO4^2-) separate and become solvated in the water. This is represented by the dissociation of (NH4)2SO4 into 2NH4+ and SO4^2- ions.
Please note that the equation does not include any hydrogen ions (H+) or hydroxide ions (OH-) because ammonium sulfate is a salt and does not significantly dissociate into these ions when dissolved in water.