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Many industrial operations, including the creation of fertilizers, dyes, and detergents, as well ase batteries, depend heavily on acids. m BASE Bases are compounds that take hydrogen ions (H+) in aqueous solutions and have a pH greater than 7. They are distinguished by their bitter flavor and slick texture. In a process referred to as neutralization, bases and acids combine to produce salts and water. A base's strength is determined by its dissociation constant and its concentration of hydroxide ions (OH-) (Kb). The creation of soap, textiles, and medications as well as their use as cleaning agents are only a few of the practical uses for bases. * 02 REAL-WORLD APPLICATIONS * Acids and bases are used often in industry and daily life and are essential to several activities. Acids like citric acid are used in the food and beverage industry as preservatives and to flavor confectionery and soft drinks. Fabrics, soap, and chocolate are all made using bases like sodium hydroxide. In household cleaning, bases like baking soda and ammonia are frequently used for their cleaning and degreasing characteristics whereas acids like vinegar and lemon juice are utilized for their cleansing and deodorizing capabilities. Weak bases like ammonia and weak acids like aspirin are used in medicine to treat pain and neutralize stomach acid, respectively. These are just a some examples of the many ways where acids and bases are part of daily life. * 03 THEORIES + EQUATIONS * ACID-BASE THEORIES ARRHENIUS According to this theory, bases are chemicals that raise the concentration of hydroxide ions (OH-) in a solution while acids raise the concentration of hydrogen ions (H+). BRONSTED-LOWRY Bases serve as proton acceptors while acids serve as proton donors. This idea states that a proton is transferred from the acid to the base during an acid- base reaction. LEWIS By designating bases as electron pair donors and acids as electron pair acceptors, this theory builds on the Bronsted-Lowry theory. An electron pair is transferred from the base to the acid during a Lewis acid-base reaction. ACID-BASE EQUATIONS ARRHENIUS Equation for the dissociation of an acid HA in water: HA+H20 H30++ A- BRONSTED-LOWRY HA+B=A- + HB+ where HA is the acid, B is the base, A- is the conjugate base of the acid, and HB+ is the conjugate acid of the base. LEWIS B:AB-A where B is the Lewis base (the electron pair donor) and A is the Lewis acid (the electron pair acceptor). THANK YOU FOR LISTENING C *