Equation for ammonium and metaaluminate NaOH

h+ ＋oh- ＝h20

al3+ ＋3oh- ＝al(oh)3↓

Because Al3+ and Fe3+ usually precipitate at pH 4, this step of the reaction precedes the next step.

nh4+ ＋oh- ＝nh3·h2o

al(oh)3 ＋ oh- ＝alo2- ＋2h2o

NH4+ +OH- === NH3·H2ONH3·H2O=(Heating)=NH3 +H2O Metaaluminate does not react with sodium hydroxide!

Contains hydrogen ions: H+ +OH- ==H2O

Contains ammonium: NH4+ +OH- ==NH3·H2ONH4+ +OH- = (heating)=NH3 +H2O contains aluminum ions: AL3+ +3OH- ===AL(OH)3 AL(OH)3+OH-====AL(OH)4-

NH4+ +OH-=NH3+H2O (heated) metaaluminate does not react with sodium hydroxide.

h+ +oh-=h2o

nh4+ +oh-=nh3+h2o

al3+ +3oh==al(oh)3

al(oh)3+oh-=al[oh]4-

Metaaluminate does not react with sodium hydroxide.

alo2- +nh4+ +h2o=al(oh)3 ↓+nh3↑

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ALO2- +NH4+ +2H2O=AL(OH)3 Lead +NH3·H2O

Ammonium and metaaluminate cannot coexist.

Because ammonium can be dihydrolyzed with metaaluminate:

The dihydrolysis reaction refers to the hydrolysis of weak acid ions and weak base cations, such as AlO2- and NH4+, until the reaction is complete.

Whether the dihydrolysis reaction can be fully carried out depends on two factors:

1. The degree of mutual promotion of hydrolysis (including the influence of material nature, external conditions, etc.);

2. Solubility of hydrolysate.

Because ammonia is a weak alkali and cannot be acidic, aluminum hydroxide is regarded as an acid, so aluminum hydroxide can be regarded as halo2·h2o, that is, metaaluminic acid, and the corresponding acid is aluminum hydroxide. If aluminum hydroxide is regarded as a base, it can be regarded as a combination of aluminum ions and three hydroxide groups, and the corresponding metal ions are Al3+.

Ammonium can be double-hydrolyzed with metaaluminate: NH4+ +alo2- +H2O ==Al(OH)3 +NH3; Since aluminum hydroxide and ammonia are separated from the reaction system in the form of precipitated gases and promote hydrolysis, the two ions cannot exist stably in solution at the same time.

If you are not satisfied, you can continue to ask.

Summary. Ammonium ions and metaaluminate ions react to form precipitate, aluminum hydroxide and ammonia, and the ammonium can be double-hydrolyzed with metaaluminate, NH4+ +ALO2- +H2O = Al(OH)3 + NH3

Ammonium ions react with metaaluminic acid empty silver ions to form precipitate, aluminum hydroxide and ammonia, and ammonia, and the root can be double-hydrolyzed with metaaluminate, NH4+ +alo2- +H2O = Al(OH)3 + NH3

The generation of ammonia monohydrate or ammonia gas, generally speaking, the generation of ammonia ha

Isn't ammonium ion hydrolysis to produce ammonia monohydrate, which is a bit incomprehensible.

It depends on the reaction environment and the concentration of the products Generally, the alkaline environment produces ammonia; The ammonia produced has a large concentration and also decomposes into ammonia.

For this double hydrolysis, ammonia is generally generated

Okay, sodium metaaluminate and ammonium bicarbonate react, what is the product.

Which ion does metaaluminate react with first?

It depends on the concentration, which is that double hydrolysis occurs and first reacts with bicarbonate to form carbonate

Ion equation: 2alo2- +2HCO3- +2H2O==2Al(OH)3 +2CO3 2-

The concentration is the same, first double hydrolysis with ammonium or reaction with bicarbonate.

The concentration is the same, and the bicarbonate is reacted first, and then hydrolyzed

The ion of ammonium root soothing pants is acidic and can react with alumina.

6nh4++3h2o+al2o3=2al3++6nh3·h2o

Metaaluminate and carbonate are both weak acid acids, so they can be hydrolyzed, metaaluminate hydrolysis to produce aluminum hydroxide, metaaluminic acid and carbonate can not coexist! It will be double hydrolyzed to produce aluminum hydroxide and ammonia (this reaction can also explain the problem that excess ammonia water will not dissolve aluminum hydroxide), and so on with other hydrolyzed acidic salt solutions such as soluble copper salt solution, etc., it will also double hydrolyze to form aluminum hydroxide and corresponding hydroxides. Metaaluminic acid (i.e., aluminum hydroxide) is weaker acidic than carbonic acid, so sodium metaaluminate that has been in the air for a long time will deteriorate.

Metaaluminate can be obtained by dissolving aluminium or alumina or aluminium hydroxide in a strong alkaline solution!

It cannot exist in alkaline solutions, at least not in large quantities, because it will react with hydroxide ions to form ammonia monohydrate, which is a weak electrolyte and is not easy to ionize into ammonium ions. It should be able to coexist with general ions except hydroxide ions, because the radius of ammonium ions is similar to that of potassium ions, so the solubility is basically the same, so ammonium salts are basically soluble.

Both are susceptible to hydrolysis. Metaaluminate ions are weak acids (bases), which are easy to combine with hydrogen ions to form aluminum hydroxide precipitates;

Ammonia ions are weak acids, which are easy to combine with hydroxide ions to generate ammonia monohydrate (NH3·H2O), which is heated to release ammonia gas.

When the two meet in solution, a "double hydrolysis" reaction (two mutually reinforcing hydrolysis reactions) occurs, resulting in aluminium hydroxide precipitates and ammonia.

Metaaluminate and acid will form a precipitate, excess acid will redissolve, excess CO2 will not be dissolved, ammonium ions and alkaline solution will form gas.

Hydrolysis will occur, and metaaluminate ions will combine with hydrogen ions in water to form metaaluminic acid, and ammonia ions will combine with hydroxide ions in water to form ammonia monohydrate.