Acids and Bases l Properties of Acids and Bases Ionization l Acid-Base Theory l Acid-Base Reactions l Neutralization Reactions

Properties of Acids l Characteristics – Aqueous acid solutions have a sour taste – Acids change the color of acid-base indicators – Some acids react with active metals to release hydrogen gas, H 2 – Acids and bases produce salts and water – Some acids conduct electric current.

Properties of Acids l Acid Nomenclature – Binary Acid: has two different elements (Hydrogen and an electronegative element) – Binary Nomenclature The name begins with the prefix (Hydro-) The second element is the root which follows this prefix The name then ends with the suffix (-ic) – Oxyacid: An acid with hydrogen, oxygen, and a third element, usually a nonmetal

Properties of Acids l Common Industrial Acids – Sulfuric Acid: Most common acid used as an effective dehydration agent – Nitric Acid: Volatile unstable dissolving agent rarely used industrially – Phosphoric Acid: A nutritional and flavoring agent for food and fertilizer – Hydrochloric Acid: AKA muriatic acid, used to remove surface impurities of metals – Acetic Acid: A common natural product of organic processes like fermentation

Properties of Acids l Common Industrial Acids – Sulfuric Acid: Most common acid used as an effective dehydration agent – Phosphoric Acid: A nutritional and flavoring agent for food and fertilizer – Hydrochloric Acid: AKA muriatic acid, used to remove surface impurities of metals – Nitric Acid: A common natural product of organic processes like fermentation – Acetic Acid: Volatile unstable dissolving agent rarely used industrially

Properties of Bases l Characteristics – Aqueous base solutions have a bitter taste – Bases change the color of acid-base indicators – Dilute solutions of bases feel slippery – Bases and acids produce salts and water – Bases conduct electric current.

Arrhenius Acids and Bases l Characteristics l Aqueous Solutions of Acids: The Hydrogen usually disassociates/ionizes from the acid l Aqueous Solutions of Bases

Arrhenius Acids and Bases l Characteristics – Arrhenius Acid: increases Hydrogen ions, H + concentration of aqueous solutions – Arrhenius Base: increases Hydroxide ions, OH - concentration of aqueous solutions

Arrhenius Acids and Bases l Aqueous Solutions of Acids: The Hydrogen usually disassociates/ionizes from the acid – Strength of Acids Strong Acids: one that ionizes completely in an aqueous solution Weak Acids: one that partially ionizes and forms a weak electrolyte

Arrhenius Acids and Bases l Aqueous Solutions of Bases: – Alkaline: a base that completely disassociates to form Hydroxide ions, OH - – Strength of Bases Strong Bases: form strong electrolytes in aqueous solutions Weak Bases: form weak electrolytes in aqueous solutions

Acid Base Theory l Acid-Base Theory – Bronstead-Lowry Acids and Bases – Lewis Acids and Bases

Bronstead-Lowry Theory l Bronstead-Lowry Acids and Bases – Bronstead-Lowry Acid: a molecule or ion that is a proton donor, usually a H + All Arrhenius Acids are Bronstead-Lowry Acids Not all Bronstead-Lowry Acids are Arrhenius Acids – Bronstead-Lowry Base: a molecule or ion that is a proton acceptor, usually a H + – Bronstead-Lowry Acid-Base reaction: a proton transfer from one reactant to another, usually a H + from an Acid to a Base

Bronstead-Lowry Theory l Monoprotic and Polyprotic Acids – Monoprotic Acid: an acid that can donate only one proton (H + ) per molecule – Polyprotic Acid: an acid that can donate more than one proton (H + ) per molecule Diprotic Acid: an acid that can donate two protons (H + ) per molecule Triprotic Acid: an acid that can donate three protons (H + ) per molecule

Lewis Theory l Lewis Acids and Bases – Lewis Acid: An atom, ion, or molecule that accepts a pair of e - to form a covalent bond – Lewis Base: An atom, ion, or molecule that donates a pair of e - to form a covalent bond – Lewis Acid-Base Reaction: forming one or more covalent bonds by transferring electrons

Acid-Base Reactions l Characteristics l Strength of Conjugate Acids and Bases l Amphoteric Compounds: A species that can react as either an Acid or a Base

Acid-Base Reactions l Characteristics – Conjugate Base: The species that remains after a Bronstead-Lowry Acid donates a proton – Conjugate Acid: The species that is formed by a Bronstead-Lowry Base accepting a proton

Acid-Base Reactions l Strength of Conjugate Acids and Bases – The stronger the an Acid is, the weaker the conjugate Base is – The stronger the Base is, the weaker the conjugate Acid is – The proton transfer reaction favors the production of the weaker acid and weaker base

Acid-Base Reactions l Amphoteric Compounds: A species that can react as either an Acid or a Base – Molecules with an –OH – Hydroxyl Group: a molecule with a covalently bonded -OH Can be acidic or Amphoteric The acidity increases with the number of Oxygen atoms

Neutralization Reactions l Strong Acid-Strong Base Neutralizations – Neutralization: reaction of Hydronium ions and Hydroxide ions to form water molecules – Salt: an ionic compound of a cation from a base and an anion from an acid l Acid Rain – Gases such as NO, NO 2, CO 2, SO 2, and SO 3 can dissolve in the atmosphere to form acids