Electrolytes are compounds that dissociate into ions in solution and have the ability to conduct electricity. The following compounds are known to be electrolytes: 1. Inorganic salts: - Sodium chloride (NaCl): Common table salt readily disassociates into sodium ions (Na+) and chloride ions (Cl-) when dissolved in water, making it a strong electrolyte. - Potassium chloride (KCl): Similar to sodium chloride, it dissociates into potassium ions (K+) and chloride ions (Cl-) in water, acting as an electrolyte. - Calcium chloride (CaCl2): This compound dissociates into calcium ions (Ca2+) and chloride ions (Cl-) in solution and is commonly used in electrolyte solutions for medical purposes. 2. Acids and bases: - Hydrochloric acid (HCl): When dissolved in water, HCl completely ionizes into hydrogen ions (H+) and chloride ions (Cl-), making it a strong acid electrolyte. - Sulfuric acid (H2SO4): This strong acid electrolyte fully dissociates into hydrogen ions (H+) and sulfate ions (SO4^2-) in an aqueous solution. - Sodium hydroxide (NaOH): Strong base electrolyte, it dissociates into sodium ions (Na+) and hydroxide ions (OH-) when dissolved in water. 3. Ionic compounds: - Magnesium sulfate (MgSO4): This compound disassociates into magnesium ions (Mg2+) and sulfate ions (SO4^2-) in water, acting as an electrolyte. - Calcium phosphate (Ca3(PO4)2): Although less soluble in water, calcium phosphate can still partially dissociate into calcium ions (Ca2+) and phosphate ions (PO4^3-), making it a weak electrolyte. Sources: - Kumar, R., & Sinha, S. (2012). Chemistry: Preparatory Manual for Undergraduates. New Age International. - Timberlake, K. C. (2016). Chemistry: An Introduction to General, Organic, and Biological Chemistry. Pearson. - Petrucci, R. H., Herring, F. G., Madura, J. D., & Bissonnette, C. J. (2017). General Chemistry: Principles and Modern Applications. Pearson.
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