Calcium bicarbonate (Ca(HCO3)2) is a compound that contains calcium, carbon, and oxygen. It is commonly found in mineral water and is important for bone health and muscle function.
| IUPAC Name | Calcium hydrogen carbonate |
| Molecular Formula | Ca(HCO3)2 |
| CAS Number | 3983-19-5 |
| Synonyms | Calcium acid carbonate, Calcium hydrogencarbonate, Calcium bicarbonate hydrate, Calcium hydrogen carbonate hydrate, EINECS 223-070-3 |
| InChI | InChI=1S/C2H2O3.Ca/c3-1(4)2(5)6;/h(H2,3,4)(H,5,6);/q;+2/p-2 |
Calcium Bicarbonate Properties
Calcium Bicarbonate Formula
The chemical formula of calcium bicarbonate is Ca(HCO3)2. This indicates that the compound consists of one Ca2+ ion and two HCO3- ions. The formula is important in understanding the composition of the compound and its chemical properties. Ca(HCO3)2 can be formed by dissolving calcium carbonate in carbonated water, or by reacting calcium hydroxide with carbon dioxide.
Calcium Bicarbonate Molar Mass
The molar mass of Ca(HCO3)2 is 162.114 g/mol. This is calculated by adding the atomic masses of each element in the compound. Ca(HCO3)2 contains calcium, hydrogen, carbon, and oxygen atoms, and the molar mass reflects the combined mass of all these atoms. Knowing the molar mass is important in determining the amount of Ca(HCO3)2 needed in chemical reactions or in determining the concentration of a solution.
Calcium Bicarbonate Boiling Point
Ca(HCO3)2 decomposes before it reaches its boiling point. At normal atmospheric pressure, Ca(HCO3)2 decomposes into calcium carbonate, water, and carbon dioxide at temperatures above 50°C. Therefore, it does not have a boiling point.
Calcium Bicarbonate Melting Point
Ca(HCO3)2 does not have a distinct melting point because it decomposes before it reaches its melting point. It decomposes into calcium carbonate, water, and carbon dioxide at temperatures above 50°C. However, the thermal decomposition of Ca(HCO3)2 can be used to produce calcium oxide, which has a high melting point of 2,613°C.
Calcium Bicarbonate Density g/mL
The density of Ca(HCO3)2 is 2.21 g/mL. This means that a cubic centimeter of Ca(HCO3)2 weighs 2.21 grams. The density of Ca(HCO3)2 is lower than the density of calcium carbonate, which is 2.71 g/mL. The density of a substance is important in determining the mass of a substance per unit volume, and can be used to calculate the concentration of a solution.
Calcium Bicarbonate Molecular Weight
The molecular weight of Ca(HCO3)2 is 162.114 g/mol. This value is calculated by adding the atomic weights of calcium, hydrogen, carbon, and oxygen in the compound. The molecular weight is important in determining the amount of Ca(HCO3)2 needed in chemical reactions, and in determining the concentration of a solution.
Calcium Bicarbonate Structure
Ca(HCO3)2 has a complex structure due to the presence of both ionic and covalent bonds. The compound consists of a Ca2+ ion and two HCO3- ions held together by ionic bonds. The HCO3- ion itself is a polyatomic ion consisting of a carbon atom, two oxygen atoms, and a hydrogen atom. The carbon atom is double-bonded to one oxygen atom and single-bonded to the other, and the hydrogen atom is attached to one of the oxygen atoms. The structure of Ca(HCO3)2 is important in understanding its reactivity and solubility in water.
| Appearance | White powder |
| Specific Gravity | 2.21 g/cm³ |
| Color | Colorless |
| Odor | Odorless |
| Molar Mass | 162.114 g/mol |
| Density | 2.21 g/mL |
| Melting Point | Decomposes above 50°C |
| Boiling Point | Decomposes above 50°C |
| Flash Point | Not applicable |
| Water Solubility | Soluble |
| Solubility | Soluble in water, insoluble in alcohol |
| Vapour Pressure | Negligible |
| Vapour Density | Not applicable |
| pKa | 6.4 – 10.3 |
| pH | 8.2 – 8.4 |
Calcium Bicarbonate Safety and Hazards
Ca(HCO3)2 is generally considered safe for use in food and beverages by regulatory agencies. However, inhaling Ca(HCO3)2 dust may cause irritation to the respiratory tract. Contact with the eyes may cause irritation or corneal injury. Ingestion of large amounts of Ca(HCO3)2 may cause gastrointestinal irritation. Handling Ca(HCO3)2 may also cause skin irritation or dermatitis in sensitive individuals. It is important to follow proper handling procedures when working with Ca(HCO3)2, such as wearing gloves and eye protection. Additionally, it is important to store Ca(HCO3)2 in a cool, dry place and away from incompatible substances.
| Hazard Symbols | None |
| Safety Description | Non-toxic and safe |
| UN IDs | N/A |
| HS Code | 2836.50.00 |
| Hazard Class | Non-hazardous |
| Packing Group | N/A |
| Toxicity | Non-toxic and safe |
Calcium Bicarbonate Synthesis Methods
The reaction of calcium carbonate (CaCO3) with carbon dioxide (CO2) and water (H2O) synthesizes Ca(HCO3)2. This reaction can occur naturally in certain bodies of water, where carbon dioxide and calcium carbonate are present.
To produce Ca(HCO3)2, one can pass carbon dioxide through a solution of calcium hydroxide (Ca(OH)2). This reaction forms calcium carbonate, which then reacts with excess carbon dioxide to form Ca(HCO3)2.
Another method for synthesizing Ca(HCO3)2 involves reacting calcium chloride (CaCl2) with sodium bicarbonate (NaHCO3). This reaction produces Ca(HCO3)2 as well as sodium chloride (NaCl) and carbon dioxide.
It is important to note that Ca(HCO3)2 is a relatively unstable compound and will decompose into calcium carbonate and carbon dioxide in the presence of heat or acidic conditions. To prevent decomposition, one must handle and store Ca(HCO3)2 with care.
Calcium Bicarbonate Uses
Here are some common uses of Ca(HCO3)2:
- Food and Beverages: Used as a food additive in the production of certain baked goods, leavening agents, and soft drinks.
- Water Treatment: Used to increase the alkalinity of water, which helps to prevent corrosion in pipes and reduce the acidity of acidic water sources.
- Agriculture: Used as a soil amendment to increase the calcium content of the soil, which can improve soil structure and plant growth.
- Pharmaceuticals: Used in some antacid formulations as a neutralizing agent to help relieve heartburn and indigestion.
- Construction: Used as a source of calcium in the production of certain construction materials, such as cement and plaster.
- Cleaning: Used as a mild abrasive in certain cleaning products, such as toothpaste and cleaning powders.
- Cosmetics: Used as a buffering agent in some cosmetic formulations to help maintain the pH of the product.
Questions:
Q: What is calcium bicarbonate?
A: Ca(HCO3)2 is a white, crystalline powder that is formed when calcium carbonate reacts with carbon dioxide and water.
Q: Which three substances are required to interact to form calcium bicarbonate?
A: Calcium carbonate, carbon dioxide, and water are required to interact to form Ca(HCO3)2.
Q: Is calcium bicarbonate a leavening agent?
A: Yes, Ca(HCO3)2 can be used as a leavening agent in baking to help dough or batter rise.
Q: Do calcium bicarbonate ear crystals ever dissolve?
A: Yes, Ca(HCO3)2 ear crystals can dissolve on their own or with treatment, such as through the use of certain medications or maneuvers.
Q: What is the total number of moles of atoms in one mole of Ca(HCO3)2?
A: There are 10 moles of atoms in one mole of Ca(HCO3)2.
Q: How many atoms are present in Ca(HCO3)2?
A: There are a total of 18 atoms present in Ca(HCO3)2, including 1 calcium atom, 2 carbon atoms, 6 hydrogen atoms, and 9 oxygen atoms.
Q: What is Ca(HCO3)2?
A: Ca(HCO3)2 is the chemical formula for calcium bicarbonate, which is a compound formed when calcium carbonate reacts with carbon dioxide and water.