The amount and concentration of the substance at room temperature are equal to the three solutions o

The ionization equilibrium of pure water is extremely weak.

h20 = reversible number = h+ +oh-

1.An acid (or alkali) solution is added to inhibit the ionization of water.

2.Externally strengthened alkaline weak salts (or strong acids and weak alkali salts) (weak acids and weak alkali salts) promote the ionization of water due to the hydrolysis of ions. Increasing the ionization of water Chengdu is improving.

The more intense the hydrolysis, the more obvious the increase in the degree of electricity to the water.

In the above question: (NH4)2CO3 anions and cations are hydrolyzed, so the ionization degree of water is the highest.

Compared with the same concentration of (NH4)2SO4 and NH4Cl, the former has a large ammonium ion concentration and is more hydrolyzed (anions are not hydrolyzed), while the latter has a higher pH in the solution and the hydrolysis is weaker.

So: your answer is correct.

nh4）2co3＞（nh4）2so4＞nh4cl

Your judgment is correct because the greater the degree of hydrolysis of the salt, the more hydrolyzed it is, the greater the ionization of the water.

Ammonium carbonate is double hydrolyzed and mutually promoted, and the degree of hydrolysis is the largest. The amount and concentration of the substance are the same, the ammonium ion of ammonium sulfate is twice that of ammonium chloride, and the ammonium ion of ammonium sulfate is more hydrolyzed, so the degree of ionization of water is larger.

Yes, all three solutions promote the ionization of water, the hydrolysis of both ions in NH4)2CO3 solution has the greatest effect on the ionization of water, NH4)2SO4 and NH4Cl are only one ion hydrolysis, but the concentration of ammonium ions in (NH4)2SO4 is larger, and the ionization of water is promoted to a greater extent.

Your judgment is correct, hydrolysis promotes the ionization of water, ammonium carbonate is double hydrolysis, and the concentration of ammonium ions that can be hydrolyzed in ammonium sulfate is greater than that of ammonium chloride. So your judgment is correct.

Analysis] Ammonia.

There is an ionization equilibrium in , and the addition of solid NH4Cl increases the concentration of NH+4 so that the equilibrium is directed towards the formation of ammonia monohydrate.

The degree of dissociation (ionization) decreases, a phenomenon called the homoionic effect. So the answer is: decrease; Homoionic effect. 【Answer】 decrease; Homoionic effect.

If C is not considered, then A=B=C in the three solutions, and in fact NH4+ will be hydrolyzed. NH4Cl is monohydrolyzed and CH3CoonH4 is dihydrolyzed, so there are more NH4+ hydrolyzed in CH3COONH4 than NH4+ in NH4Cl, and HSO4- in NH4HSO4 is completely ionized, and the solution is strongly acidic and will inhibit the hydrolysis of NH4+, so NH4+ hydrolysis in NH4HSO4 solution is the least. To make the concentration of NH4+ in the three solutions equal, then the concentration of B a C, that is, the hydrolysis of NH4+ is larger.

nh4hso4>nh4cl>ch3coonh4

DNH4Cl was selected as a strong acid and weak alkali salt, which was completely ionized, but the NH4+ part was hydrolyzed in the aqueous solution and existed in the form of NH3·H2O.

NH4HSO4 is completely ionized, and there is an acid root, which can ionize part of H+ and inhibit the hydrolysis of ammonium ions.

The concentration of C is the largest, and the concentration of B is the smallest.

hcl=h(+)cl(-) where poh=10, all of which are ionized by water, and h(+) ionized by water is equal to oh(-), so the concentration of h(+) ionized by water is minus 10 to the power of 10.

NH4(+)H2O =, H(+) are all ionized by water at a concentration of 10 to the minus 4th power.

So the ratio of the two is 10 to the minus 6 power (HCL:NH4Cl).

Hydrochloric acid solution occurs as follows.

Hydrolysis reaction. hcl

h2o*****==

h(+)oh(-)

x can then easily get x=10(-10).

That is to say, the OH- hydrolyzed in water is 10 (-10) in NH4Cl

The following hydrolysis reaction takes place in the solution:

nh4(+)h2o

h(+) From the above equation, it can be seen that the hydrogen ions ionized from water in the ammonium chloride solution are 10(-4), which means that the OH ions provided by water are also 10(-4), so you can easily get 10(-4) 10(-10)=10(6) times.

The key to this question is to know that those ions in the solution are provided by water alone, for example, in hydrochloric acid solution, hydrogen ions are produced by hydrolysis of water, and hydrogen ions are also provided in hydrochloric acid; Only.

Hydroxide ions.

It is provided separately after ionization of water, and the amount of hydroxide ions can be confirmed with the help of pH value; The problem can then be solved.

Acids or bases inhibit the ionization of water, hence NaOH and H2

The ionization degree of water in SO4 solution is small, because sulfuric acid is a dibasic strong acid, and sodium hydroxide is a monobasic strong base, so the ionization degree of water in sulfuric acid with the same substance concentration is smaller than that of water in sodium hydroxide; Hydrolyzable salts promote hydrolysis, so (NH4

The degree of ionization of water in the SO4 solution is the largest; The non-hydrolyzed salt NaCl has no effect on the ionization of water, so the correct order of the ionization degree of water is: Therefore, C

Let the concentrations of the substances in the five solutions be C, CH3COOH is a weak acid, acetic acid inhibits the ionization of water, and the concentration of hydrogen ions in the solution is less than C.

Both ammonium ions and carbonate ions in NH4) 2CO3 can be hydrolyzed, which promotes the ionization of water, and the ionization degree of water in ammonium carbonate solution is the largest among the five substances.

NaHSO4 is an acidic solution, the concentration of hydrogen ions in the solution is C, and the ionization degree of water in the sodium bisulfate solution is less than ;

NaHCO3 is a strong base and weak salt, the hydrolysis of bicarbonate ions, promotes the ionization of water, and the ionization degree of water in sodium bicarbonate solution is less than ;

If the concentration of hydroxide ions in Ba(OH)2 solution is 2C, the ionization degree of water in barium hydroxide solution is the smallest.

According to the above analysis, it can be seen that the ionization degree of water in acetic acid solution is greater than Nahso4 and Ba(OH)2, which is less than , so the ionization degree of water in the five solutions is ranked from large to small: Therefore, D is selected

In addition to the existing NH4, NH3 is combined with water to obtain some NH4, CL is more normal, and OH is increased because water binds to NH3, in fact, NH3 binds to H+ in water, and OH- is free; Therefore, the order is as above.

The second question, I don't understand it, can I make it clearer?

Sodium acetate solution has the most NA, followed by acetate, then OH, and then H

Na is all ionized, so the most, the acetate is alkaline and H is combined, and the excess OH is free.

In the case of acetic acid solution, acetic acid molecules are the most, then H, then acetate, and then OH the least. Acetate and H are ionized in the same amount, but the water itself contains a small amount of H. Even if acetate is combined with H, it is 1:1, and the relationship between the two amounts remains unchanged.

Your supplementary question:

It should not be hydrolyzed. It ionizes NH3 and H+ and is acidic. You don't have to think about its hydrolysis here.

2.If it is a mixture, then I would say that it is impossible to determine whether there are more acetate or sodium ions, and if the amount is not given. Imagine that in the extremely concentrated sodium acetate solution, sodium ions are naturally the most, followed by acetate, and adding a little acetic acid will not make acetate exceed sodium ions; However, if the acetic acid solution is very concentrated, although the acetic acid is weakly ionized and the acetic acid molecule is the most, there is still a fairly concentrated acetate, and adding a little sodium acetate cannot make the sodium ion exceed the acetate ion.

Or is there still some condition to the original question?

In fact, it is a matter of prioritization.

Mixed solution of NH4Cl and NH3H2O:

Let's not consider hydrolysis first, C(NH4+)=C(Cl-), right, and then look at NH3H2O, it needs to be partially ionized, so, in general, C(NH4+)>C(Cl-). In the same way, the key is not to think of hydrolysis very strongly, in fact, it is very weak.

The latter is the same, in short, the main aspects are considered first, the salts are of course completely ionized first, which is the main one, then the ionization of weak electrolytes, and finally hydrolysis.