Is a strong electrolyte in aqueous solution?

- Yes, a strong electrolyte is a substance that completely dissociates into ions when dissolved in water or any other polar solvent, resulting in a high conductivity of electric current. - According to the Arrhenius theory of electrolytes, a strong electrolyte is a substance that dissociates completely in water to produce ions, such as acids, bases, and salts (1). The dissociation occurs through a process called ionization, where the solid compound breaks up into its constituent ions, which are then surrounded by water molecules. - Strong electrolytes significantly contribute to electrical conductivity due to the high concentration of ions in the solution. This conductivity allows the substance to conduct electricity when electrodes are placed in the solution, resulting in the flow of electric current through the solution. - In contrast, weak electrolytes only partially dissociate into ions when dissolved in water, resulting in a lower conductivity of electric current. Examples of weak electrolytes include weak acids like acetic acid and weak bases like ammonia (2). - Strong electrolytes are commonly used in various industries and scientific research. For instance, in analytical chemistry, strong electrolyte solutions are often used as electrolyte media in electrochemical cells, electrolysis, and for preparing standard solutions. - Strong electrolytes can play a crucial role in biological processes as well. Many essential ions and molecules in our body, such as sodium, potassium, calcium, and chloride ions, function as strong electrolytes and are involved in maintaining the proper functioning of cells and tissues. - Some examples of strong electrolytes include sodium chloride (NaCl), hydrochloric acid (HCl), sulfuric acid (H2SO4), and potassium hydroxide (KOH) (3). Sources: 1. Chang, R. (1998). Chemistry (6th ed.). Boston: McGraw-Hill Higher Education. 2. Zumdahl, S. S., & Zumdahl, S. A. (2012). Chemistry (9th ed.). Boston, MA: Cengage Learning. 3. Silberberg, M. S. (2011). Chemistry: The Molecular Nature of Matter and Change (6th ed.). New York, NY: McGraw-Hill Education.

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