Sodium bisulfate is the sodium salt of sulfuric acid. It is an odorless, colorless, water-soluble crystalline compound useful in household and commercial industries. In pure form, sodium bisulfate exists as a corrosive acid, with a high melting point. Its high degree of acidity lends itself to industrial cleaning products, able to clean a variety of surfaces. Although the chemical itself is toxic, when added to foods, its acidic properties help prevent premature spoilage.
Chemical Properties
The chemical formula of sodium bisulfate is NaHSO4. This indicates that each molecule of sodium bisulfate consists of one atom of sodium, Na; one atom of hydrogen, H; one atom of sulfur, S; and four atoms of oxygen. Sodium bisulfate exists in solution with a pH of 1.4, making it extremely acidic. Crystals of sodium bisulfate melt at 136 degrees Fahrenheit. As an hygroscopic compound, it absorbs moisture. Although sodium bisulfate is a stable compound under normal storage conditions, decomposition releases dangerous sulfur oxides.
Food Additive
Sodium bisulfate acts as an acidulant when used a food additive. Acidulants are acids that, when added to food, impart a tart or sour taste. This helps enhance flavor. Acidulants also act as preservatives, helping prevent the growth of bacteria by lowering the pH, or increasing its acidity. Although most acidulants are organic acids, sodium bisulfate is an exception.
Toxicity
Sodium bisulfate toxicity can be acute or chronic. In acute toxicity, sodium bisulfate corrodes and burns the human body upon ingestion, severely burning the mouth, throat and stomach, leading to a painfully sore throat, vomiting, diarrhea and even death. Direct contact with skin or eyes causes pain, redness and burning. Inhalation of the pure chemical form irritates the lining of the nose and throat, and damages mucous membranes and the upper respiratory tract.
Chronic exposure to wet or moist forms of sodium bisulfate chemical causes respiratory problems including lung irritation, tracheal bronchitis and coughing. In some cases, excessive exposure to breathing dust particles of sodium bisulfate through the mouth corrodes the teeth.
Household Use
Sodium bisulfate provides acidic-based cleaning for a variety of household cleaning products, such as toilet bowl cleaners. In addition, the acidity of sodium bisulfate provides chemical cleaning power useful for home pool maintenance. In swimming pools, sodium bisulfate, also called "dry acid," removes hard water stains and iron deposits, as well as organic matter, tarnish and corrosion. Commonly sold under the name of pH decreaser, sodium bisfulate neutralizes alkaline discoloration and decreases the alkalinity of the pool water, making it more neutral.
Fabric Bleaching
Sodium bisulfate creates unique designs in fabrics through a process called devoré, or burn-out. In this process, sodium bisulfate is placed in specific areas on composite fabrics, such as cellulose/synthetic or cellulose/protein blends. The physical placement of the sodium bisulfate on the fabric determines the patterns that result. The sodium bisulfate selectively burns out the cellulose fibers in the fabric, leaving the remainder of the fabric intact. Cut velvet is an example of the results of the devoré process.
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