High school chemistry problems often encounter problems with bisulfite and bicarbonate

When heated, there will be gas overflow, and the colored one is sulfite, and vice versa.

Bisulfite and bicarbonate only react with strong acids and bases;

React with the acid to produce the same gas as the magenta solution!

The hydrogen ions in bisulfate and bisulfite are ionized separately, although the degree of ionization is different, so the aqueous solution of sodium bisulfate and sodium bisulfite is acidic, so it will react to form carbonic acid and sulfite, and carbonic acid is decomposed into water and carbon dioxide.

reaction to produce water and carbon dioxide and sulfite.

Bicarbonate is a weakly acidic acid that is not completely ionized into bicarbonate in an aqueous solution, and will also be hydrolyzed into carbonic acid.

When it reacts with acid, carbonic acid is formed, and carbonic acid is generally easy to decompose to form water and carbon dioxide, and carbon dioxide mostly escapes in the form of gas.

When it reacts with alkali, carbonate and water are generated, and when it reacts with Ca(OH)2 and Ba(OH)2, carbonate combines with calcium ions to form CaCO3 and BaCO3 precipitates.

There are few reactions with salts except for hydrolysis reactions, and the most important in the hydrolysis reaction is the complete double hydrolysis with iron ions and aluminum ions: Fe(OH)3, Al(OH)3 and CO2 are generated

Bisulfate exists in very small amounts in water, and can be considered to be completely ionized to generate hydrogen ions and sulfate, so it does not react with strong acids, reacts with weak acids or acid acids, neutralizes with alkalis, and reacts with acid salts, basic salts and barium salts.

For example: NaHSO4+NAHCO3=Na2SO4+H2O+CO2, NAHSO4+BACl2=NaCl+HCl+BASO4

Hope it helps.

Bisulfate ion is equivalent to the combination of hydrogen ion and sulfate ion, what are the properties of hydrogen ion and sulfate ion, what are the properties of bisulfate ion.

Bicarbonate ions can react with strong alkali solutions, acid solutions, and double hydrolysis with aluminum ions, iron ions, etc.

Bicarbonate, bisulfate, etc. in high school chemistry are the products of incomplete neutralization of multiple acids and alkalis, for bicarbonate, bisulfite, hydrogen phosphate, dihydrogen phosphate belong to weak acid hydrogen ions, which can be ionized and hydrolyzed, the ionization equation is HCO3- reversible sign H+ +CO32-, and the hydrolysis equation is HCO3- +H2O reversible = H2CO3 = OH-, so it can react with both acid and base, such as HCO3- +H+ =CO2 +H2O, hco3- +oh- =co32- +h2o;

Bisulfate, on the other hand, is a strong acid acid root ion, completely ionized, non-hydrolyzed, HSO4- = SO42- +H+; Therefore, it can be equivalent to acid, reacting with active metals to release hydrogen gas, reacting with metal oxides, reacting with alkalis and other common properties of acids.

Sulfuric acid is a binary strong acid, which is completely ionized into ions in the ion reaction, so it is divided into two hydrogen ions and one sulfate ion in the ion equation, so the bisulfate is separated into hydrogen ions and sulfate ions in the ion equation;

Carbonic acid, sulfurous acid, phosphoric acid, etc. are multiple weak acids, and some of them are ionized into ions in the ion reaction, so they cannot be separated in the ion equation, so their "hydrogen roots" must not be separated in the ion equation.

Summary: The "hydrogen roots" of strong acids are disassembled into hydrogen ions and acid groups in the ion equation, and the "hydrogen roots" of weak acids cannot be disassembled.

Sulfuric acid is a binary strong acid, which is completely ionized into ions in aqueous solution, so it is divided into two hydrogen ions and one sulfate ion in the ion equation, so the bisulfate is separated into hydrogen ions and sulfate ions in the ion equation;

Carbonic acid, sulfurous acid, phosphoric acid, etc. are multiple weak acids, and some of them are ionized into ions in the ion reaction, so they cannot be separated in the ion equation, so their "hydrogen roots" must not be separated in the ion equation.

Summary: The "hydrogen root" of strong acid is disassembled into hydrogen ions and acid roots in the ion equation in aqueous solution, and the "hydrogen root" of weak acid cannot be disassembled.

You can understand that bicarbonate is insoluble in water, while bisulfate itself can be dissolved in water.

The fact is that bicarbonate is a monolithic molecular structure, and bisulfate is just a temporary combination of hydrogen ions and sulfate.

Because carbonic acid is a weak acid, it is hydrolyzed and ionized in water to produce bicarbonate. Sulfuric acid is a strong acid, so it is directly converted into hydrogen ions and sulfate.

Bao2 is easily soluble in water and reacts with water to form Ba(OH)2.

Joining bao2 is essentially adding ba(oh)2.

A small amount of Ba(OH)2 2HCO3- +BA2+ +2OH- =BACO3 +2H2O +(CO3)2-

Excess Ba(OH)2 Ba2+ +OH- +HCO3-=BaCO3 +H2O

ba2++（so3）2-=baso3↓

Oxygen and barium hydroxide are generated.

Consider oxidation. There will be barium sulfate and barium carbonate in sufficient amounts, and sulfur ions are hard to say, because the so3 2- of +6 is oxidized and the -2 will oxidize, but I don't know to that extent that I forget more in high school, and the idea is probably like this.

Reaction principle: Bisulfite, which has strong reducibility, loses electrons at the negative electrode of the galvanic cell or the anode of the electrolytic cell to generate sulfate.

The role of hydrogen ions: equilibrium the charge on the right side of the equation.

If hydrogen is generated, water is needed to obtain electrons, and it is impossible to react with the above electrode at the same electrode.

If you don't understand anything, please feel free to ask.

Because if there is a large amount of HCO3- in the solution, the addition of BA(OH)2 will also have a white BAC3 precipitation (HCO3- +OH-+BA2+==BAC3 +H2O), and the addition of hydrochloric acid will dissolve, resulting in CO2 to make the clear lime water turbid, so that it is not certain that there is a large amount of CO32- in the solution.

NaHCO3 and others can also precipitate with Ba(OH)2.

It is assumed that there is SO32- in the original solution

When ba(no3)2 is added:

The solution has NO3- and SO32- at this time, but because there is no H+ in the solution, NO3- cannot oxidize SO32-

At this point, HCL is added, and H+ is introduced

So first of all, NO3- will oxidize SO32- to SO42- but beware... After NO3- is reduced, NO2 (or NO2) should be generated, neither of which does not meet the condition of colorless and odorless gas...

Because although no is colorless and odorless, it is quickly oxidized to no2 in the air, red...

So I think it's wrong, you teachers are wrong ...

Unless, assuming that the experiment is done in isolation from air, no cannot be converted to no2, then the experimental phenomenon is in line with ...

So.. I don't know if I'm thinking too much...