How to distinguish between strong and weak salts and strong and weak alkali salts

In middle school chemistry, acid is composed of acid ions and hydrogen ions, while alkali is composed of metal ions and hydroxide ions (ammonia monohydrate is special, it is composed of ammonium and hydroxide), the fundamental difference between strong acid and weak acid is whether acid and base can be completely ionized in water, that is, whether acid can be completely ionized into acid ions and hydrogen ions, if it can, then this acid is a strong acid, if not, then it is a weak acid. Whether the alkali can be completely ionized into metal ions and hydroxide ions, if it can, then this alkali is a strong base, if not, then it is a weak base.

Common strong acids: H2SO4, Hi, HBR, HCl, HNO3

Common strong bases: Naoh, Koh, Ba(OH)2, Ca(OH)2, etc.

Common weak acids: HCl, H2CO3, H2SO3, etc.

Common weak bases: NH3 H2O, Cu(OH)2, Fe(OH)2, Fe(OH)3, Al(OH)3, etc.

Salt is the product of the reaction between acid and base, and is composed of acid and metal ions (ammonium salt is composed of ammonium and acid group).

For example, NaCl, the base corresponding to Na is NaOH (strong base), and the acid corresponding to Cl is HCL (strong acid), which is a strong acid and strong alkali salt.

Strong acid: hydrochloric acid, sulfuric acid, nitric acid, etc., the acid ions containing them in the salt are strong salts, weak acids: carbonic acid, acetic acid, phosphoric acid (medium strong acid, also considered weak acid), salt contains their acid ions is weak salt, strong alkali:

KOH, NaOH, BA (OH), etc., the metal cations containing them in the salt are strong alkali salts, weak bases: NH3*H2O, Fe(OH)3, AL(OH)3, Cu(OH)2, etc., and the cations containing them in the salt are weak alkali salts, such as sodium sulfate, which are strong acids and strong alkali salts.

Sodium carbonate is a strong base and weak salt.

Ferric chloride is a strong acid and weak alkali salt.

My chemistry isn't very good! After you read it, think about it yourself, you have to be familiar with the periodic table when you ask this question! From left to right, the metallicness gradually decreases!

Grow from top to bottom! The stronger it is, the less likely it is to hydrolyze! Ammonia and halogens are acidic!

Because of ammonia hydrolysis! Hydrogen root is generated! That's acidic!

The alkalinity of beryllium ions is less than that of magnesium ions, and it is also less than sodium I....

The main thing is to look at the things that are combined. Look at nak

ca these elements have a high period.

Electrons are very free.

Hydroxide is combined.

That's a strong alkali.

The strong acid that high school talks about is generally that.

Sulphuric acid. Hydrochloric acid.

Nitric acid these 3.

Nothing else is said.

The first one is very professional. I won't talk about it. Hehe.

1. Strong acid and alkali salt.

Strong acid and strong alkali salt is a salt formed by the reaction of strong acid and strong base, and the solution is generally neutral.

For example: sodium chloride, sodium sulfate, potassium nitrate.

naoh+hcl=nacl+h2o

2naoh+h2so4=2h2o+na2so4

2. Strong acid and weak alkali salt.

Strong acid and weak alkali salt are salts produced by the reaction of strong acids and weak bases.

For example: copper sulfate.

cuso4=cu2+ +so42-

cu2+ +2h2o⇌cu(oh)2 + 2h+ [2]

Soluble in water is acidic, such as: copper sulfate, ferric chloride, ammonium chloride, aluminum chloride, iron sulfate.

3. Strong alkali and weak salt.

Strong alkali weak salts are salts formed by the reaction of strong bases and weak acids.

For example: sodium carbonate.

na2co3 = 2na++co32-

co32-+h2o ⇌ hco3- +oh-

hco3- +h2o ⇌ h2co3 +oh-

Soluble water is alkaline, such as sodium carbonate, sodium acetate, sodium phosphate, sodium bicarbonate.

4. Weak acid and weak alkali salt.

Weak acid and weak alkali salt is a salt formed by the reaction of weak acid and weak base, and the acidity and alkalinity are determined by the relative strength between weak acid and weak base.

For example: ammonium carbonate, ammonium acetate, copper sulfide.

This salt can be dissolved in water and pH test paper can be used to test the acidity and alkalinity of the solution.

If the solution is acidic, it means that it is a strong acid and weak alkali salt;

If the solution is alkaline, it means that it is a strong base and weak salt;

Weak acid and weak alkali salts should be judged and determined according to the specific composition and pH of the solution.

Generally, the acidity and alkalinity of salt aqueous solution can judge the composition of acid and alkali, and the law is: who is weak and who is hydrolyzed, who is strong and who is strong, and the weaker the hydrolysis.

First of all, this substance must be salt, not salt Do not make this judgment.

After that, you swap out the cation of this substance for H+ and see if it is a strong or weak acid (strong acid is a weak acid to see if it is completely ionized in water).

Then, the cation remains unchanged, and the anion is replaced with oh-, to see if it is a strong or weak base, and the same is to ask whether it is completely ionized.

For example: Na Co, we first replace the cation with H+ to get H Co, and the carbonic acid is obviously a weak acid.

Then we change the anion to OH-, and we find that it is NAOH and sodium hydroxide is of course a strong base.

So it's a strong base and weak salt.

I guess you mean the classification of salt. Salt can be divided into 4 categories according to the ** of acid-base neutralization: strong acid and strong alkali salts (such as NaCl, KNO3, etc.), strong acid and weak alkali salts (such as NH4Cl, MGSO4, etc.), weak acid and strong alkali salts (such as NaAC, Na2S, etc.), weak acid and weak alkali salts (such as NH4AC, NH4HCO3, etc.).

When put into water, if it is acidic, it is generally a strong acid and weak alkali salt, and if it is alkaline, it is generally a strong alkali and weak salt.

Test strips bought at chemical stores are measurable.

1. Strong acid and strong alkali salt, the salt generated by the reaction of strong acid and strong alkali, the solution is generally neutral. For example: sodium chloride, sodium sulfate, potassium nitrate.

2. Strong acid and weak alkali salt, salt formed by the reaction of strong acid and weak alkali. For example: copper sulfate.

3. Strong alkali and weak salt, strong alkali and weak acid are salts produced by the reaction of strong alkali and weak acid. For example: sodium carbonate.

4. Weak acid and weak alkali salt, the salt formed by the reaction of weak acid and weak base, the acidity and alkalinity are determined by the relative strength between weak acid and weak base. For example: ammonium carbonate, ammonium acetate, copper sulfide.

1. Strong alkali and weak acid are salts formed by the reaction of strong alkali and weak acid. Because acid ions or non-metal ions consume part of the hydrogen ions in the hydrolysis and ionize hydroxide ions, the solution is weakly alkaline.

For example, sodium carbonate:

na2co3 = 2na++co32-

CO32- +H2O = invertible number = HCO3- +OH-

hco3- +h2o = h2co3 +oh-

Dissolved water is alkaline, such as sodium carbonate, sodium acetate, sodium phosphate, sodium acetate.

Weak acid ions: such as carbonate ion CO32-, sulfite ion SO32-, hydrosulfate ion S2-, silicate SIO32-, metaaluminate ALO2-, acetate CH3COO-, etc.

Strong base ions: such as Na+, K+, Ca2+, Ba2+, etc.

Sodium hypochlorite (Naclo) is also a strong base and weak salt.

2. Strong acid and weak alkali salt are salts produced by the reaction of strong acid and weak base. Because metal ions or ammonium ions consume a part of the hydroxide ions in hydrolysis and ionize hydrogen ions, the solution is weakly acidic. [1]

For example, copper sulphate:

cuso4=cu2+ +so42-

Cu2+ +2H2O=Reversible=Cu(OH)2+2H+[2].

Soluble in water is acidic, such as: copper sulfate, ferric chloride, ammonium chloride, aluminum chloride, iron sulfate.

Strong acids: six inorganic strong acids in chemistry.

Sulfuric acid, nitric acid, hydrochloric acid (hydrochloric acid), hydroiodic acid, hydrobromic acid, perchloric acid.

The eight strong acids in high school chemistry include the six inorganic strong acids, chloric acid, and permanganic acid.

Weak alkali: NH3·H2O (ammonia monohydrate).

Alkalis that are insoluble in water, such as Fe(OH)3, Cu(OH)2, Mg(OH)2, Al(OH)3

Strong alkali weak salts are salts formed by the reaction of strong bases and weak acids. Because acid ions or non-metal ions consume part of the hydrogen ions in the hydrolysis and ionize hydroxide ions, most of the strong alkali and weak acid solutions are alkaline, but there are also special cases, such as sodium bisulfite aqueous solution.

Soluble water is alkaline, such as sodium carbonate, sodium acetate, sodium phosphate, sodium bicarbonate. Sodium hypochlorite (Naclo) is also a strong base and weak salt.

1. Weak acid ions: such as carbonate ions, sulfite ions, hydrosulfate ions, silicate, metaaluminate, acetate, etc.

2. Strong base ions: such as Na+, K+, Ca2+, Ba2+, etc.

These terms relate to the classification of salt, which are explained as follows:

1. Strong acid and strong alkali slow residual salt: Refers to a salt composed of cations and anions in strong acids and bases. These salts are completely dissociated in water, resulting in a solution that is neutral.

Example cavity rollers: sodium chloride (NaCl), potassium sulfate (K2SO4), ammonium nitrate (NH4NO3), etc.

2. Strong acid and weak alkali salt. : Refers to a salt composed of cations and anions in strong acids and weak bases. These salts also dissociate in water, but the solution is acidic.

Examples: ammonium chloride (NH4Cl), ammonium sulfate (NH4HSO4), etc.

3. Weak acid and strong alkali salt: Refers to a salt composed of cations and anions in weak acids and strong bases. These salts dissociate in water, resulting in an alkaline solution.

Examples: sodium acetate (CH3COONA), sodium carbonate (Na2CO3), etc.

4. Weak acid and weak alkali salt. : Refers to a salt composed of cations and anions in weak acids and bases. The degree of dissociation of these salts in water is low, and the acidity and alkalinity of the solution depends on the weak acid and the weak nucleus of the weak base.

Examples: sodium biacetate (CH3COOH + NaHCO3), etc.

It is important to note that while these salts affect the acid-base properties of the solution when dissolved in water, they do not necessarily exhibit significant acid-base properties in the solid state.