NaH2SO4, also known as sodium bisulfate, is a white crystalline solid that is highly soluble in water. When NaH2SO4 is added to water, it readily dissolves and dissociates into its constituent ions:

NaHSO4(s) → Na+(aq) + HSO4-(aq)



The HSO4- ion is a weak acid and can donate a proton to water molecules to form H3O+ ions and SO42- ions:

HSO4-(aq) + H2O(l) → H3O+(aq) + SO42-(aq)

This reaction results in the solution becoming acidic. The degree of acidity depends on the concentration of HSO4- ions in the solution. The more NaH2SO4 added to the water, the more HSO4- ions are released, making the solution more acidic.



NaH2SO4 has several practical uses. It is commonly used as a pH adjuster in swimming pools and in the production of detergents. It is also used in the food industry to acidify foods and as a preservative. In addition, NaH2SO4 is used as a reducing agent in certain industrial processes.



Although NaH2SO4 is generally considered safe, it can be corrosive to skin, eyes, and mucous membranes. It should be handled with care and appropriate personal protective equipment should be worn. In case of skin or eye contact, the affected area should be washed with copious amounts of water and medical attention sought if necessary.