Bak ing soda is sodium bi carbonate, or more correctl y named, sodi um hydr ogen carbonate: Calcium bicarbonate (Ca(HCO3)2), also called calcium hydrogen carbonate, does not refer to a known solid compound; it exists only in aqueous solution containing the ions calcium (Ca2+), dissolved carbon dioxide (CO2), bicarbonate (HCO3–), and carbonate (CO32–). The relative concentrations of these carbon-containing species depend on the pH; bi carbona te pr ed omina te s wi th in the range 6.36-1 0. 25 in fr es h wa te r. Attempts to prepare compounds such as calcium bicarbonate by evaporating its solution to dryness invariably yield the solid carbonate instead: Ca(HCO3)2(aq) → CO2(g) + H2O(l) + CaCO3(s). If you need this product, then you would have to buy it as a solution. And even then I am not sure that you could bu y it. -- Calcium bicarbonate (Ca(HCO3)2), also called calcium hydrogencarbonate, does not refer to a known solid compound; it exists only in aqueous solution containing the calcium (Ca 2+ ), bicarbonate (HCO 3 – ), and carbonate (CO 3 2– ) 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 contact with the atmosphere absorb carbon dioxide, and as these waters come into contact with rocks and sediments they acquire metal ions, most commonly calcium and magnesium, so 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 form carbonate scale in pipes and boilers and they react with soaps to form an undesirable scum. Attempts to prepare compounds such as calcium bicarbonate by evaporating its solution to dryness invariably yield the solid carbonate instead: Ca(HCO 3 ) 2 (aq ) → CO 2 (g) + H 2 O(l) + CaCO 3 (s). Very few solid bicarbonates other than those of the alkali metals and ammonium ion are known to exist. The above reaction is very important to 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 CO 2 acquired from soil organi sms) passes through limes tone or other calcium carbonate containing minerals , it dissolves part of the calcium carbonate and 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 be deposited. Dis sol ved car bon dioxide (CO 2) in rainwater (H2O) rea cts wit h limest one, cal cium carbona te (CaCO 3 ) to for m sol ubl e cal ciu m bic arbonate (Ca (HCO 3 ) 2 ). Thi s sol ubl e compound is then washed away with the rainwater. This is form of weathering is called 'Carbonation'.

Calcium Bicarbonate

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Baking soda is sodium bicarbonate, or more correctly named, sodium hydrogen

carbonate:

Calcium bicarbonate (Ca(HCO3)2), also called calcium hydrogen carbonate, does notrefer to a known solid compound; it exists only in aqueous solution containing the ions

calcium (Ca2+), dissolved carbon dioxide (CO2), bicarbonate (HCO3–), and carbonate

(CO32–). The relative concentrations of these carbon-containing species depend on the pH; bicarbonate predominates within the range 6.36-10.25 in fresh water.

Attempts to prepare compounds such as calcium bicarbonate by evaporating its solution

to dryness invariably yield the solid carbonate instead: Ca(HCO3)2(aq) → CO2(g) +H2O(l) + CaCO3(s).

If you need this product, then you would have to buy it as a solution. And even then I am

not sure that you could buy it.

Calcium bicarbonate (Ca(HCO3)2), also called calcium hydrogencarbonate, does not

refer to a known solid compound; it exists only in aqueous solution containing thecalcium (Ca2+), bicarbonate (HCO3 – ), and carbonate (CO3

2– ) ions, together with dissolved

carbon dioxide (CO2). The relative concentrations of these carbon-containing speciesdepend on the pH; bicarbonate predominates within the range 6.36-10.25 in fresh water.

All waters in contact with the atmosphere absorb carbon dioxide, and as these waters

come into contact with rocks and sediments they acquire metal ions, most commonly

calcium and magnesium, so most natural waters that come from streams, lakes, andespecially wells, can be regarded as dilute solutions of these bicarbonates. These hard

waters tend to form carbonate scale in pipes and boilers and they react with soaps to form

an undesirable scum.

Attempts to prepare compounds such as calcium bicarbonate by evaporating its solutionto dryness invariably yield the solid carbonate instead: Ca(HCO3)2(aq) → CO2(g) +

H2O(l) + CaCO3(s). Very few solid bicarbonates other than those of the alkali metals and

ammonium ion are known to exist.

The above reaction is very important to 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, itdissolves part of the calcium carbonate and 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 be deposited.

Dissolved carbon dioxide (CO2) in rainwater (H2O) reacts with limestone, calciumcarbonate (CaCO3) to form soluble calcium bicarbonate (Ca(HCO3)2). This soluble

compound is then washed away with the rainwater. This is form of weathering is called

'Carbonation'.

http://en.wikipedia.org/wiki/Aqueous

http://en.wikipedia.org/wiki/Calcium

http://en.wikipedia.org/wiki/Bicarbonate

http://en.wikipedia.org/wiki/Carbonate

http://en.wikipedia.org/wiki/Carbon_dioxide

http://en.wikipedia.org/wiki/Hard_water

http://en.wikipedia.org/wiki/Aqueous_solution

http://en.wikipedia.org/wiki/Calcium_carbonate

http://en.wikipedia.org/wiki/Alkali_metal

http://en.wikipedia.org/wiki/Ammonium