ACIDS BASES Properties of an Acid Sour Taste

ACIDS & BASES

Properties of an Acid Sour Taste Corrosive Changes color when reacting with an indicator An indicator is an organic compound that changes color in acid and base. Acids will turn blue litmus paper red

Common Acids Foods such as citrus fruits, yogurt, pickles contain acid Your stomach uses hydrochloric acid to digest food Sulfuric, phosphoric, nitric, and hydrochloric acids are used in industrial applications

Common Acids Acid Acetic acid Acetylsalicylic acid Asorbic acid Carbonic acid Hydrochloric acid Nitric Acid Phosphoric acid Sulfuric acid Uses Vinegar Asprin Vitamin C In carbonated drinks In stomach, used to clean steel Used to make fertilizers Used to make detergent, fertilizer, soft drinks Car batteries, fertilizers, and other chemicals

Properties of Bases Bitter taste Slippery to touch Corrosive Create a predictable color change with an indicator Turns litmus paper blue In their pure state, many bases are solids

Common Bases Used in drain cleaners Soap Milk of magnesia

Common Bases Base Use Aluminum hydroxide Color-fast farics, antacid, water treatment Calcium hydroxide Leather making, plaster Magnesium Laxative, antacid hydroxide Sodium Hypochlorite Ammonia Makes soap, oven cleaner, drain cleaner, paper Bleach Cleaner, fertilizer, to make rayon and nylon

Solutions of Acids and Bases Many common acids and bases are actually solutions Cleaning products and vinegar are a solution of base or acid

How do we define and acid and a base? There are 3 theories as to what acids and bases are. They are Arrhenius, Bronsted-Lowry, and Lewis Theory.

What is an Acid and Base? (Arrhenius) An acid is a substance that produces hydrogen ions (H+) when dissolved in a water solution Acids contain hydrogen in their chemical formula These hydrogen ions react with the water molecules and form hydronium ions (H 3 O+) Any substance that forms hydroxide ions (OH-) in a water solution is called a base Most bases will end in hydroxide (OH)

HCl -> H+ (aq) + Cl- (aq) Na. OH -> Na+ (aq) + OH- (aq)

Bronsted-Lowry Acids and Bases Arrhenius definition does not fit the bases of NH 3 and Na 2 CO 3 In Bronsted-Lowry theory, an acid is something that donates protons while a base is something that accepts them. In this case a H+ and a proton are the same thing. Everything that is an acid or base under Arrhenius is an acid or base under Bronsted. Lowry

Bronsted-Lowry Acids and Bases NH 3 + H 2 O -> NH 4 + + OH BASE ACID Which is the acid and which is the base?

Conjugate Acids and Bases Conjugate Base NH 3 + H 2 O -> NH 4 + + OH Conjugate Acid What is is a conjugate acid or base? A conjugate acid is the particle formed when a base gains a hydrojetn ion. A conjugate base is the particle that remains when an acid has donated a hydrogen ion Together, they are a conjugate acid/base pair

Examples HCl + H 2 O -> H 3 CA CB + O + Cl ACID BASE H 2 SO 4 + H 2 O -> H 3 O+ + HSO 4 ACID BASE CA CB

Lewis Acids and Bases A Lewis acid is something that accepts electron pairs to form a covalent bond A Lewis base is something that donates electron pairs to form a covalent bond