The reaction formula of sodium nitrite with 4 valent cerium ions under strong acidic conditions unde

In fact, this reaction does not need to be in a strong acidic solution.

And there is also acid formation in this reaction.

And if you are a landlord, you will learn it slowly on the way to learn chemistry in the future.

Actually, it's not just this one reaction at all, and there are a lot of reactions that are like this.

In redox reactions, we actually have three redox environments.

1. The most common: acidic That is to say, it must be oxidized with the help of hydrogen ions (but this oxygen.

The most complete chemical is permanganate or dichromate, which are completely oxidized).

2. The least common: alkaline conditions A few reactions can be completed under alkaline conditions, but they are also the least complete for oxidation.

For example, potassium permanganate will only become potassium manganate under alkaline conditions.

3. Relatively rare: neutral conditions can be partial reaction in a neutral environment can not only be completed, but even will.

There is an acid or a base that is produced in this category

The equation for the reaction that occurs is: 2CE4+ +NO2- +H2O == 2CE3+ +NO3- +2H+

It is precisely because there is such a classification of redox reactions that he has his difficulty:

What are the necessary reactants for some reactions? Is it water? Or is it an acid or a base?

And I'm going to give you a little bit of advice here, which is that we can try to add hydrogen ions on the left side and the right side without any doubt.

Ask if it's a water molecule and if it is found that it can't be leveled during the balancing process!! It's going to be back on the left right away.

It should be changed to alkaline oh-, and of course, if you give it an environment, it will be very helpful for us.

It's all hand-made, and if I hadn't thought I'd be doing an internship in September this year, I'd probably come across something like this.

I didn't bother to talk hehe

Hee-hee, I hope it helps, thank you

The answer on the ground floor is good! I'm not here to answer the question. I'm here to give advice.

Some of the equations under acidic conditions are water on the left and hydrogenation ions on the right. According to him. This kind of can't be matched at all.。。

And CE is easy to hydrolyze, and you have to be strongly acidic to ensure that it is CE4+!.

So.. Landlord.. College students (postgraduates?) Although the professional knowledge is strong, there are many times when it is not standardized. So.. Kindness.. I still listen to the teacher. Kindness..

The equation is as follows.

2ce4+ +no2- +h2o == 2ce3+ +no3- +2h+

5nano2+2kmno4+3h2so4 =5nano3+2mnso4+k2so4+3h2o

Sodium nitrite is oxidized to sodium nitrate, and manganese in potassium permanganate is reduced from positive heptavalent to positive bivalent.

Sodium nitrite is oxidized to sodium nitrate, and the reduction product of KMno4 under acidic conditions is Mn2+

5 nano2 + 2 kmno4 + 3 h2so4 = 5 nano3 + 2 mnso4 + k2so4 + 3 h2o

5 no2- +2 mno4- +6 h+ = 5 no3- +2 mn2+ +3 h2o

The answer is C;

A is wrong, NO2- becomes NO3-, the valency of N increases from +3 to +5 is a reducing agent, B is wrong, it is constantly consumed, the concentration of H+ decreases, and the pH increases. It is important to know that the weaker the acidity of the acid, the greater the pH. C pair, +7 mno4- becomes +2 mn2+, Mn decreases from +7 to +2 and decreases pentavalent, so 5mol electrons D error is obtained, NO3- is an oxidation product, the oxidation is less than Mno4-, and the oxidation of the oxidant is greater than the oxidation of the oxidation product.

A is wrong, NO2- becomes NO3- the increase in valency is the reducing agent B is wrong, H+ is constantly consumed, the concentration decreases, and the pH becomes larger.

C pair, +7 mnO4- becomes +2 mn2+, 5mol electron D error is obtained, NO3- is an oxidation product, and the oxidation is less than that of Mno4-

KMno4 is a strong oxidant under acidic conditions, and its strength exceeds that of nitric acid, which is also shown by the reaction formula above. In the reaction, permanganate acts as an oxidizing agent and nitrite acts as a reducing agent, and this reaction consumes the acid (H ions) in the reaction, and the pH increases, so the answer comes out, c.

If I'm not mistaken, this is a high school redox reflection chemistry, which belongs to the basics, so take a good look at the connection.

The answer is c, a oxidant is permanganate ion.

b Consumption of hydrogen ions PH increases.

d The oxidizing property of the oxidant is greater than that of the oxidation product.

The anions produced when an acid is ionized are acid ions. Acid radicals are generally divided into strong acid and weak acid roots. The former includes sulfate, hydrochloride, nitrate, etc., which are basically inorganic acids.

The latter includes carbonate, acetate, oxalate, etc. Except for carbonate, which is basically an organic acid.

Common acid ions are:

Carbonate CO3 -2 valence Sulfur Ion Constant -2 Valence Sulfate SO4 -2 Valence Sulfite SO3 -2 Valence Phosphate PO4 -3 Valence Permanganate MNO4 -1 Valence Manganate MNO4 -2 Valence Chloride Constant -1 Valence Chlorate Clo3 -1 Valence Chlorite CLO2 -1 Valence Hypochlorite CLO -1 Valence Perchlorate ClO4 -1 Valence Nitrate NO3 -1 Valence Nitrite NO2 -1 Valence Selenate SELase SEO4 -2 Valence Chromate CRO4 -2 Valence Dichromate Cr2O7 -2 valence Ferritate FeO2 -1 valence Ferritate FeO4 -2 valence Aluminate Alo 3 -3 valence Metaaluminate Alo 2 -1 valence Hydrocyanide CN -1 valence Oxalate C2O4 -2 valence.

Common junior high school textbooks:

Carbonate CO3-2 valence, sulfate SO4-2 valence, hypochlorite CLO -1 valence, nitrate NO3 -1 valence.

Hydrogen ions and hydrolysis produce hydrogen ions.

Different theories have different definitions, and high school thought that hydrogen ions and ions that produce hydrogen ions after hydrolysis are sufficient.

The acidity is H+, which is the hydrogen ion.

The opposite is oh-, which is hydroxide.

Hydrogen ions and ions or ion clusters that produce hydrogen ions after hydrolysis.