Chemical Reactivity of Sodium Bicarbonate with Halogen

The most crucial leavening ingredient in wafers & waffles, and usually the only one, is sodium bicarbonate. For soft, well-filled, & also well – formed wafers and waffles, the pH value rises, the flour acids are neutralised, and the batter distributed more evenly and easily in the hot baking mould. The browning is accelerated when the pH value rises. Additionally, the sodium bicarbonate concentration balances out any effects from the water’s pH level.

Overview of Sodium Bicarbonate

Monoclinic crystalline structure describes sodium bicarbonate, also known as sodium hydrogen carbonate. In the year 1791, a French chemist named Nicolas Leblanc created sodium carbonate. The first plant to make baking soda was established by New York bakers Austin Church & John Dwight in the year 1846. It is a white, crystalline, solid chemical substance that is typically in the form of powder. Sodium ions & bicarbonate ions make up this salt. Its chemical name is NaHCO3. Its foundation is thin. It is used in cooking and is frequently referred to as baking soda. pH is around 8.31.

A salt called sodium bicarbonate decomposes in water to produce sodium and bicarbonate. A solution becomes alkaline as a result, making it capable of neutralising acid.

The capacity of sodium bicarbonate to neutralise acid aids in the treatment of diseases associated with high acidity in bodily fluids, including indigestion, which is brought on by excess acid in the stomach.

Sodium Bicarbonate Uses

  1. In order to kill cockroaches and stop the growth of fungus, Sodium Bicarbonate is used as pest control.

  2. It serves as a disinfectant and as a barrier against irritation and odour in the armpit area.

  3. It is employed in cooking, particularly for baking food.

  4. It is given intravenously in medicine to lessen the negative effects of chemotherapy.

  5. Because of its antibacterial characteristics, Sodium Bicarbonate is used to wash kitchen items.

  6. It is used to keep the mouth and teeth clean.

Sodium Bicarbonate and Halogen

Halogen

Nonmetals are halogens. Fluorine, chlorine, and bromine are all gases at ambient temperature while bromine is a liquid. Astatine and iodine are both solids. Halogens are extremely reactive; from fluorine to astatine, the reactivity diminishes. In nature, halogens do not occur in their elemental form. The radioactive astatine isotopes have brief half-lives.

Any of the 6 non-metallic elements that make up Group 17 in the periodic table are considered halogens. Fluorine (F), Chlorine (Cl), Bromine (Br), Iodine (I), Astatine (At), and Tennessine (Ts) are the halogen elements.

The free halogen elements are not found naturally due to their high reactivity. Fluorine is the halogen that is present in the highest concentration in the crust of the Earth. Due to the fact that they are made up entirely of transient radioactive isotopes, astatine and tennessine are not found in nature.

Halogen Uses

  1. Water, open wounds, swimming pools, dishes, and surfaces are frequently disinfected with bromine and chlorine.

  2. Halogen lamps contain trace amounts of a halogen, like iodine or bromine.

  3. Products like toothpaste, infant formula, and vitamin supplements all include fluoride.

  4. About 0.15 percent of a person’s body weight is chlorine, which plays a number of crucial roles in the body’s operation. Chlorine and bromine compounds are both employed as disinfectants and sterilisers.

Chemical Reactivity of Sodium Bicarbonate with Halogen

Halogen and sodium bicarbonate combine to form sodium halide, sodium halate, carbon dioxide, and water

Sodium Bicarbonate + Halogen →sodium halide+ sodium halate+ carbon dioxide+water

Reaction with Chlorine

Chlorine and sodium bicarbonate combine to form sodium chloride, sodium chlorate, carbon dioxide, and water. Concentrated sodium bicarbonate solution. A boiling solution serves as the reaction’s medium.

6NaHCO3 + 3Cl2 → NaClO3 + 5NaCl + 3H2O + 6CO2

Reaction with Bromine

6NaHCO3 + 3Br2 → NaBrO3 + 5NaBr + 3H2O + 6CO2

Bromine and sodium bicarbonate combine to form sodium bromide, sodium bromate, carbon dioxide, and water. Concentrated sodium bicarbonate solution. A boiling solution serves as the reaction’s medium.

Reaction with Iodine

6NaHCO3 + 3I2 → NaIO3 + 5NaI + 3H2O + 6CO2

Iodine and sodium bicarbonate combine to form sodium iodide, sodium iodate, carbon dioxide, and water. 

Conclusion

Monosodium salt of the carbonic acid with electrolyte replacement & alkalinizing characteristics is sodium bicarbonate. Sodium bicarbonate breaks down to sodium & bicarbonate ions. 

A white, crystalline powder known as sodium bicarbonate is frequently used as a pH buffer, an electrolyte restorer, a systemic alkalizer, and in topical cleansing treatments.

The halogens are the elements that make up group 17. Fluorine, Chlorine, Bromine, Iodine, & Astatine are the halogen elements. Fluorides, Bromides, & Iodides are less prevalent but still decently available, with chlorides being the most common.

Halogen and sodium bicarbonate combine to form sodium halide, sodium halate, carbon dioxide, and water

Sodium Bicarbonate + Halogen → sodium halide + sodium halate + carbon dioxide + water

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