Ask for a chemistry about ionization equilibrium problems

Hydrochloric acid is a strong acid, pH = 1 means C(HCl) = , and the mixing of MOH with HCl in equal volumes happens to be completely reacted to indicate that C(MoH) = is correct, so option A is correct.

C(MoH) = and the pH of the MOH solution = 11, indicating that the MOH is a weak base. The solution after the reaction is a solution of strong acid and weak alkali salt MCl, because of the hydrolysis of M+ ions, so C(Cl-)>C(M+)>C(H+)>C(OH-), option B is correct.

After the reaction, it is equivalent to diluting the concentration of element M by a doubling, so the total concentration of element M is halved, i.e., C(M+)+C(MoH)=, and the C option is wrong.

Although MOH is a weak base, the ionization of OH- by MOH inhibits the ionization of H2O, and it can be approximated that OH- is ionized by MOH. In the original MOH solution, POH = 3, C(OH)=10 (-3)mol L can be obtained, so the power balance constant of KOH kb=C(OH)C(MoH)=1 10 -5

The wrong thing is B, if MoH is a strong base, because they are mixed in equal volume, and at room temperature, the mixed solution should be neutral, if MoH is a weak base, according to "who shows whom", the solution is alkaline after the reaction, C(H+)<=C(OH-).

I'm just dizzy... Ionization equilibrium still needs to be proved?? If you really want to prove it, so be it:

For the prepared MgSO4 strong electrolyte solution, the Mg content was calculated by titrating the Mg (EBT indication) first. Add the same volume of BaCl2 solution, centrifuge the precipitate after the reaction, weigh it after drying, and calculate the amount of precipitated substance; Compare the results of gravimetric and complexation titration, whether the content of mg ions and SO4 is consistent with the rest of the rest, think more about it yourself.

1: Take the ionization of acetic acid molecules as an example. When the acetic acid molecule is added, the equilibrium shifts to the right, i.e., in the direction of ionization, depending on the nature of the chemical equilibrium.

However, acetic acid is a weak electrolyte, that is, if you don't add one, you will ionize one, and if you add 100, maybe only a few ionizations, that is, more and less ionization, the degree of natural ionization will be smaller.

2: Also take acetic acid as an example, when adding water, one method is to regard ionization as the reaction of acetic acid and water, increase the reactants, balance the ionization direction shift, and increase the degree of ionization. Or ionization is regarded as the Brownian motion of water molecules, and its impact on acetic acid molecules makes it ionized, and when there is more water, the degree of impact is greater, and there is more ionization.

What is the relationship between ionization equilibrium and equilibrium of the residual stupid and flat erection fluid.

Ionization equilibrium, like chemical equilibrium, can be explained by the direction of equilibrium movement using Le Chatre's principle. Since ionization equilibrium is the equilibrium present in solution, pressure has no effect on ionization equilibrium. The ionization equilibrium is mainly affected by temperature and concentration.

In addition, when studying the ionization equilibrium, it is often necessary to consider both the ionization balance of the weak electrolyte in water and the ionization balance of the very weak electrolyte itself, which is very weak.