Take sulfuric acid as an example, write the five chemical properties of the acid, and write the chem

1) The acid solution can react with the acid-base indicator. The purple litmus test solution turns red when it meets acid, and the colorless phenolphthalein test solution does not change color when it meets acid. Note that the chromogenic substance is an indicator.

2) Acids react with a variety of reactive metals, usually to produce salts and hydrogen.

For example, Mg2SO4 MgSO4+H2

3) Acids can react with basic oxides to form salts and water: H2SO4CAOCASO4H2O

4) Acids can react with certain salts to form new acids and salts: H2SO4BAC2BASO4+

2HCL5) acid and alkali neutralization reaction to form salt and water: H2SO4 BA(OH)2BASO4 (white precipitate) 2H2O

Chemical properties of dilute hydrochloric acid:

1) Reaction with acid-base indicator:

The purple litmus test solution turns red, and the colorless phenolphthalein test solution cannot be discolored;

2) Lively metal. Dilute salt. Sour.

Salt. Hydrogen. Zn+2HCl=ZnCl2+H2 (gas).

3) Basic oxides. Dilute salt. Sour.

Salt. Water. cuo+2hcl=cucl2+h2o

4) Alkali. Dilute salt. Sour. Salt.

Water. naoh+hcl=nacl+h2o

5) Salt. Dilute salt.

Sour. Another salt.

Another acid (the product is eligible for metathesis).

AgNO3 + HCl = AGCL (precipitate) + HNO3

The chemical formula of sulfuric acid is as follows:

Analysis: SO4 represents sulfate ions (clusters) with a valency of -2. The chemical formula of any acid ion remains unchanged, but to become an acid atom, as long as h is added before the acid ion, it becomes an acid atom.

But the valency of H is +1, and to make the valency of the whole chemical formula 0, there must be 2 H atoms, so the chemical formula of pure sulfuric acid is H2SO4.

Sulfuric acid is one of the most reactive binary inorganic acids that reacts with most metals. High concentration of sulfuric acid has strong water absorption, can be used as a dehydrating agent, carbonized wood, paper, cotton and linen fabrics and biological skin and other carbohydrate-containing substances. When mixed with water, a large amount of heat energy is also emitted.

It is highly corrosive and oxidizing.

Pure sulfuric acid is generally a colorless oily liquid with a density; , boiling point 337, can be miscible with water in any proportion, and at the same time release a large amount of heat, so that water boils. When heated to 290, sulfur trioxide is released, and finally becomes an aqueous solution, which boils at 317 and becomes an azeotropic mixture.

The high boiling point and viscosity of sulfuric acid are due to the strong hydrogen bonds inside its molecules. Due to the higher dielectric constant of sulfuric acid, it is a good solvent for electrolytes, whereas solvents as a non-electrolyte are less ideal. The melting point of sulfuric acid is that the freezing point will decrease when added to water or sulfur trioxide.

The chemical formula of sulfuric acid is written: h so.

It should be noted that concentrated sulfuric acid and dilute sulfuric acid are both mixtures of sulfuric acid and water, and only pure sulfuric acid is pure.

Both SO2 and SO3 are SP2 hybridizations. According to the VSEPR theory, sulfur donates six electrons and oxygen as a coordination atom does not donate electrons, 6 2 = 3, so it is both sp2 hybridized, there is no doubt about this. Regarding the molecular configuration (not electron pairs), SO2 is V-type and SO3 is planar regular triangle.

Sulfur is a sp2 planar triangular structure, because it is combined with three oxygen, there must be at least 3 orbitals, and the outermost shell of sulfur has 6 electrons, if the oxygen atom combines two electrons each, it reaches a steady state, and there is no lone pair of electrons, and the lone pair of electrons no longer needs to occupy the orbital, so only three orbital hybridizations are required, which is sp2 hybridization.

The statement on the first floor is basically correct, but it should be clear that the industrial production of sulfuric acid is to pass SO3 into dilute sulfuric acid to make concentrated sulfuric acid and then dilute it. If it is directly introduced into the water, the utilization rate of SO3 is not high, and some of them may become bubbles and bubble out, and there is a risk of boiling and splashing. And dilute sulfuric acid will not.

As for other acids, this is not the case. For example, if you take nitric acid, the reaction formula is H2SO4(L) + Na3(S) = > Na2SO4(S) + HNO3(G), which is a laboratory method. The industrial method is 3NO2 + H2O ==2HNO3 + NO.

Hydrochloric acid, for example, is ignited with hydrogen and chlorine to produce HCl gas, which is then introduced into water. The laboratory method is 2Naci (solid) + H2SO4 (concentrated) = Na2SO4 + 2HCI Condition: heating.

Supplement: Laboratory sulfuric acid method.

It can be strengthened with heat, condensed with ice-water mixture + U-shaped tube, and SO2 can be absorbed with NaOH, and the theoretically available H2SO4 can be obtained

S+O2 = Ignition = SO2

If SO2 is further oxidized, sulfuric acid is formed, usually in the presence of a catalyst.

2SO2+O2 === 2SO3 (heating, vanadium pentoxide as catalyst, reversible) SO3+H2O===H2SO4

Sulfur is also called bisulfate according to the chemical formula.

Category: Acid Yumin.

The chemical formula of sulfuric acid is H2SO4.

Sulfuric acid is a common inorganic acid with the chemical formula H2SO4. It consists of 2 hydrogen atoms, 1 sulfur atom, and 4 oxygen atoms. In the air, sulfuric acid is a colorless, toxic, viscous liquid that can be dissolved in water and is strongly corrosive and acidic.

In practical production and application, sulfuric acid has important chemical and industrial uses, and is widely used in pharmaceutical, chemical, metallurgy, textile and wastewater treatment fields.

Sulfuric acid is an important inorganic chemical with a wide range of applications in various industries. When using sulfuric acid, it is necessary to pay attention to its strong corrosive and acidic nature, and appropriate safety measures must be taken to avoid direct contact with or inhalation of its vapors. When storing and transporting sulfuric acid, it is also necessary to follow the corresponding regulations and standards, select appropriate containers and storage conditions to ensure its safety and stability.

1) The acid solution can react with the acid-base indicator. The purple litmus test solution turns red when it meets acid, and the colorless phenolphthalein test solution does not change color when it meets acid. Note that the chromogenic substance is an indicator.

2) Acids react with a variety of reactive metals, usually to produce salts and hydrogen.

For example, Mg2SO4 MgSO4+H2

3) Acid can react with basic oxides to form salt and water: H2SO4 + CAO

CaSO4H2O4) acid can react with certain salts to form new acids and new salts: H2SO4+BACl2

=baso4↓+

2HCL5) acid and alkali neutralization reaction to form salt and water: H2SO4 BA(OH)2BASO4 (white precipitate) 2H2O

Chemical properties of dilute hydrochloric acid:

1) Reaction with acid-base indicator:

The purple litmus test solution turns red, and the colorless phenolphthalein test solution cannot be discolored;

2) Lively metal.

Dilute hydrochloride salt.

Hydrogen zn + 2HCl = ZnCl2 + H2 (gas).

3) Basic oxides.

Dilute hydrochloride salt.

Water CuO+2HCl=CuCl2+H2O

4) Alkali. Dilute hydrochloride salt.

Water NaOH + HCl = NaCl + H2O

5) Salt. Dilute hydrochloric acid.

Another salt. Another acid (the product is eligible for metathesis).

AgNO3 + HCl = AGCL (precipitate) + HNO3

1) The acid solution can react with the acid-base indicator. The purple litmus test solution turns red when it meets acid, and the colorless phenolphthalein test solution does not change color when it meets acid. Note that the chromogenic substance is an indicator.

2) Acids react with a variety of reactive metals, usually to produce salts and hydrogen.

For example, Mg2SO4 MgSO4+H2

3) Acids can react with basic oxides to form salts and water: H2SO4CAOCASO4H2O

4) Acids can react with certain salts to form new acids and salts: H2SO4 + BACL2 === BASO4 + 2HCl

5) Acid and alkali neutralization reaction to produce salt and water: H2SO4 BA(OH)2 === BASO4 (white precipitate) 2H2O