Magnesium bicarbonate, also known by its IUPAC name magnesium hydrogen carbonate, is a salt containing bicarbonate anion and magnesium cation represented by the formula C₂H₂MgO₆ or Mg(HCO₃)₂ ^[1]. Since magnesium bicarbonate is unstable in a solid state, it exists in a dilute aqueous solution ^[2].

Magnesium Bicarbonate Identification
CAS Number	2090-64-4 [1]
PubChem CID	102204 [1]
ChemSpider ID	92335 [3]
EC Number	235-192-7 (EU Food Improvement Agents) 218-240-1 (ECHA) [1]
UNII	19E9A0647O [1]
InChI Key	QWDJLDTYWNBUKE-UHFFFAOYSA-L [1]

How is Magnesium Bicarbonate Prepared

It can be synthesized by treating magnesium acetate with sodium bicarbonate, involving the following reaction:

Mg(CH₃COO)₂ + 2NaHCO₃ → Mg(HCO₃)₂ + 2CH₃COONa

A solution of Mg(HCO₃)₂ commonly called magnesium bicarbonate water can be produced through the reaction of magnesium hydroxide (such as milk of magnesia) and pressurized carbon dioxide (like seltzer water) ^[4]:

Mg(OH)₂ + 2CO₂ → Mg(HCO₃)₂

The resulting solution when dried decomposes magnesium bicarbonate into magnesium carbonate, water, and carbon dioxide:

Mg + 2HCO₃ → MgCO₃ + CO₂ + H₂O

Properties and Characteristics of Magnesium Bicarbonate

General Properties
Molar Mass/Molecular Weight	146.337 g/mol [1]
Physical Properties
Color and Appearance	Light, white, unstable friable mass or powder  [1, 2]
Odor	Odorless [2]
Melting Point	N/A
Boiling Point	333.6 °C, 632.48 °F [2]
Charge	0 (Mg2+ and HCO3–) [1]
State of matter at room temperature	Unstable in solid form but exists in the liquid state [2]
Solubility	Insoluble in ethanol [1]
Solubility in Water	Almost insoluble in water (0.077 g per 100 mL) [1]

Uses

• Magnesium bicarbonate has numerous health benefits and is used for resisting changes in blood pH and keeping it within an optimal range ^[5].
• As an essential mineral, it helps in blood pressure regulation, protein synthesis, nerve and muscle functions, and blood glucose control in the human body ^[5].
• It is used as food additives like acidity regulators, alkali, anti-cracking and bleaching agents ^{[1, 6]}.

References
1. Carbonic Acid, Magnesium Salt (2:1) – Pubchem.ncbi.nlm.nih.gov
2. Magnesium Bicarbonate – Mg(HCO₃)₂ – Byjus.com
3. Magnesium Bicarbonate – Chemspider.com
4. Preparation of Solutions of Magnesium Bicarbonate for Deacidification – Jstor.org
5. Magnesium Bicarbonate Water – The importance of bicarbonates and magnesium – Dancingwithwater.com
6. Acidity Regulators – Chm.bris.ac.uk