ca(hco3)2

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Calcium bicarbonate
Calcium bicarbonate
Names
IUPAC name

Calcium hydrogencarbonate

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Systematic IUPAC name

Calcium bicarbonate

Other names

Cleansing lime
Bicarbonate of lime
Rain salt

Identifiers

CAS Number

  • 3983-19-5 check

3D model (JSmol)

  • Interactive image
  • Interactive image
ChemSpider
  • 8351767 check

PubChem CID

  • 10176262
UNII
  • 7PRA4BLM2L check

CompTox Dashboard (EPA)

  • DTXSID50893964 Edit this at Wikidata

InChI

  • InChI=1S/2CH2O3.Ca/c2*2-1(3)4;/h2*(H2,2,3,4);/q;;+2/p-2 check

    Key: NKWPZUCBCARRDP-UHFFFAOYSA-L check

  • InChI=1/2CH2O3.Ca/c2*2-1(3)4;/h2*(H2,2,3,4);/q;;+2/p-2

    Key: NKWPZUCBCARRDP-NUQVWONBAN

SMILES

Properties

Chemical formula

Ca(HCO3)2
Molar mass 162.11464 g/mol

Solubility in water

16.1 g/100 mL (0 °C)
16.6 g/100 mL (20 °C)
18.5 g/100 mL (100 °C)[citation needed]
Hazards
Occupational safety and health (OHS/OSH):

Main hazards

Irritant
Flash point Non-flammable
Related compounds

Other cations

Magnesium bicarbonate

Related compounds

Sodium bicarbonate

Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

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Infobox references

Calcium bicarbonate, also called calcium hydrogencarbonate, has the chemical formula Ca(HCO3)2. The term does not refer to lớn a known solid compound; it exists only in aqueous solution containing calcium (Ca2+), bicarbonate (HCO
3
), and carbonate (CO2−
3
) ions, together with dissolved carbon dioxide (CO2). The relative concentrations of these carbon-containing species depend on the pH; bicarbonate predominates within the range 6.36–10.25 in fresh water.

All waters in tương tác with the atmosphere absorb carbon dioxide, and as these waters come into tương tác with rocks and sediments they acquire metal ions, most commonly calcium and magnesium, so sánh most natural waters that come from streams, lakes, and especially wells, can be regarded as dilute solutions of these bicarbonates. These hard waters tend to lớn sườn carbonate scale in pipes and boilers, and they react with soaps to lớn sườn an undesirable scum.

Attempts to lớn prepare compounds such as solid calcium bicarbonate by evaporating its solution to lớn dryness invariably yield instead the solid calcium carbonate:[1]

Ca(HCO3)2(aq) → CO2(g) + H2O(l) + CaCO3(s).

Very few solid bicarbonates other kêu ca those of the alkali metals (other kêu ca ammonium bicarbonate) are known to lớn exist.[clarification needed]

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The above reaction is very important to lớn the formation of stalactites, stalagmites, columns, and other speleothems within caves, and for that matter, in the formation of the caves themselves. As water containing carbon dioxide (including extra CO2 acquired from soil organisms) passes through limestone or other calcium carbonate-containing minerals, it dissolves part of the calcium carbonate, hence becomes richer in bicarbonate. As the groundwater enters the cave, the excess carbon dioxide is released from the solution of the bicarbonate, causing the much less soluble calcium carbonate to lớn be deposited.

In the reverse process, dissolved carbon dioxide (CO2) in rainwater (H2O) reacts with limestone calcium carbonate (CaCO3) to lớn sườn soluble calcium bicarbonate (Ca(HCO3)2). This soluble compound is then washed away with the rainwater. This sườn of weathering is called carbonation and carbonatation.

In medicine, calcium bicarbonate is sometimes administered intravenously to lớn immediately correct the cardiac depressor effects of hyperkalemia by increasing calcium concentration in serum, and at the same time, correcting the acid usually present.

References[edit]