Profile
Settings
Refer your friends
Sign out
Magnesium hydroxide is a chemical compound with the formula Mg(OH)2. Magnesium hydroxide is a magnesium-containing compound. It can be found naturally as the mineral brucite. It appears in water as a white solid with a low solubility (Ksp = 5.611012). Magnesium hydroxide, a common component of the compound, is found in antacids such as milk of magnesia.
Magnesium hydroxide is an inorganic chemical compound found in nature as a white solid. Hydroxide is defined as any polyatomic anion composed of oxygen and hydrogen with the chemical formula (OH-) indicating that it is a single negative charge anion. In general, it is well understood that magnesium atoms can donate two electrons in order to form an anion and achieve a stable electronic configuration. This results in the formation of magnesium hydroxide, an acidic neutral salt compound formed by the reaction of a monatomic anion of magnesium and a polyatomic anion of hydroxide. The chemical formula for magnesium hydroxide, Mg(OH)2, is derived from this. In some circles, it is also known as milk of magnesia, and the formula for magnesium hydroxide is the same as the formula for milk of magnesia.
Properties of Magnesium Hydroxide
The mineral magnesium hydroxide, which occurs naturally in the environment, is known as brucite. It occurs naturally in chlorite in the form of 1:2:1 clay minerals, where it is found in the interlayer position between the mineral layers. Magnesium hydroxide salt has the physical properties of a white crystalline solid mineral with a crystalline structure.
The following are some of the most common physical properties of magnesium hydroxide:
The molar mass of magnesium hydroxide is 58.3197 grams per mole of magnesium hydroxide, according to the magnesium hydroxide chemical formula.
An odourless inorganic compound with the chemical formula for magnesium hydroxide.
It’s worth noting that the chemical formula for magnesium hydroxide represents a compound with a very low solubility in water.
In its solid state, magnesium hydroxide has a hexagonal crystal structure.
It is not recommended for use because it is non-flammable.
Applications and Reactions
The reaction of magnesium salts with alkaline water produces magnesium hydroxide, and because magnesium hydroxide is extremely poorly soluble in water, it is separated from the water by precipitation. The following reactions for this method of production are described:
Mg2++ 2OH-→ Mg(OH)2
The above equation is by far the most effective for writing down the formula for magnesium hydroxide while also depicting the ionic forms of the component molecules.
The industrial production of magnesium hydroxide is accomplished by treating seawater with lime, which is made up of the elements calcium and oxygen.
Calcium hydroxide is more soluble in water than magnesium hydroxide, which is insoluble in water and precipitates as a solid, making the separation of the two compounds easier. The following reactions occur as a result of this manufacturing method:
Magnesium oxalate is formed when magnesium oxide and water are combined.
The industrial production of magnesium oxide, also known as magnesia, is a common application for magnesium hydroxide, which is important because it has the dual properties of low electrical conductivity and high thermal conductivity, making it a useful material for a variety of applications. When the chemical formula for magnesium hydroxide is written out completely, the fact that MgO can be obtained from it is easily understood.
One of the most common applications for magnesium hydroxide is as an antacid or a laxative in suspension form. The compound works via a simple neutralisation reaction in which the hydroxide ions from the magnesium hydroxide combine with the H+ ions from the hydrochloric acid produced by the parietal cells in the stomach to form water. The reaction is straightforward and simple.
Because magnesium hydroxide is directly absorbed by foods, it has received worldwide approval from the Food and Drug Administration (FDA). It has been marketed for medical purposes in the form of chewable tablets, capsules, powder, and liquid suspensions, all of which come in a variety of flavouring options. In some cases, it is also used as an antiperspirant. Magnesium hydroxide can also be used topically to treat canker sores (aphthous ulcers). Aside from that, it is used in the industrial neutralisation of acidic waters, and in its natural state, its mineral form is used as a fire retardant.
Side effects are possible with magnesium hydroxide-containing medications.
Severe nausea, vomiting, or diarrhoea; no bowel movement after using the medication as a laxative; rectal bleeding; or worsening symptoms are possible.
Conclusion
Finally, magnesium hydroxide is a good thermal conductor due to its high melting point, but it is a poor electrical conductor due to its low conductivity. When taken as a suspension, it acts as a laxative and an antacid. It is used in food products as an additive. It is widely used in wastewater treatment.
