A small amount of sodium hydroxide solution is dropped into ammonium bicarbonate solution to write the ion equation. So the question is, is this small amount of hydroxide reacting with ammonium, or is it going to react with the bicarbonate?
According to zhihong optimization, a small amount of hydroxide will react with the acid root, the hydrogen carbonate, and the ion equation is:
OH- + HCO3- = H2O + CO32-.
But the problem is that the remaining ammonium ions are acidic, and the resulting carbonate ions are alkaline. Can they coexist? Don't they hydrolyze?
The hydrolysis rate of ammonium ion and carbonate ion concentration were calculated to be about 70 %. The hydrolysis rate is more than 50 percent, indicating that this small amount of hydroxide and ammonium ion reaction, the ion equation should be:
OH- + NH4+ = NH3.H2O.
It's wrong here.
The question comes up -- is ammonium carbonate in solution? There are no strokes in the material's solubility table. I again calculate standard double hydrolysis conditions of the concentration of ammonium carbonate solution, found that carbonate root hydrolysis rate up to what, because of the ammonium ion concentration doubled, promote the hydrolysis of carbonate ions. Of course, the hydrolysis rate of ammonium is reduced from 70 percent to more than 40 percent. At ordinary times, we say that ammonium and carbonate ions can coexist, because their double hydrolysis is not obvious, and the ammonia solubility is very large. In addition, it also has the properties of ammonium carbonate, for example, calcium chloride solution will still be formed by calcium carbonate. In fact, there are a lot of ammonium bicarbonate and ammonium bicarbonate. Why don't you draw bars in the solubility table? This is a lot of ammonia water and we still call it "ammonia".
Because the ammonium ion and carbonate ion are mutually promoted, the double hydrolysis is complete, so the ammonium nitrogen fertilizer cannot be mixed with the ash. In the field, the reaction of fertilization in the field has its particularity -- in the field, it is more volatile to volatilize the ammonia gas and promote the double hydrolysis of ammonium carbonate.
In fact, with respect to the addition of a small amount of alkali to ammonium bicarbonate, the ammonium ion is more acidic than the bicarbonate, which is, of course, the first and the base reaction. The ammonium sulfate ion should be reacted first and the hydrolysis rate of ammonium carbonate was calculated.