20 points It s simple. The magnitude of the ion concentration

H2S is a weak electrolyte, and only a small part of it ionizes C(H2S) to the maximum acidic solution C(H+) C(OH).

Partial H2S ionization out of H+ and Hs Partial Hs ionization out of H+ and S2 so C(H+) C(Hs) C(S2).

Na2S is a strong electrolyte, and all of them ionize Na+ and S2 alkaline solutions C(OH) C(H+).

Part of S2 combines with H+ to generate HS Part of Hs combines with H+ to form H2S

First of all, if the H2S process is acidic, H+>OH-; Then the H2S molecule is dissolved in water, and its concentration is the largest, and then Hs- is the first-order ionization, which is greater than the second-level ionization of S2-, and the first-level ionization should also inhibit the second-level ionization, and the first one should be selected in general.

The first one is a weak electrolyte, so there are the most molecules and only one cation, according to the conservation of charge, so the hydrogen ion ranks second, the sulfide ion ionizes in one step, the sulfur ion ionized in two steps, so the sulfur is greater than the sulfur ion, and the acid solution hydroxide is the least.

The second strong electrolyte, sodium is definitely the most. Because the sulfur ion is less than one-half of sodium, it ranks second. Then consider hydrolysis, hydroxide is equal to hydroxide plus two hydrogen sulfide hydrogenation ions.

Therefore, hydroxide is the most, and it takes two steps to hydrolyze hydrogen sulfide in one step, so hydrogen sulfide is greater than hydrogen sulfide alkaline solution with the least hydrogen ions.

H2S is a weak acid, only a small part of the solution is ionized, and the solution is acidic; Na2S is a strong base and weak salt, all of which are ionized, and the solution is alkaline.

Divide the strength and weakness, and look at **!

Ammonium chloride: chlorine corresponds to strong acid, ammonium corresponds to weak alkali (ammonium ion hydrolysis), so the chloride ion concentration is greater than the ammonium ion concentration; However, the hydrolysis process is also a relatively weak process, so the concentration of ammonium ions is greater than that of the particles produced by hydrolysis. But the hydrolysis of ammonium is greater than the ionization of water, so NH3H2O is greater than OH-, as for H+, NH3H2O, OH-, combined with the ionization of water and the hydrolysis of ammonium ions, H+** is more, so the concentration of H+ is greater than , OH-

In the case of ammonium sulfate, the ammonium ion concentration is greater than the sulfate ion concentration (compare from ** first).

The comparison of ion concentrations is a comparison of the size of various ions in a solution.

1. To analyze the solutes in the solution, there are acid solutions, alkali solutions, and salt solutions.

2. According to the nature of the solute, the strength, the degree of ionization, the degree of hydrolysis, the acidity and alkalinity of the solution, the ionization of water, etc.

3. Pay attention to the law of conservation of charge.

Acetic acid with 100 ml

Hydrogen hand clear sodium oxide.

The solution is mixed with the amount of acetic acid of the substance.

The amount is equal to the amount of NaOH substance, so it is equivalent to sodium acetate solution when mixed. The ions in sodium acetate solution are Na+, acetate ion, H+, and Oh-. Obviously, Na+ is the most, and the acetate is less than Na+ due to partial hydrolysis, and the hydrolysis is very little, so oh- is less than acetate, and the solution is alkaline, so oh- is greater than H+.

Ion concentration order is NA+>CH3COO->OH->H+

2. It is best to add an equal volume to mix this question. Mix the solution.

The ions present in are also Na+, acetate ions, H+, and Oh-. If acetic acid is not ionized and acetate is not hydrolyzed, Na+ and acetate concentrations are the same. Since the ionization of acetic acid is stronger than the hydrolysis of acetate, the ionized acetate is more than the hydrolyzed, so the total acetate increases, resulting in acetate greater than Na+.

Since acetic acid ionization is stronger than acetate hydrolysis, the ionized H+ is more than the OH- produced by hydrolysis, so H+ is greater than OH. Ion concentration magnitude order: CH3CoO->Na+>H+>OH-

3. Take NaHCO3 as an example. HCO3- is ionized (producing CO32-) and hydrolyzed (producing H2CO3) but is rarely present and is basically present as HCO3-. Mass balance: [HCO3-]+CO32-]+H2CO3]=

Charge balance: [Na+]+H+]=HCO3-]+OH-]+2[CO32-].

4. Take MGO as an example:

fe3+3h2o

3h+fe(oh)3↓

It can be seen that if Fe3+ is removed, only the H+ concentration needs to be reduced, and the reaction can be carried out to the right.

The following reaction occurs when the MGO is added:

mgo2h+

Mg2+H2O, just enough to consume H+ and promote the hydrolysis of Fe3+. Similar to MGCo3, of course MG(OH)2Y is also possible.

The latter one is similar to the front.

1.It can be seen that after the reaction, the substance after the reaction can be understood as 1 acetic acid, one hydrogen potassium, and one potassium acetate.

Because pH <7, the ionization of acetic acid is greater than the hydrolysis of potassium acetate.

Therefore, the amount of acetic acid molecule is less than that of acetate, but because acetic acid is a weak electrolyte, only a small amount of hydrogen ions is electrolyzed.

It can be inferred that the amount of acetate is greater than the amount of chloride ions.

It is compared to acetate, chloride ions, acetic acid molecules, and hydrogen ions.

(1) After the reaction, it is acetic acid, potassium acetate and potassium chloride solution of the same concentration. pH <7, indicating that the degree of ionization of acetic acid is greater than that of acetate ions. Then only acetic acid ionization can be considered, and acetate hydrolysis can not be considered.

The concentration of potassium ions is the highest, followed by acetate ions, followed by chloride ions. Acetic acid molecules and hydrogen ions are generally not compared because you have to know the ionization constant of acetic acid. However, they are all less concentrated than chloride ions, and the smallest is hydroxide ions.

2) After the reaction, it is an equivalent concentration of ammonium chloride, ammonia monohydrate, and sodium chloride solution. The solution is alkaline and only ionization is considered, not hydrolysis. So:

The concentration of chloride ion is the largest, followed by ammonium ion, sodium ion again, ammonia monohydrate and hydroxide ion are smaller than sodium ion, and the smallest is hydrogen ion.

Conclusion: Hydrogen ions are large.

Explanation: C(H+)+C(Na+)=C(HCO3-)+2C(CO32-)+C(OH-) This formula is called conservation of charge.

The formula C(Na+)=C(HCO3-)+C(CO32-)+C(H2CO3) is called conservation of materials.

Subtract the two formulas.

The formula C(H+)=C(CO32-)+C(H2CO3) is called conservation of protons.

It can be seen that the concentration of hydrogen ions is greater than that of carbonate.

In the explanation, some charge numbers can not be written on the superscript, pay attention to your own observations).

Ammonium chloride is a strong acid and weak alkali salt, the strong acid part (Cl-) does not undergo ionization hydrolysis, and the weak alkali part (NH4+) is hydrolyzed, making the solution acidic.

NH4Cl solution, the main molecular ions present in the solution are H2O, NH4+, Cl-, H+, OH-.

Obviously, in addition to H2O, Cl- is the largest, and NH4+ microhydrolysis concentration is second, and the main comparison is H+, OH-.

There are two equilibrium present in the solution: H2O = H+ +OH-, NH4+ + H2O = + H+

In these two equilibriums, the ionization equilibrium of water is very weak, mainly considering the hydrolytic equilibrium of ammonium ions.

Both equilibrations produce H+, so the concentration is maximum. Secondly, the concentration of OH- is completely ionized by water, which is very low.

So H2O Cl- NH4+ H+

As for ammonium sulfate, except for NH4+ and SO42-, the other concentrations are the same, because the equilibrium present in the solution is the same.

The only common ionization that is greater than hydrolysis in high school seems to be HSO3-, H2PO4-, and HC2O4-. Others are generally hydrolyzed more than ionized.

1. If the volume of the solution is not the same, it cannot be compared, if it is equal, then: Na+=Cl->OH->NH4+>H+

The two substances react to form NaCl and NH3H2O, and both ammonia monohydrate ionization and water ionization form OH-

2. If the volume of the solution is not the same, it cannot be compared, if it is equal, then: Cl->NH4+>Na+>OH->H+

After the reaction, the substances in the solution are the same concentration of NaCl, NH4Cl, NH3H2O, the solution is alkaline, so NH4+>NA+, OH- is partially ionized by ammonia, so it is less than NA+