Chemistry Does HSO3 in saturated NaHSO3 solution inhibit the dissolution of SO2?

Yes, when SO2 dissolves to form H2SO3, it ionizes H2SO3 ==ionization reversible ==H+ +HSO3-

If there is HSO3- in the solution, it will inhibit the ionization of H2SO3, so that the concentration of H2SO3 is large, it is easy to re-decompose into SO2 and escape from the solution, that is, the amount of SO2 dissolution decreases.

OK. SO2 has two forms in water, one in the molecular form of SO2 and one in the form of sulfurous acid.

Principle: SO2 + H2O = reversible number = H2SO3H2SO3 = reversible number = HSO3- + H+ HSO3- in saturated NaHSO3 solution- is a large amount, and the lower equilibrium shifts left, so the previous equation is also shifted to the left, inhibiting SO2 in the form of H2SO3. However, it does not have much effect on the SO2 in the molecular state.

Yes, I see that there is an analysis below, so I won't repeat it, but what I want to say is that the important thing about this knowledge point is how to prevent the gas from dissolving in water when doing experiments, similar to carbon dioxide, etc., I think this is the meaning of this knowledge point.

When SO2 enters the water, it will dissolve and hydrate These two effects are different There is no free in the aqueous solution of SO2'Sulfurous acid'However, the relevant constants can still be used in the calculation of acid-base equilibrium: Back to the question The dissolution of SO2 necessarily causes the ionization equilibrium of H2O to shift due to HSO3'The dissolution of SO2 will be inhibited.

OK. The aqueous solution of SO2 is H2SO3

H2SO3 is a weak acid that is weakly ionized in water.

H2SO3 is reversible = H+ + HSO3-

Utilize the principle of Le Chatre.

An increase in the product can inhibit the reactants from continuing the reaction.

In a saturated NaHSO3 solution, HSO3- ions have been saturated with chain silver, while SO2 dissolves to justify the ionization equation.

It is SO2 + H2O = HSO3- ion + H+ ion, and SO2 can no longer be dissolved in solution due to the saturation relationship of HSO3- ion.

SO3 is dissolved in water to form sulfuric acid, which reacts with NaHSO3: SO3 + H2O + 2NaHSO3 = NA2SO4 + 2H2O + SO2 (Solubility of SO2 in water purity.

It's not big, so it will volatilize)

By the way, the essence of the reaction (I don't know if you learned that): SO3 dissolves in water to form sulfuric acid, which greatly increases the density of H+ ions in the water, so that the formula proceeds in the opposite direction, which is an ionization equilibrium.

reversible reactions.

In fact, the saturated NaHSO3 solution does not no longer absorb SO2, but the volatilization and dissolution of SO2 reach a balance.

Hello! SO2 is an acidic oxide, and the excess SO2 is introduced into the saturated Na2SO3 solution, which is the same as the reaction of the excess CO2 in the saturated Na2CO3 solution, SO32-+SO2+H2O=2HSO3-

When in doubt, please ask.

If you ask that, it should be similar to CO2, right? so3

so2h2o

2na+===2nahso3↓

That's a reasonable migration, right? Since saturation of Na2SO3 is emphasized, the solubility of NaHSO3 should be small and will precipitate, the same as CO2.

1. SO3 dissolves in water to form sulfuric acid, and then it is gone...

2. Sodium bisulfite corresponds to sulfurous acid, which is weaker acidic than sulfuric acid and can react with sulfuric acid, and the ion equation is: HSO3- +H+ = H2O+SO2

3. Sodium bisulfite can actually be regarded as the final product of the reaction of sodium sulfite solution that continues to pass into a sufficient amount of SO2, so SO2 can no longer be dissolved.

Sulfuric acid is more acidic than Nahso3, i.e., sulfuric acid has less attraction to hydrogen ions.

This is an ionization equilibrium problem, there is a lot of HSO3- in the saturated solution, and if the SO2 is dissolved, HSO3- and H- will be produced, which will cause the equilibrium to move and produce SO2.

Sulfuric acid is stronger than NaHSO3, the principle of strong acid to weak acid!

The ionic effect allows you to eat the same thing to your heart's content, and if you are allowed to eat it, can you still eat it? But let you drink some water, and you will be able to drink it.

Hello, because the reaction of SO3 and water will release a lot of heat, whether it is water absorbing SO3 or NAHSO3 solution absorbing SO3, it is easy to produce acid mist, which is not conducive to the absorption of SO3, in addition to SO3 in SO3 generally with more concentrated sulfuric acid, SO3 and sulfuric acid reaction to obtain SO3 sulfuric acid complex H2SO4*XSO3, this component is relatively stable, and the absorption efficiency of SO3 is very high, and SO2 will not be dissolved in strong acidic sulfuric acid.

Hope it helps!

If you don't understand, please ask!

It can be used, but it should be saturated, because the acidity of sulfuric acid is stronger than that of sulfurous acid, and strong acid makes weak acid.

The removal of SO3 from SO2 is done through saturated NaHSO3.

Saturated NaHSO3 solution no longer dissolves SO2.

hso3- +h+ =h2o+so2

So that's it.

Above. [Welcome to ask, thank you for adopting!] 】

Because strong acid makes weak acid, sodium bisulfite will become sodium sulfate, so it cannot be used.

So to speak ...

Because the formation of HSO3 is a reversible reaction: SO3(2-) H2O HSO3(-)OH-

After the addition of NaOH, the OH- generated by the ionization of NAOH causes the reaction of sulfite to move in the opposite direction, so that HSO3(-) reacts with OH- to form SO3(2-) and H2O.

Hso3(-) is then "reacted".

Hope, thank you! Good luck in your studies!

The hydrolysis you are talking about is a reversible reaction, which is essentially a hydrolysis equilibrium, which is a dynamic equilibrium, SO3(2-) H2O HSO3(-)OH- that is to say, the hydrolysis process and the neutralization process (OH- and HSO3- reactions) are carried out at the same time, and the equilibrium state is reached.

Conclusion: The process you are talking about exists.

In addition, most of the water that we often say relieves the double hydrolysis that has precipitation, and it does not affect the large number of coexistence problems we talked about before.

For example, we still think that sulfites can coexist in large quantities in water, while hydroxide ions and bisulfite ions still cannot coexist in large quantities, and the amount of them generated in this question is very small.

Hope it helps.

Hydroxide inhibits sulfite hydrolysis.

A small amount of sulfur dioxide produces sodium sulfite, water and carbon dioxide

2NaHCO3 SO2=Na2SO3 H2O 2CO2 Excess sulfur dioxide produces sodium bisulfite and carbon dioxide:

so2 nahco3=nahso3 co2↑