If you want to remove calcium bicarbonate from calcium carbonate, is it better to dissolve filtratio

Thermal decomposition is better, calcium carbonate can only be decomposed after high temperature, and the temperature reached when calcium bicarbonate is decomposed can not make calcium carbonate decompose, calcium bicarbonate dissolves in water, will decompose after heating, precipitate calcium carbonate, release carbon dioxide, and increase the quality of carbon dioxide, more resource-saving.

The decomposition of calcium carbonate needs to be 825 degrees.

When calcium bicarbonate is dissolved in water, its aqueous solution is also known as "hard water".

Ca(HCO3)2== heating ==CaCO3 +CO2 +H2O calcium carbonate is dissolved at a high temperature.

Chemical formula CA (HCO3) 2 formula, relative molecular mass, calcium carbonate dissolved in carbon dioxide aqueous solution to form calcium bicarbonate. The powder is white, and the crystals are colorless and transparent. Soluble in water.

Just control the temperature.

The decomposition of calcium carbonate into calcium oxide requires a high temperature of more than 800 degrees, and the laboratory is generally used to burn this in a muffle furnace.

Ordinary heating only causes calcium bicarbonate to decompose.

Calcium carbonate is insoluble in water. It is not easy to decompose when heated.

Whatever I think, it can be purified.

Separate the size, the elementary school level of the question. There is no pure calcium bicarbonate, which is only found in dilute solutions.

It should be filtered.

ca(hco3)2=caco3↓+co2↑+h2o

That's how the cave was formed.

Calcium carbonate. Heating produces calcium oxide and carbon dioxide.

Carbon dioxide is a gas, and it is easy to get lost with the flow of air in an open container, so all that remains is calcium oxide, that is, calcium carboparaate in calcium oxide can be removed by heating.

Both calcium carbonate and calcium oxide can react with hydrochloric acid:

caco3+2hcl=cacl2+co2+h2o

cao+2hcl=cacl2+h2o

The removal method can be used by hand: the sample is placed in water, a sufficient amount of carbon dioxide is introduced, the mixture is heated to 80 degrees, and filtered for drying.

cao+co2=caco3

CaCO3 + CO2 (excess) + H2O = Ca(HCO3)2

Ca(HCO3)2 = CaCO3 + CO2 + H2O (more than 60 degrees).

Calcium carbonate uses:

1. Rubber: A large amount of calcium carbonate filled in rubber products can increase the volume of the product, thereby saving expensive natural rubber.

or synthetic rubber to reduce costs; Improved processability without affecting the vulcanization system of the rubber due to changes in the addition ratio; Improve the performance of vulcanized rubber, play a reinforcing or semi-reinforcing role; The hardness can be adjusted by varying the amount of calcium carbonate filling; Adjust the viscosity in the latex glue and the glue of the rubber, etc.

2. Plastics: adding calcium carbonate to plastics can play a skeleton role and improve the dimensional stability of plastic products; Improve the hardness and rigidity of plastic products; The addition of calcium carbonate can change the rheological properties of plastics.

Improve the surface gloss and surface flatness of products; Reduce the shrinkage rate and linear expansion coefficient of plastic products.

Creep properties, which contribute to the processing and forming of plastics; Improve the heat resistance of plastic products and improve the astigmatism of plastics.

Sex; Reduce the cost of plastic products.

The above content refers to Encyclopedia - Calcium Carbonate.

Calcium carbonate. High temperature (heating is not possible, high temperature or calcination is required) decomposition and generationCalcium oxideand water, the chemical reaction equation is as follows:

Chemical equation for calcium carbonate pyrolysis.

Calcium bicarbonate is not a precipitateCalcium carbonate. is a precipitate, calcium bicarbonate is an inorganic acid salt, soluble in water, can be made ofSodium bicarbonateIt is obtained by reacting with calcium salts that are easily soluble in water.

The chemical formula of calcium bicarbonate is Ca(HCO) relative molecular weight.

Calcium carbonate is dissolved in carbonic acid to form calcium bicarbonate. Evaporation of calcium bicarbonate solution yields calcium carbonate solids. Soluble in water, pyrolysis, and alkali to form positive salts.

When calcium carbonate meets carbon dioxide.

When it is mixed with water, chemical erosion occurs to generate soluble calcium bicarbonate, and the phenomenon of "water droplets and stones wear" occurs over time.

Calcium bicarbonate**

Karst landforms. It is made by re-precipitating calcium carbonate from natural water in caves. When there is more calcium bicarbonate dissolved in the water, it becomes hard water.

The composition of the primordial atmosphere above the Earth 3 billion years ago was gases such as CO, CO2, N2, CH4, but there was no oxygen. There are seaweeds in the ocean, which photosynthesize when exposed to sunlight.

and the CO2 in the atmosphere is consumed.

This leads to the escape of O2 dissolved in water to replenish the atmosphere, and this change causes the decomposition of calcium bicarbonate Ca(HCO3)2] dissolved in water to form calcium carbonate CaCO3], Ca(HCO3)2== heating CaCO3 CO2 H2O to form limestone on Earth.

The above content reference: Encyclopedia - calcium bicarbonate.

Calcium carbonate is insoluble in water, so it can be removed by filtering. (Filtration can quietly remove insoluble impurities).

Because dilute hydrochloric acid can react with both calcium oxide and calcium carbonate.

cao+2hcl=cacl2+h2o

CaCO3+2HCl=CaCl2+CO2( )H2O,4,Calcium oxide reacts with water to generate calcium hydroxide and hydrochloric acid,2,Calcium oxide also reacts with hydrochloric acid,2,If dilute hydrochloric acid removes the small amount of calcium carbonate in calcium oxide,To dissolve solid impurities with dilute hydrochloric acid,After dissolution, the calcium chloride solution is obtained,Destroy the substance。 , 2, calcium oxide will also be known to react with dilute hydrochloric acid. ,2, first of all, we must figure out what is impurity, impurity, as the name suggests, is just to remove impurities, dilute hydrochloric acid can react with calcium oxide, calcium carbonate, so you can't use dilute hydrochloric acid, cao+2HCl=CaCl2+H2O CaCO3+2HCl=CaCl2+CO2 +H2O, if you want to remove calcium carbonate, you can heat the mixture, CaCO3 CaO+CO2, 2, because CAO+2HCl=CaCl2+H2O

Calcium oxide also reacted ·

It is necessary to use the method of high-temperature calcination,1, because calcium oxide is an alkaline oxide, which will react with acid to form salt and water, and will also react with water to become alkali (Ca(OH)2).

Therefore, it is generally calcined at high temperature, heated to 1000 degrees Celsius, and calcium carbonate will decompose into calcium oxide and carbon dioxide

caco3=cao+co2↑

This not only removes impurities, but also increases the yield of calcium oxide, which is generally an industrial method.

The lab is a bit more complicated...1. Because dilute hydrochloric acid and calcium oxide will also react, the calcium carbonate will be removed at the same time. It is best to perform high-temperature calcination.

0, dilute hydrochloric acid will react with calcium oxide, calcination is OK. ,0,CAO reacts with hydrochloric acid to generate calcium chloride and carbon dioxide, not to mention calcium oxide - all become calcium chloride, 0, because dilute hydrochloric acid can react with calcium oxide and calcium carbonate.

cao+2hcl=cacl2+h2o

caco3+2hcl=cacl2+co2（^)h2o

Because CA + 2 HCl = CACl2 + H2O

Calcium oxide also reacted ·

To use the method of high-temperature calcination, 0,

Calcium carbonate is heated to produce calcium oxide and carbon dioxide, carbon dioxide is a gas, which is easy to get lost with the air flow in an open container, so all the rest is calcium oxide, that is, the calcium carbonate in calcium oxide can be removed by heating.

Both calcium carbonate and calcium oxide can react with hydrochloric acid:

CaCO3 + 2HCl = CACl2 + CO2 + H2OCAO + 2HCl= CaCl2 + H2O removal method can be selected: the sample is placed in water, a sufficient amount of carbon dioxide is introduced, the mixture is heated to 80 degrees, and filtered for drying.

cao + co2 = caco3

CaCO3 + CO2 (excess) + H2O = Ca(HCO3)2Ca(HCO3)2 = CaCO3 +CO2 + H2O (over 60 degrees).

Because calcium carbonate can react with hydrochloric acid to form gas and solvent reflux, silica will not react and will not be dissolved, so it is filtered and separated.

Calcium carbonate (CACO) is an inorganic compound commonly known as limestone, limestone, stone powder, marble, etc. Calcium carbonate is neutral, basically insoluble in water, and sensitive to hydrochloric acid. It is one of the most common substances on earth, found in aragonite, calcite, chalk, limestone, marble, travertine and other rocks, and is also the main component of animal bones or shells.

Calcium carbonate is also an important building material and has a wide range of industrial uses.