Sodium carbonate hydrolysis to the second step, the ionization process of carbonic acid is present

Actually, this idea you are talking about, not only the hydrolysis of sodium carbonate to the second step, is there an ionization process of carbonic acid? So in the first step of hydrolysis, is there ionization of bicarbonate ions? What about the hydrolysis of other ions?

This question should be understood as follows: in the system of carbonate ion hydrolysis, bicarbonate ion ionization is its inverse process! [The positive process is that the carbonate ions combine with hydrogen ions (but the hydrogen ions ionized by water, so it is written as water in the equation) to become bicarbonate ions, and the reverse process is that the hydrogen ions given by the bicarbonate ions become carbonate ions.

Since it is a reverse process, of course it exists. This is the same for any reversible reaction, so do you think it's necessary to discuss its effect on the positive reaction separately?

To be exact, it exists, it will reach a dynamic equilibrium, and it can be said that the impact is negligible.

In solution, it can exist when there are few carbonic acid molecules, but it will decompose into water and carbon dioxide when there are many carbonic acid molecules.

Carbonate is first hydrolyzed into bicarbonate, and bicarbonate is then hydrolyzed into carbonic acid, it must be noted that the hydrolysis of carbonate mainly exists in the first step and the second step is very weak.

Whether it is hydrolysis or ionization, it is very weak, remember!

No, carbonic acid is unstable, and once generated, it decomposes into water and carbon dioxide.

Only carbonate is present for hydrolysis, and sodium carbonate is a salt that is completely ionized.

Only hydrolysis of carbonate exists: CO3

2-+H2O = reversible = HCO3-+OH- (there is a second step, but to a small extent) Bicarbonate is ionized and hydrolyzed: HCO3-= reversible = H++CO32- (ionized), HCO3-+H2O= reversible = H2CO3+OH- (hydrolysis, also the second step of hydrolysis of carbonate), and bicarbonate hydrolysis is greater than ionization.

Yes, sodium carbonate hydrolysis is an inverse process, hydrolysis produces carbonic acid, and carbonic acid will also hydrolyze to reach an equilibrium. It has no effect on hydrolysis because it is a balance.

NA2CO3=2NA+ +CO32-Water Good First Step CO32- +H2O = HCO3- +OH-Second State HCO3- +H2O=H2CO3+0H-Hope, thank you.

Ionized HCO3-=H++CO32- Because bicarbonate is a weakly acidic acid, the acid salt of carbonic acid can either ionize the properties of an acid or hydrolyze the properties of a base.

The reason for the hydrolysis of HCO3-+H2O=H2CO3+OH- is that carbonic acid can be secondarily ionized.

h2co3=hco3-+h+

hco3-=h++co32-

2. NaHCO3 ==Na+ +HCO3- (with an inverse sign).

HCO3- = reversible == CO32- +H+ (with a reversible sign).

Sodium bicarbonate hydrolysis.

HCO3- +H2O = H2CO3 + OH-sodium bicarbonate ionization.

hco3- = co32- +h+

Sodium carbonate hydrolysis.

CO32- +H2O = HCO3- +OH- mainly takes place in this hydrolysis reaction.

A very small amount of HCO3- can undergo secondary hydrolysis: HCO3- +H2O = H2CO3 + OH-, and the second hydrolysis is negligible relative to the previous hydrolysis.

Sodium carbonate does not ionize.

Hello. An ion equation is a formula that represents a reaction with the symbols of the ions that actually participate in the reaction.

That is, it must be an ionic reaction to be represented by an ionic equation.

The conditions for ionic reactions to occur are aqueous solution or molten state, generally aqueous solution.

The decomposition of sodium bicarbonate 2NaHCO3===Na2CO3+H2O+CO2 This reaction is the decomposition reaction of solids, and the reaction conditions are not aqueous solutions.

Solid-to-solid, solid-to-gas, and gas-to-gas reactions are not ionic reactions. It cannot be expressed by ionic equations.

For example, Na2O2 and CO2 are not ionic reactions, while Na2O2 and H2O are ionic reactions.

Whereas, sodium bicarbonate and potassium bisulfate are carried out in an aqueous solution with ion participation, which is an ionic reaction.

So both sodium bicarbonate and potassium bisulfate must be taken apart.

Sodium bicarbonate ionizes HCO3- and Na+ under the action of water molecules, and potassium bisulfate ionizes K+, H+ and SO42-HCO3-+H+=H2O+CO2 under the action of water molecules

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If the reaction is in solution, it can be disassembled into ionic form, and this reaction heats sodium bicarbonate in solid form and does not need to be disassembled. The latter example is a reaction in solution, and the strong electrolyte naturally has to be disassembled.

Whether it is disassembled into ions or not, depending on its form of existence, the solution exists in the form of ions, which is written in the form of ions, and the solid is written as the chemical formula.

In other words, the ion equation can only be used when the particles in the reaction system are in the ionic state, in other words, the ion equation can only be used to represent the reaction when the reactants or products ionize out of the reaction.

In the reaction of 2AhCO3 = ( ) = Na2CO3 + H2O + CO2, the reactants and products are both solid or gas, there is no ionization, and there are no ions participating in the reaction, so it cannot be expressed using the ion equation, while the reaction of NaHCO3 and Khso4 is in an aqueous solution, and both reactants can ionize ions in water, that is to say, the reaction occurs between ions, so it can be expressed by the ion equation:

hco3-+h+=h2o+co2↑

There is also a situation where the electrolyte is melted, and the electrolyte can ionize ions in the case of melting, so this reaction can also be expressed by the ion equation, but the reaction in the molten state will not be encountered in the high stage, so I will not go into details.

I hope you can understand the above explanation.

The ionic equation for the hydrolysis reaction of sodium bicarbonate: HCO−HO==(reversible) HCO+OH-

Hydrolysis with aluminium chloride double hydrolysis: 3NaHCO+AlCl ==Al(OH)3CO+3NaCl

Double hydrolysis with aluminum sulfate: Al(SO)6NaHCO==3NaSO+2Al(OH)6CO

Sodium bicarbonate. Sodium bicarbonate (Nahco), commonly known as baking soda. White fine crystals, less soluble in water than sodium carbonate. It is an industrial chemical with low toxicity.

Solids above 50 begin to gradually decompose to produce sodium carbonate, carbon dioxide and water, and completely decompose at 440. Sodium bicarbonate is an acid salt formed after neutralization of strong alkali and weak acid, which is weakly alkaline when dissolved in water. This property allows it to be used as a leavening agent in the food production process.

Sodium bicarbonate will remain sodium carbonate after action, and too much use will make the finished product have an alkaline taste. ‍

Hydrolysis of sodium bicarbonate: HCO3 + H2O = (reversible) H2CO3 + OH

HCO3- +H2O == (reversible) H2CO3 + OH-

HCO3- hydrolysis is: HCO3- binds hydrogen ions in water, so that the solution containing OH- becomes alkaline!

Reaction with CuSO4: CuSO4 + 2 NaOH == Cu(OH)2 (precipitation) + Na2SO4 i.e. copper ions combine with hydroxide to form copper hydroxide precipitates.

The bicarbonate takes the h in the water and turns into carbonic acid, leaving the hydroxide to make the solution alkaline, at this time, adding copper sulfate, copper ions and hydroxide combine to form copper hydroxide, consuming hydroxide, making the bicarbonate further hydrolyzed, leaving more hydroxide, continuing to combine with copper ions, and starting to precipitate after saturation, which is the reaction of sodium hydroxide and copper sulfate.

Hydrolysis equation: HCO3- +H2O = H2CO3 + OH-

The hydrolysis equation is the hydrolysis of bicarbonate into carbonic acid and hydroxide, note that the reversible sign should be used because both sides are reversible.