Both HCl and H2SO4 are completely ionized, why is the latter highly acidic

The so-called complete ionization refers to the vast majority of ionization, which is not really "complete ionization".

There are still a small amount of HCL molecules in HCl, but this amount is very small and can be ignored. And sulfate.

One step is completely ionized, so it is said that sulfuric acid is more acidic than hydrochloric acid.

In fact, sulfuric acid is not really completely ionized, although the first step of sulfuric acid is 100 ionization, but the second step of ionization is not completely ionized, but in a relatively dilute solution, the degree of ionization is close to 100, so it is generally considered that sulfuric acid is completely ionized.

The strongest acid, perchloric acid, is the strongest acid because it ionizes more completely than them.

The acidity of the two is actually very close.

The reason why sulfuric acid is highly acidic is because concentrated sulfuric acid has strong oxidizing properties.

Sulfuric acid is a strong acid, it can completely ionize the 2 H ions contained in it, so the ammonium bisulfate solution contains a large number of H ions, and the solution is acidic.

1. HSO4- is a strong acid, which can be completely ionized into H+ and SO4 (2-).

2. The hydrolysis of NH4+ can indeed produce H+, but this is a very small part.

Because the book tells us that no matter what God Ma Dongdong, the degree of hydrolysis is very small, generally within 1%.

Analysis: NH4HSO4 distributed ionization:

Step 1, Complete Ionization:

NH4HSO4 NH4+ + HSO4 - Second step, partial ionization:

HSO4- H+ +SO4)2- (denotes reversible symbol) while NH4 ions are also hydrolyzed in small amounts:

The degree of ionization of NH4+ + H2O NH3·H2O + H+HSO4- is much greater than that of NH4+ hydrolysis, and inhibits NH4+ hydrolysis to a certain extent.

Therefore, it can be assumed that H+ in solution is mainly produced by HSO4 ionization.

Note: HSO4- is considered to be fully ionized in the middle school range.

HCl and H2SO4 are electrolytes in any condition as long as they are pure (solutions are not OK).

Liquid HCl, gaseous HCl, and H2SO4 are all electrolytes.

But concentrated sulfuric acid, hydrochloric acid is not an electrolyte, nor is it a non-electrolyte. They are mixtures.

Whether a substance is an electrolyte or not is independent of the form in which the substance exists.

A substance is an electrolyte, and its solution or molten state must be able to conduct electricity, but this state of the substance is not necessarily conductive.

For example, solid KNO3 is an electrolyte, and the KNO3 solution conducts electricity, but the solid KNO3 does not.

From strong to weak: hclo4

hno3h2so4

HCO4 is the most acidic of the oxygenated acids.

The non-metallic properties of N are stronger than S, so.

hno3h2so4

The acidity of an acid mainly depends on how easy it is to produce hydrogen ions, and if it is easy to produce hydrogen ions, then it is very acidic. It's not easy, it's not strong. Concentrated sulfuric acid is mainly present in sulfuric acid molecules, that is, hydrogen ions are difficult to ionize out.

Then he is not a strong acid at this time; Concentrated sulfuric acid is diluted, and the ability to ionize hydrogen ions is enhanced, so it becomes a strong acid.

The oxidation of the acid should be regarded as the valency of the acid element. The higher the valency and the higher the number of electrons that can be obtained, then the stronger the oxidation. For example, the acid-forming element in Hno3 is nitrogen, with valency +5, high valency, strong electron acquisition ability and strong oxidation.

In HCl (which has a strong ability to ionize hydrogen ions and is a strong acid), the acid-forming element Cl shows negative monovalent and has no ability to gain electrons in the lowest valence state. Therefore, it is not oxidizing. That is, non-oxidizing acids.

As can be seen from the above, acidity and oxidation of acids refer to different aspects. So be clear!

To add, whether the strong electrolyte or the weak electrolyte depends on whether the part dissolved in water is completely ionized. If it is, then it is a strong electrolyte, and concentrated sulfuric acid exists in molecular form and only a small amount is ionized, so it is not a strong electrolyte. Another example, barium sulfate, although it is a precipitate, but its slightly soluble in water part is completely ionized to form sulfate and barium ions, so it is a strong electrolyte!

Concentrated sulfuric acid is equivalent to sulfuric acid is the solution, water is the solute, and dilute sulfuric acid is equivalent to water is the solution, and sulfuric acid is the solute. Electrolysis is the conduct of electricity, and the conduction seems to be a free ion ......It's a hassle to explain, and I've been away from high school for many years.

Except for a few such as sulfuric acid, most of the other strong acids and alkalis are.

Isn't concentrated H2SO4 a strong electrolyte?

Definition of electrolyte: A compound that conducts electricity in an aqueous solution or in a molten state.

Weakly ask——— is concentrated sulfuric acid a chemical compound? Not a mixture?? (Since there is a concentration difference, there should only be a mixture).

Speaking of which——— mixture does not fit the definition.

And sulfuric acid alone has two meanings,1Sulfuric acid solution (certainly not an electrolyte) 2Sulfuric acid molecule (electrolyte correct).

..PS: Please read the chemical definition clearly in the future, and then ask OK ???

Concentrated sulfuric acid molecules have strong oxidation and dehydration, so concentrated sulfuric acid cannot be disassembled. Strong oxidation means that it is very easy to obtain electrons, so it will catch hydrogen ions, so it cannot be electrolyzed. The dehydration of concentrated sulfuric acid means that when it forms a solution, there is very little water in the solution, and it is even less likely to be separated as an ion in the case of near anhydrous.

Strong electrolytes are remembered Six strong acids: hydrochloric acid, dilute sulfuric acid, nitric acid, hydrogen bromide, iodine bromide, perchloric acid, four strong bases: potassium, sodium, calcium, barium, and soluble salts These are all detachable, and the rest are weak electrolytes like elemental oxides, weak acids, weak alkalis, and water.

Strong acids, strong bases, and tolerant salts in an aqueous solution or in a molten state are strong electrolytesDefinition of electrolyte: An electrolyte is a compound that can conduct electricity (electrolyze into cations and anions) and produce chemical changes when dissolved in an aqueous solution or in a molten state. So sulfuric acid is a strong electrolyte, whereas concentrated sulfuric acid is not a strong electrolyte.

It's too complicated, and it's very professional.