What impurities does sodium bicarbonate generally remove?

No matter what gas impurities must be taken into account, for example, in addition to the impurities in carbon dioxide, sodium hydroxide can not be selected, to prevent the occurrence of NaOH + CO2 = NaHCO3 reaction, followed by Na2CO3 can not be selected, Na2CO3 + H2O + CO2 = 2NaHCO3, if HCl is removed, a strong alkali such as soda lime will generally be selected, but it will react with carbon dioxide, so a saturated NaHCO3 solution is selected, The solubility of this solution to CO2 is small, and it does not lose a lot of carbon dioxide, and the reaction with HCl, NaHCO3+HCl=NaCl+H2O+CO2 can increase a part of carbon dioxide.

In addition, sodium bicarbonate is commonly used in high school to remove impurities: sulfur dioxide in carbon dioxide.

We generally use saturated sodium bicarbonate, which can reduce the dissolution of carbon dioxide in the liquid

NaHCO3 is often used to remove other gas impurities in CO2 gas, such as HCl, Cl2, etc.

This is the use of HCO3- in NaHCO3, which inhibits the hydrolysis of CO2 and reduces the amount of CO2 dissolved in water, while removing HCl, Cl2 and no new impurities are generated.

Sodium carbonate is mixed with sodium bicarbonate, the solid is heated, and sodium hydroxide is added to the solution.

Sodium bicarbonate is mixed with sodium carbonate, and the solution is prepared to pass carbon dioxide.

Add an appropriate amount of sodium hydroxide to make sodium bicarbonate react into sodium carbonate.

Chemical equation: NaHCO +NaOH = NA CO +H O Then use titration to add magnesium carbonate solution dropwise (magnesium carbonate is slightly soluble, it will not be saturated and then precipitated when a small amount is added dropwise) until no precipitation is generated, and the solution can be filtered to extract filtrate.

Chemical equation: 2NaOH + MGCO = MG (OH) Na Co <>

Sodium hydroxide is added to the sodium carbonate solution, sodium carbonate will not react with sodium hydroxide, but sodium bicarbonate can react with sodium hydroxide to form sodium carbonate and water, nahco3 naoh na2co3 h2o, so sodium bicarbonate can be converted into sodium carbonate, while water has no effect.

The simplest method: heating, sodium bicarbonate is unstable, decomposes by heat, and produces sodium carbonate and carbon dioxide.

Whatever gas is removed, the reactivity of the gas must be taken into account, e.g. carbon dioxide removal.

The impurities in the can not be selected to trap the source of sodium hydroxide.

To prevent the reaction of NaOH + CO2 = NaHCO3, NA2CO3 cannot be selected, and NA2CO3 + H2O + CO2 = 2NAHCO3 can occur

If HCl is removed, a strong alkali such as alkali lime is generally selected, but it will react with carbon dioxide, so the saturated NaHCO3 solution is selected, which has a small solubility to CO2 and will not lose a lot of carbon dioxide, and reacts with HClNaHCO3 + HCl = NaCl + H2O + CO2

It is possible to add a portion of carbon dioxide.

In addition, sodium bicarbonate is commonly used in high school.

In addition to the miscellaneous there is also the idea of finch: the removal of sulfur dioxide in carbon dioxide.

We generally use saturated sodium bicarbonate, which can reduce the dissolution of carbon dioxide in the liquid

The effect of removing sodium carbonate impurities in sodium hydroxide and adding calcium hydroxide is to turn sodium carbonate into calcium carbonate precipitate, and at the same time convert it into sodium hydroxide. The chemical equation that occurs:

Na2CO3 + Ca(OH)2 = CaCO3 + 2NaOH, calcium carbonate is a precipitate, after filtration, the remaining solution is sodium hydroxide solution.

Method for removing sodium carbonate from sodium hydroxide:

First, add an appropriate amount of calcium hydroxide solution dropwise, and then let it be filtered to obtain sodium hydroxide solution, and then evaporate, you will get sodium hydroxide solid, Na2CO3 + Ca(OH)2= CaCO3 +2NaOH (Note: Acid such as hydrochloric acid or sulfuric acid cannot be used in the first game, because acid reacts with sodium carbonate and sodium hydroxide at the same time, and NaCl or Na2SO4 will be generated, introducing new impurities; Second, salt solutions such as calcium chloride cannot be used, because they react with sodium carbonate to form NaCl, introducing new impurities. )

Summary. Yes, inhalation includes something to be dried.

Hello, I am Mr. Xiao Liu, engaged in digital integrated circuit design, rent brother and focus on the education of various student grades, I have received your dusty questions, it takes time to solve the problem, please wait a while.

We are happy to answer for you, because sodium bicarbonate reacts with dilute hydrochloric acid to form water and carbon dioxide, so it also needs to be dried and dewatered.

Hope mine is helpful to you.

It's the second one.

Yes, inhalation includes something to be dried.

Sodium carbonate contains a small amount of sodium chloride, which can be removed with silver nitrate, which can react with both sodium chloride and sodium carbonate, which makes it impossible to accurately determine the amount of sodium carbonate.

Silver nitrate can react with sodium chloride to form white precipitated AGCL, and the reaction equation is:

agno3 + nacl → agcl↓ +nano3

At the same time, sodium carbonate can also react with silver nitrate to form a white precipitated Ag2CO3, and the reaction equation is:

2agno3 + na2co3 → ag2co3↓ +2nano3

Therefore, if sodium carbonate contains a small amount of sodium chloride, the removal of sodium chloride with silver nitrate will react with the sodium carbonate at the same time, resulting in an inaccurate mass of the precipitate, making it impossible to correctly determine the amount of sodium carbonated masked.

In order to avoid this, sodium carbonate can be dissolved with acid first, and then the content of chloride ions can be detected with silver chloride solution, so as to accurately determine the content of sodium carbonate.

1) The aqueous solution of sodium carbonate is alkaline, and silver nitrate will generate silver oxide precipitate!

2) Silver carbonate can also precipitate!

Chloride and silver ions form precipitates, but nitrate ions are added to the solution.