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Baking soda, a seemingly simple, basic, and inexpensive substance, holds a multifaceted nature with various applications. Chemically known as sodium bicarbonate, it is naturally found in mineral deposits, oceans, and lake sediments as trona ore. Within the human body, it plays a crucial role in maintaining blood pH, neutralizing stomach acids, and aiding in the transportation of carbon dioxide. This white crystalline powder, chemically represented as NaHCO3, goes by several names such as sodium bicarbonate, bicarbonate of soda, sodium hydrogen carbonate, or sodium acid carbonate, reflecting its diverse uses.
Sodium bicarbonate is classified as an acid salt, formed by the combination of an acid (carbonic) and a base (sodium hydroxide).
It acts as a mild alkali and reacts with other chemicals. When subjected to temperatures above 300 degrees Fahrenheit (149 degrees Celsius), baking soda undergoes decomposition into sodium carbonate (a more stable substance), water, and carbon dioxide. The discovery of sodium bicarbonate is attributed to two researchers at a Berlin college of medicine in 1800 during a period of great interest in the properties of 'fixed air' or carbon dioxide.
During colonial times in America, baking soda was imported from England, gaining popularity.
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However, it wasn't until 1839 that it began to be produced in the United States. In 1846, a factory was established in New York by Austin Church, a Connecticut physician, and John Dwight, a Massachusetts farmer. This marked the beginning of baking soda production in the U.S., and the company adopted the iconic arm and hammer logo, representing Vulcan, the Roman god of forge and fire.
The inherent chemical and physical properties of baking soda contribute to its versatile range of applications.
It serves as an effective cleaner, deodorizer, and buffer. Unlike masking or absorbing odors, baking soda chemically neutralizes them. Its uses extend to bath salts, deodorant body powders, antacids, and denture cleaning products due to its ability to tabletize. Sodium bicarbonate is a component of some anti-plaque mouthwash products and toothpaste.
As a cleaning agent, baking soda's crystalline structure provides gentle abrasion, making it suitable for removing dirt without causing scratches on sensitive surfaces. Its mild alkalinity transforms fatty acids in dirt and grease into a soap-like substance, facilitating easy dissolution in water and rinsing. Additionally, baking soda functions as a leavening agent in baking, releasing carbon dioxide gas when combined with acidic agents like lemon juice, causing the product to rise.
Beyond its household uses, baking soda finds application in various industrial sectors. It proves valuable in fire extinguishers as it releases carbon dioxide when heated, suppressing flames by excluding oxygen. In air pollution control, baking soda absorbs sulfur dioxide and other acid gas emissions. It is employed in abrasive blastings for surface coating removal, chemical manufacturing, leather tanning, and oil well drilling fluids, where it precipitates calcium and acts as a lubricant. The versatility of baking soda extends to rubber and plastic manufacturing.
In conclusion, baking soda's journey from a basic compound to a household staple and industrial asset underscores its remarkable versatility. From its chemical composition to varied applications, sodium bicarbonate has woven itself into the fabric of everyday life and industry. Its story is one of adaptability, resilience, and continuous discovery, showcasing the dynamic relationship between science and practicality.
The Versatility of Baking Soda: From Chemistry to Applications. (2018, Aug 25). Retrieved from https://studymoose.com/history-of-baking-soda-essay
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