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Chemistry-Arrhenius Base
Chemistry (CHM104)
Rockland Community College
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Chemistry Arrhenius Base - An Arrhenius base is a substance that, when dissolved in water, increases the concentration of hydroxide ions (OH-) in the solution. - According to the Arrhenius theory of acids and bases, a base is defined as a substance that produces hydroxide ions (OH-) when dissolved in water. - The Swedish chemist Svante Arrhenius proposed this theory in 1884, which states that when a base is dissolved in water, it dissociates into hydroxide ions (OH-) and cations. - For example, when sodium hydroxide (NaOH) is dissolved in water, it dissociates into hydroxide ions (OH-) and sodium ions (Na+): NaOH(aq) → Na+(aq) + OH-(aq) - Arrhenius bases are characterized by their ability to accept hydrogen ions (H+) in aqueous solution. - Strong bases, such as sodium hydroxide (NaOH), potassium hydroxide (KOH), and calcium hydroxide (Ca(OH)2), dissociate almost completely in water to produce high concentrations of hydroxide ions (OH-). - Weak bases, such as ammonia (NH3) and carbonates (CO32-), dissociate only partially in water to produce lower concentrations of hydroxide ions (OH-). - Arrhenius bases are important in many different fields, such as chemistry, biology, and medicine. - They are used in the production of many different types of chemicals, including soaps, detergents, and pharmaceuticals.
- They are also involved in many biological processes, such as the regulation of blood pH and the functioning of enzymes.
Chemistry-Arrhenius Base
Course: Chemistry (CHM104)
University: Rockland Community College
