Weak acid, strong acid, neutral, weak base, strong base, PH value, respectively

The first thing to say is that there is no obvious definition of the strength of the acid and base, and it is impossible to measure it by pH, and you have a wrong understanding of this concept.

Strong acid, weak acid, weak base, and strong base refer to whether the acid and base can be completely ionized or ionized as the standard, and the acid-base concentration can vary greatly, and the pH will also vary greatly.

The pH value corresponds to the concentration of hydrogen ions in the solution. For example, for a low concentration of a strong alkali solution, although the pH of the strong alkali solution is not very large, it is completely ionized in the solution. For example, if the concentration of weak alkali is very large, it can also have a large pH value.

Neutralization is a description of a process in which an acid reacts with a base exactly completely, and the pH range will be in the weakly acidic or weakly alkaline range depending on the ionization ability of the acid-base in which the neutralization action occurs.

In addition, pH is only a description of the pH of a solution where the concentration of hydrogen ions in the solution is in the range, and in other ranges, it can be directly used as hydrogen ion or hydroxide ion concentration, or even acid-base concentration.

Common weak acids: H2CO3 (carbonic acid), HF (hydrofluoric acid, less common), CH3COOH (also known as C2H4O2 acetic acid, also known as acetic acid), H2S (hydrosulfuric acid), HClo (hypochlorous acid), HNO2 (nitrous acid, less common), all organic acids within the middle school range (middle schools do not learn organic strong acids), H2SO3 is also a weak acid Common medium and strong acids: phosphoric acid, oxalic acid, formic acid Common strong acids:

Sulfuric acid H2SO4, HCl hydrochloride, HNO3 nitrate, HBR hydrobromide, HI hydroiodic acid, HCO4 perchloric acid HCO4 Common weak bases: Mg(OH)2, Al(OH)3, Zn(OH)2, Fe(OH)3, Fe(OH)2, Cu(OH)2, only soluble in water. Common strong bases:

koh naoh ba(oh)2 ca(oh)2

Strong acid and strong alkali salt: refers to a salt composed of strong acid and cations and anions in strong base. In aqueous solutions, they completely dissociate to produce acidic and basic ions. For example, sodium chloride (NaCl), sodium sulfate (Na2SO4), etc.

Strong acid and weak alkali salt: refers to a salt composed of cations and anions in strong acids and weak bases. In aqueous solutions, they partially dissociate, producing acid-stealing ions. For example, ammonium chloride (NH4Cl), ammonium nitrate (NH4NO3), etc.

Weak acid and strong alkali salt: refers to the silver salt composed of cations and anions in weak acid and strong base. In an aqueous solution, they partially dissociate, producing basic ions. For example, sodium acetate (CH3COONA), sodium bicarbonate (NaHCO3), etc.

Weak acid and weak alkali salt: refers to a salt composed of cations and anions in weak acids and weak bases. In aqueous solutions, they partially dissociate, producing acidic or basic ions, but they are usually not noticeable.

For example, ethyl acetate (CH3COOC2H5), methyl formate (HCOOCH3), etc.

These are some common examples, but not all:

Strong acids and alkali salts: sodium chloride (NaCl), sodium sulfate (Na2SO4).

Strong acid and weak alkali salts: ammonium chloride (NH4Cl), ammonium nitrate (NH4NO3).

Weak acid and strong alkali salt: sodium acetate (CH3coona), sodium bicarbonate (NaHCO3).

Weak acid and alkali salts: ethyl acetate (CH3COOC2H5), methyl formate (HCOOCH3).

These examples are just some of them, and there are other strong acids, strong bases, weak acids, and weak alkali salts.

Strong acids are acids that are completely ionized in aqueous solution (except for polyacids such as sulfuric acid), or acids with a PKA value of < 6 in terms of acidity coefficient. This value can be understood as the concentration of hydrogen ions under standard conditions is equivalent to the concentration of the solution after the addition of strong acids.

The chemical equation for the complete dissociation of a strong acid in an aqueous solution is given below

ha(aq) →h+(aq) +a�6�1(aq)

Generally, acids do not completely dissociate in water, so they are mostly expressed in the form of chemical equilibrium rather than complete reactions, and weak acids refer to acids that are not completely dissociated. It is not obvious to use the acidity coefficient as a difference between strong and weak acids (because the numerical difference is difficult to understand and not obvious), so it is more reasonable to use the equation to distinguish between the two.

Since the strong acid is completely dissociated in the aqueous solution, the concentration of hydrogen ions in water is equivalent to carrying the acid to other solutions

ha] = [h+] = [a�6�1]；ph = �6�1log[h+]

The KA value of the weak acid is approximately between and or the PKA value is greater than that. Therefore, with the exception of a few acids that are defined as strong acids or superstrong acids, most acids are weak.

··· There is no setting for this.

The pH of dilute acids (bases) approaches 7

The pH of concentrated acids (bases) approaches 1(14).

This is related to concentration, not strength.

The strength of the acid and base is not clearly defined, and it is impossible to measure it by pH.

Strong acid, strong base, weak acid, and weak base refer to whether the acid and base can be completely ionized or ionized as the standard, as long as it can be completely ionized in the aqueous solution, it is a strong acid or strong base. The pH varies depending on the concentration. The pH value corresponds to the concentration of hydrogen ions in the solution.

The same is true for monobasic strong acids and monobasic weak acids, pH strong acids, weak acids, and alkalis. The pH of the two can only be compared if the conditions are the same. It is not possible to judge whether it is a strong acid or a weak acid according to the pH value, but only the relative strength of the acidity according to the pH value.

Strong acids, sulfate, hydrochloric acid, phosphoric acid, nitric acid.

Strong alkali: sodium hydroxide, potassium hydroxide, calcium hydroxide.

Weak acid H2CO3, HF, CH3Cooh, H2S, HCl, Hno2 weak alkali ammonia monohydrate, note that ammonia is not a weak base, it is a mixture), mg(OH)2, Fe(OH)2, Fe(OH)3, Cu(OH)2

Just go and see the sour ka. This one is clearer.