Barium Bromide Formula

Barium bromide Formula

From this article students will be able to learn about Barium Bromide Formula.

Barium bromide Formula Structure

The Barium Bromide Formula is also known as the barium (2+) dibromide formula. In aqueous form, it acts as a simple salt, but crystallizes in the lead chloride motif, forming deliquescent orthorhombic white crystals. Barium bromide’s molecular or chemical formula is BaBr2 (anhydrous).

Barium (2+) dibromide can be made by reacting barium carbonate or barium sulphide with hydrobromic acid (HBr) to produce hydrated barium bromide.

Properties Of Barium bromide Formula

Some of the Physical properties of Barium Bromide Formula are:

  1. Molecular Weight: Barium bromide has a molecular mass of 297.14 gram per mole.
  2. Melting Point: Barium bromide has a high melting point. At 857 degrees Celsius, the inorganic compound melts.
  3. The boiling point of barium bromide is 1835 degrees Celsius.
  4. Density: The barium bromide formula has a density of 4.78 g/cm3.
  5. Solubility: The inorganic compound BaBr2 dissolves in its own water-of-hydration at 75 degrees Celsius. It usually dissolves before the anhydrite decomposes.

Some of the Chemical properties of Barium Bromide Formula are:

The compound barium bromide is a white crystalline powder.

  1. The compound BaBr2 is made up of three covalently bonded units.
  2. This inorganic compound has a molecular weight of 297.74 grams. The monoisotopic mass of BaBr2 is, however, 297.742 grams per mole.
  3. In the barium bromide formula, the number of hydrogen bond donors is equal to 0.
  4. In barium bromide, the number of hydrogen bond acceptors is equal to two.

What is Barium Bromide?

Barium Bromide Formula, also known as BaBr2, is a significant chemical compound. It is also known as barium (2+) dibromide or anhydrous barium bromide. It appears as a white solid that is water soluble but toxic in aqueous form.

Crystallization of barium (2+) dibromide to lead chloride motifs results in white, deliquescent orthorhombic crystals. It behaves like a simple salt in aqueous solution. It reacts with the sulpuric acid (H2SO4) ion to form barium sulphate (BaSO4) precipitates.

Derivation of Barium Bromide Formula

By reacting barium carbonate or barium sulphide with hydrobromic acid (HBr), hydrated barium bromide can be produced. The reaction is given below for students understanding:

BaS + 2HBr → BaBr2 + H2S

BaCO3 + 2HBr → BaBr2 + CO2 + H2O

In its dihydrate form, barium (2+) dibromide can be crystallised from solution. BaBr2H2O becomes anhydrous when heated to around 120 °C.

Students can learn more about the derivation of Barium Bromide Formula from the website and mobile application of Extramarks. Extramarks’ resources will help students understand the basic concepts of Chemistry fully.

Uses of Barium Bromide

There are various uses of the Barium Bromide Formula. Some of the uses are given below:

  1. In the chemical industry, barium bromide is used as a precursor.
  2. Barium Bromide is used by Photographers.
  3. It is used to purify radium through a process known as fractional crystallization.
  4. It is also used in the production of other bromides.
  5. Barium Bromide is used in the manufacture of phosphors.

To learn more about the various uses of Barium Bromide Formula, students must download the resources provided by Extramarks. Extramarks provides resources such as NCERT Solutions, Revision notes, Past years’ papers solutions etc. All the resources offered by Extramarks are written by expert subject teachers.

Health Hazards of Barium Bromide

There are several known risks associated with the use of the Barium Bromide Formula. Inorganic compounds containing barium can inhibit intracellular potassium inflow. As a result, potassium is transferred from the extracellular compartment to the intracellular compartment. The resting membrane potential decreases, which electrically excited the muscle fibres. As a result, it can cause paralysis.

When Barium Bromide Formula is ingested, it can cause severe poisoning in humans.

Bromine is a powerful oxidizer. It can extract free oxygen radicals from water and release them into mucous membranes. The free radicals produced can act as powerful oxidizers, causing tissue damage.

Furthermore, the formation of bromic acids can affect the outcome of secondary irritation. It can also cause bromism, which has an effect on the central nervous system.

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