What is the reaction of ammonium sulfate solution and urea solution when heated

Why ammonium sulfate solution and barium hydroxide solution react to produce ammonia gas (not heated).

It is true that the reaction starts with the formation of ammonia monohydrate, but as the reaction progresses, the ammonia monohydrate is gradually saturated, and ammonia gas is precipitated from the liquid.

Summary. The sodium bowl acid reaction is a common chemical reaction that involves the reaction of bowl bowl acid (EDTA) with urea (NH4OH). In this reaction, EDTA reacts with NH4OH to produce a compound called ammonium bowlate.

The reason for this reaction is that EDTA is more basic and NH4OH is more acidic, so there is a reaction between them. In addition, EDTA has strong complexability and can combine with hydrogen ions in NH4OH to form ammonium bowlate. The solution to this reaction is that the EDTA solution should be diluted before mixing EDTA and NH4OH to reduce the alkalinity of EDTA, thereby reducing the reaction between EDTA and NH4OH.

In addition, the contact time between EDTA and NH4OH should be minimized to reduce the occurrence of reactions. Personal tip: When mixing EDTA and NH4OH, the alkalinity of EDTA should be minimized, and the contact time between EDTA and NH4OH should be minimized to reduce the occurrence of reactions.

Ammonium nitrate reacts with sodium carbonate The reaction of ammonium nitrate with sodium carbonate is a chemical reaction that can produce gas holding early body nitrogen (N2) and water (H2O). The chemical equation of the reaction is: 2NH4NO3 + NA2CO3 N2 + 3H2O + 2NANO3

Fellow, I really didn't understand, I can be more specific.

The sodium bowl acid reaction is a common chemical reaction that involves the reaction of bowl bowl acid (EDTA) with urea (NH4OH). In this reaction, EDTA reacts with NH4OH to produce a compound called ammonium bowlate. The reason for this reaction is that EDTA is more alkaline and NH4OH is more acidic, so there is a reaction between them.

In addition, EDTA has strong complexability and can combine with hydrogen ions in NH4OH to form ammonium bowlate. The solution to this reaction is that the EDTA solution should be diluted before mixing EDTA and NH4OH to reduce the alkalinity of EDTA, thereby reducing the reaction between EDTA and NH4OH. In addition, the contact time between EDTA and NH4OH should be minimized to reduce the occurrence of reactions.

Personal tip: When mixing EDTA and NH4OH, the alkalinity of EDTA should be minimized, and the contact time between EDTA and NH4OH should be reduced as much as possible to reduce the occurrence of reactions.

Reaction Commentary:

Urea and magnesium sulfate solution can react, urea is hydrolyzed first, and then metathesis with magnesium sulfate to form magnesium carbonate precipitate and ammonium sulfate.

Chemical equation for reaction:

Con2H4+MgSO4+2H2O ====MgCO3 (precipitate) +2 (NH4)2SO4

Note: The reaction occurs in solution or in a wet condition, as the reaction requires the participation of water.

Expansion: Mixed use of urea and magnesium sulfate. (Urea is a fertilizer, magnesium sulfate is a pesticide).

1) The mixed use of chemical fertilizers and pesticides can not only provide crop nutrients, but also prevent diseases, insects and weeds, which is a technology widely adopted in recent years. The benefits are:1

Improve the efficacy of the drug 2Improve fertilizer efficiency 3Improve ergonomics.

When nitrogen fertilizer is applied for the first time in early rice, the herbicide Fuxing grass is mixed to provide fertilizer and weeding.

2) Although there are many advantages to mixing fertilizers with pesticides, not all pesticides and fertilizers can be mixed, and whether they can be mixed depends on two principles:

1. Do not reduce the fertilizer efficacy and drug efficacy. For example, ammonium nitrogen fertilizer or water-soluble phosphate fertilizer cannot be mixed with alkaline pesticides such as Bordeaux liquid, otherwise the active composition of fertilizer will be reduced.

2. It is harmless to crops after mixing.

3) Throughout the local experiments, the following fertilizers and pesticides can be mixed:

1.Mancozeb can be mixed with urea, magnesium sulfate, ammonium sulfate, etc.

2.Herbicides 2 potassium 4 chlorine, flulolu, Nongdeshi, fuca, butachlor, etc. can be mixed with urea or compound fertilizer.

3.Plant growth regulators gibberellin, triacosanol, and polycephalic acid can be mixed and sprayed with urea, potassium dihydrogen phosphate, and boric acid.

4) When fertilizers and pesticides are mixed, we must pay attention to the mixing method. If both fertilizers and pesticides are solid and applied to the soil, they can be mixed together and spread on the surface. If the agent is a wettable powder, you can spray the surface of the fertilizer with a small amount of water first, and then add the solution and stir it thoroughly.

If the agent is emulsifiable or aqueous, it can be poured directly on the fertilizer and mixed, if it is too wet, a small amount of dry fine soil can be added. If foliar sprays are required, emulsifiable concentrate, water or wettable powder pesticides can be used in a solution with chemical fertilizers.

It's about temperature.

At room temperature, urea is readily soluble in concentrated sulfuric acid to form stable urea sulfate.

co(nh2)2 + h2so4 = co(nh2)2•h2so4

co(nh2)2 + 2 h2so4 = co(nh2)2•2h2so4

80 90, the hydrolysis reaction will occur in the aqueous solution system of sulfuric acid and urea, CO(NH2)2 + H2SO4 + H2O = (NH4)2SO4 + CO2

When it is above 150, sulfuric acid and urea react to form sulfamic acid and ammonium sulfate.

co(nh2)2 + 2 h2so4 = 2 nh2so3h + co2 + h2o

co(nh2)2 + h2so4 + h2o = (nh4)2so4 + co2

No, urea is alkaline and ammonium sulfate is acidic, and the two react to form ammonia gas, which loses the N element in the fertilizer.

Answer: There is no chemical reaction between ammonium sulfate solution and urea solution.

The dissolution of urea into water produces the following reactions:

CO(NH2)2+2H2O = (NH4)2CO3Ammonium carbonate and ammonium sulfate are not chemically reacting.