Why is the strongest acid in aqueous solution H3O in acid base proton theory?

Note that H30+ is not the strongest acid, its PKA=1, it can only be said that other strong acids such as H2SO4 in aqueous solution are also PKA=1, that is, the accurate PKA of H2SO4 cannot be measured, so H2O is a leveling solution of strong acids such as H2SO4 and H3O+, you can learn about the leveling effect and the discrimination effect.

H30+ is not the strongest acid.

H2SO4 and H20 produce H30+ and Hs04-

So in the proton theory, H2SO4 is of course more acidic than H30+.

CH3NH2 is a protonic acid.

As long as it is an amine, it can bind protons, because there are lone pairs of electrons on n, so CH3NH2 (methylamine.

is a Bronster base, judging by the definition. Protons are slightly lighter than neutrons. Protons belong to the baryon class and are made up of two upper quarks and one lower quark by gluon in a strong interaction. Nucleus.

The number of protons determines the type of element and it belongs to the chemical element of the species of Haozhi Heyouli.

Limitations. The acid-base ion theory was developed by Arrhenius based on his theory of ionization, which states that hydrogen ions can be ionized in water and no other cations are produced.

The substance is called acid. Hydroxide ions can be ionized in water and no other anions are produced.

The substance is called a base. The essence of the acid-base neutralization reaction is the combination of hydrogen ions and hydroxide ions into water.

This theory is classic, but it has some limitations because its description of acids and bases is limited to aqueous solutions. For example, ammonium chloride.

The aqueous solution is acidic, but it does not contain hydrogen ions per se; For example, the aqueous solution of ammonia is alkaline, and it was erroneously believed that NH3 and H2O form weak electrolytes.

NH4OH molecule, which is then dissociated to OH-etc.

The above content refers to: Encyclopedia - acid-base proton theory.

In acid-base proton theory, the macro-change that accepts protons is acid. （）

a.Cover the eggplant properly.

b.Wrong hail mistake.

Correct answer: B

The strength of an acid refers to its ability to ionize hydrogen ions in water, and the more completely ionized it is, the more acidic it is.

In fact, hydrogen ions in water do not exist as a single hydrogen atom with a positive charge, that is, not in the form of H+, but in the form of hydrogen hydrate ions (H3O+), we just abbreviate it as H+, in this sense, hydrogen hydron ions are acids that can ionize hydrogen ions (itself) 100% (a bit like nonsense), of course, the strongest acid.

By extension, solvated protons are the most acidic.

In the aqueous solution, if there is an acid stronger than the hydronium hydrate ion, the water will be atomized to form the hydronium hydride ion, so as long as it is a stable aqueous solution, there will be no acid stronger than the hydronium hydrate ion.

In aqueous solutions, any acid that is more acidic than H3O+ is flattened to the level of H3O+ through the leveling effect of water. In other words, H3O+ is the strongest form of acid that can be present in an aqueous solution.

The leveling effect is also known as the leveling effect. Through the action of solvents, acids or bases of different strengths show the effect of equal strength.

For example, hydrochloric acid, nitric acid, and perchloric acid have different acid strengths in glacial acetic acid (i.e., different acidity), but when water is used as a solvent, it is difficult to distinguish their acid strength (it can be assumed that they are all strong acids, and their acidity is the same). This is due to the fact that water has a greater affinity for protons, which masks the difference in the ability of these acids to give protons, and flattens out the different strengths of these acids. Similarly, when dimethylamine and aniline are dissolved in formic acid, the strength of these two bases is flattened due to the strong ability of formic acid to donate protons.

The study of the leveling effect is helpful to understand the influence of solvents on acid-base strength, and has certain significance in chemical research.

According to the acid-base proton theory, the strength of an acid or base exhibited by a substance in a solution is related not only to the nature of the acid-base but also to the nature of the solvent. For example, HCO4 is a strong acid in water and tends to be completely dissociated, but it cannot be completely dissociated in glacial acetic acid.

Water is not the only solvent, if S is used to represent any solvent, the dissociation equilibrium of acid Hb in it is .

hb+s--〉hs++b-， hb+hac--〉h2ac-+b-

Experiments show that there is a difference in the acid strength of HCO4, H2SO4, HCl>HNO3 in the order of HCO4>H2SO4>HClHno3, and the difference in their strength can not be seen in aqueous solution.

This is because strong acids have a strong ability to give protons in aqueous solution, and the alkalinity of water is sufficient to accept the protons given by these acids, as long as the concentration of these acids is not too large, then they will quantitatively interact with water and all be converted into H3O+, i.e.

hclo4+h2o, h3o++clo4-, etc.

That is, the intensity of their acids is all flattened to the level of H3O+, and this effect of leveling the acids of different strengths to the level of solvated protons (in this case, hydrated protons H3O+) is called the leveling effect. Solvents that have a leveling effect are called leveling solvents. Here, water is the leveling solvent for HCO4, H2SO4, HCl, and HNO3.

Whether it is a strong acid or a weak acid, the hydrogen ions ionized in water are in the form of hydronium ions in solution, and the H+ we usually see is just a shorthand for hydronium ions.