Commonality of acidic oxides, using equations

Acidic oxides (non-metallic oxides): any oxide that reacts with alkali to form salts and water.

Acidic oxide + base --salt + water.

Caustic soda deteriorates when exposed to air: 2NaOH + CO2 ==== Na2CO3 + H2O

Caustic soda absorbs sulfur dioxide gas: 2NaOH + SO2 ==== Na2SO3 + H2O

Caustic soda absorbs sulfur trioxide gas: 2NaOH + SO3 ==== Na2SO4 + H2O

Slaked lime deteriorates when placed in air: Ca(OH)2 + CO2 ==== CaCO3 + H2O

Slaked lime absorbs sulfur dioxide: Ca(OH)2 + SO2 ==== CaSO3 + H2O

Acidic oxide + water --- acid.

co2+h2o===h2co3

so2+h2o==h2so3

so3+h2o===h2so4

Acidic oxide + base --salt + water.

1. Carbon dioxide is passed into the clarified lime water: CO2 + Ca(OH)2 ==CaCO3 + H20

2. Calcium hydroxide and sulfur dioxide reaction: SO2 + Ca(OH)2 ==CaSO3 + H20

3. Calcium hydroxide and sulfur trioxide reaction: SO3 + Ca(OH)2 ==CaSO4 + H20

4. Reaction of sodium hydroxide and carbon dioxide (removal of carbon dioxide): 2NaOH + CO2 ==== Na2CO3 + H2O

5. Sodium hydroxide and sulfur dioxide reaction (removal of sulfur dioxide): 2NaOH + SO2 ==== Na2SO3 + H2O

6. Reaction of sodium hydroxide and sulfur trioxide (removal of sulfur trioxide): 2NaOH + SO3 ==== Na2SO4 + H2O

Acidic oxides.

Reacts with water to form the corresponding acid SO3+H2O=H2SO42Reacts with alkali to form salt and water 2NaOH+CO2=Na2CO3+H2O3

It reacts with basic oxides to form salts CO2+cao==caCO3 basic oxides1It reacts with water to form the corresponding base CaO+H2O==Ca(OH)22Reacts with acid to form salt and water CaO+2HCl==CaCl2+H2O3

React with acidic oxides to form salt Na2O+CO2=Na2CO3 Remember one thing that the valency of any element in the reaction is constant.

Acidic oxides react with basic oxides to form salts CO2+MGO=MGO3 acidic oxides.

1.Reacts with water to form the corresponding acid SO3+H2O=H2SO42

2.Reacts with alkali to form salt and water: CO2+2NaOH=Na2CO3+H2O.

3.Salt and water corresponding to the production of basic oxides: CO2 + MGO = MgCO3 basic oxides.

It reacts with water to form the corresponding alkali CaO+H2O==Ca(OH), reacts with acid to form salt and water CaO+H2SO4==CaSO4+H2O reacts with acidic oxides to form salt Mgo+CO2=MgCO3

Acidic oxides.

1. React with water to form the corresponding acid (except for silica SiO2, which does not react with water), most of the acidic oxides can be directly combined with water to form oxygenated acid. CO2 + H2O = (reversible) H2CO3

so3+h2o=h2so4

2.Reacts with alkali to form salt and water.

co2+2naoh=na2co3 +h2o3.Reacts with basic oxides.

co2+na2o=na2co3

Basic oxides.

1.A small number of basic oxides react with water.

Alkali metals such as sodium and potassium, as well as oxides of calcium and barium can react with water to form corresponding hydroxides. They are all strong bases:

na2o+h2o==2naoh

cao+h2o==ca(oh)2

But Cuo Fe2O3 does not react with water.

2 Partial Alkaline Oxides React with Acidic Oxides:

na2o+co2==na2co3

cao + siO2 = high temperature = casio3

3.Basic oxides can also react with acids.

na2o+h2so4===na2so4+h2o

1: Acidic oxides are a class of oxides that can react with water to form acids or react with alkalis to form salts and water or react with alkaline oxides to form salts.

2: It can react with acid to form an oxide of salt and water called alkaline oxide.

3: Oxides that can react with acids to form salt and water and alkali to form salt and water are called amphoteric oxides.

4: Haven't heard of alkali salt oxides.

It shouldn't be a salt oxide, right? Oxides that cannot react with acids or bases to form salts and water in the corresponding valence state are called non-salt oxides.

5: The landlord is a high school freshman, right? In fact, you don't need to understand this concept thoroughly, you just need to write an equation on the spot and you can deduce it.

1. Definition of acidic oxides.

Any oxide that can react with alkali to form salt and water is called an acid oxide.

For example: CO2 + 2NaOH = Na2CO3 + H2O SO3 + Ca(OH)2 = CaSO4 + H2O

Therefore, CO2 and SO3 are acidic oxides. Acidic oxides are also known as oxytic anhydrides.

In terms of element composition, most of the acid oxides are non-metal oxides, and there are also a few metal oxides.

Among the common non-metallic oxides, in addition to CO and H2O, most of them are acid oxides, such as CO2, SO2, SO3, P2O5, SiO2, etc.

Most acidic oxides can be directly combined with water to form corresponding acids (except SiO2).so3 + h2o = h2so4 co2 + h2­o = h2co3 so2 + h2o = h2so3

Comments] Non-metallic oxides are not necessarily acidic oxides; Such as NO, CO (non-salt oxide), NO2, N2O4, H2O

Acidic oxides are not necessarily non-metallic oxides; Such as Mn2O7, CRO3

Anhydride is not necessarily an acidic oxide; Such as acetic anhydride (CH3CO) 2O, etc.

Acidic oxides must be anhydrides.

NO2 - due to the reaction with the alkali not only to produce salt and water, but also NO, so not acidic oxides;

Not all acidic oxides react directly with water to form the corresponding acid. Such as SIO2

An oxide that does not react with water to form an acid must be the anhydride of the acid, such as NO2

2. Properties of acidic oxides.

1) It can quickly synthesize with water to form the corresponding oxygenated acid, which is very stable and not easy to decompose.

s03+h20na2si03+h2o

na2si03+2hcl+h20＝＝＝h4si04↓+2nacl

orthosilicic acid) H4Si04 H2Si03 + H20

Silicic acid) 4) Reaction of acidic oxides with bases:

c02+ca(oh)2＝＝＝cac03↓+h20

If there is an excess of oxides, the reaction can continue to form acid salts

cac03 ca(hc03)2

5) Reaction of acidic oxides with salts:

si02+na2c03na2si03+c02↑

Most acid oxides are non-metallic oxides; A few are also metal oxides, such as Mn2O7; However, a few non-metallic oxides, such as C0 and N0, are not acidic oxides, but not salt oxides.

Anhydride is not necessarily an acidic oxide, such as acetic anhydride (CH3CO) 20, etc.; Acidic oxides must be anhydrides. N02 - due to the reaction with the base not only to form salt and water, but also N0, so it is not an acidic oxide.

Acidic oxides.

Reacts with water to form the corresponding acid (except.

Silicon dioxide. SiO2, which does not react with water).

Acidity. Oxide.

Most of them can be formed directly by combining with water.

Oxyacid. CO2 + H2O = (reversible) H2CO3SO3 + H2O = H2SO4

2.It reacts with alkali to form salt and water.

co2+2naoh=na2co3

h2o3.And.

Basic oxides.

React. co2+na2o=na2co3

Basic oxides.

1.A small number of basic oxides react with water.

Alkali metal. Sodium, potassium, etc., as well as calcium and barium oxides can react with water to form correspondingly.

Hydrogen and tumbling oxides.

They are. Alkali.

na2o+h2o==2naoh

cao+h2o==ca(oh)2

But cuofe2o3

Does not react with water.

2 Partial Alkaline Oxides React with Acidic Oxides:

na2o+co2==na2co3

cao+sio2=

High temperature. casio3

3.Alkaline oxides can react with acids.

na2o+h2so4===na2so4+h2o

Oxidizing acids --- generally oxygenated acids, which refer to the central elements in the acid except hydrogen and oxygen that exhibit strong oxidation in chemical reactions. The more common ones are: concentrated and dilute nitric acid, concentrated sulfuric acid, hypochlorous acid, chloric acid, chlorous acid, perchloric acid, nitrous acid, etc.

Oxygenated acids that are more oxidizing than hydroxide ions have a higher valence state in the acid roots. It is easier to obtain electrons than hydrogen ions in the reaction. Common oxidizing acids include concentrated sulfuric acid, concentrated nitric acid, dilute nitric acid, nitrous acid and oxygenated acids of chlorine, bromine and iodine.

They are higher than hydrogen in terms of the numerical value of the standard electrode potential.

Cu + 2H2SO4 (concentrated) = CuSO4 + SO2 + 2H2O (heated) 3AG+4HNO3 (dilute) = 3AGnO3 + NO +2H2O 2FE+6H2SO4 (concentrated) = Fe2 (SO4)3+3SO2 +6H2O FE+4HNO3 (rare) = Fe(NO3)3+NO +2H2O

Non-oxidizing acids Since most acids can ionize H+ when dissolved in water, hydrogen ions have weak oxidation, so acids have weak oxidation. What we usually call non-oxidizing acids--- refers to acids that exhibit only hydrogen ions in the reaction. Such as:

HCl, HBR, HF, H2CO3, dilute sulfuric acid, phosphoric acid, etc.

Reaction of non-oxidizing acid with aluminum: 2al+6h+=2al3+ +3h2

For example, Hno3, because N in No3 is 5 valence, under H+ acidic conditions, has strong oxidation, then when it reacts with metal, it is not H+ deoxidized metal, but +5 valence N direct oxidation, itself is reduced, its oxidation is much greater than H, and the main thing reflected is the oxidation of N, not the oxidation of H+. This acid is what we usually call oxidizing acid, such as concentrated H2SO4, HNO3, HCO4, HCO3, etc.

For HCl, Hi, HBR, etc., it is a non-oxidizing acid. Note that non-oxidizing acids are not without oxidation, because H+ is also oxidizing, but that its acid roots do not have direct oxidation ability, and only reflect the properties of H+, that is, acidity, but not the oxidation of acid roots.

In addition, some acids are sometimes regarded as oxidizing acids, such as concentrated sulfuric acid, while very dilute dilute sulfuric acid is usually regarded as non-oxidizing acid, that is, the embodiment of the oxidation of the acid group is also related to certain conditions.

Anhydride is defined as an acidic oxide formed when an acid loses water, but it does not mean that an oxide that reacts with water to form an acid is an acid. For example, nitrogen dioxide can react with water to form nitric acid, but it also produces nitric oxide, so it is not an anhydride of nitric acid. Do you understand when I say that?

There is also a way to judge the anhydride, that is, the valency of the anhydride is the same as that of the central element in its corresponding acid. If the valency of the central element in the oxide is not the same as the valency of the central element in the acid, then it must not be the anhydride of the acid.

Acid oxides are a class of oxides that can react with water to form acids or alkalis to form salts and water, but generally do not react with normal salts or acid salts. Generally, it is the oxide of non-metallic elements and the **oxide of certain transition metal elements. For example, sulfur trioxide SO3, phosphorus pentoxide P2O5, manganese heptaoxide Mn2O7, chromium trioxide CRO3, etc.

We know that alkali reacts with acid to form salt and water, and alkali reacts with certain non-metal oxides to form salt and water. For example.

2naoh+co2=na2co3+h2o

Ca(OH)2+SO3=CASO4 +H2OCA(OH)2+SO2=CASO3 +H2O (CaSO4 and CASO3 are both precipitated).

Such non-metal oxides are called acidic.