Acids and Bases

Arrhenius Acid Compound that increases the concentration of hydrogen ions (H+1) in an aqueous solution. Example of ionization: HCl → H+1 + Cl-1

Arrhenius Base Compound that increases the concentration of hydroxide ions (OH-1) in an aqueous solution. Example of ionization: NaOH → Na+1 + OH-1

Bronsted-Lowry Definition Involves the movement of a proton (hydrogen ion)

Bronsted-Lowry Acid Molecule that is a proton donor. Conjugate base: species that is left over after a Bronsted-Lowry acid has given up a proton.

Bronsted-Lowry Base Molecule that is a proton acceptor. Conjugate acid: species that is formed when a Bronsted-Lowry base has gained a proton.

Things Acids and Bases Have In Common Change colors of indicators React together to form water and salt Conduct electricity (electrolytes)

The most common types of indicators are: Indicators – solutions that change color based on the amount of hydrogen ions found (pH). The most common types of indicators are: Phenolphthalein Bromothymol blue Litmus paper Universal indicator

Properties of Acids Sour taste React with metals to produce hydrogen (H2) gas All contain hydrogen (H+1) ions pH < 7

Properties of Bases Bitter taste Feels slippery  All contain hydroxide (OH-1) ions pH > 7

pH Scale Measures the amount of hydrogen ions in solution. Strong Weak Neutral Weak Strong Acid Base 0 1 2 3 4 5 6 7 8 9 10 11 12 13 14 Battery Acid Gastric Acid Hydrochloric Acid Soda Acid Rain Black Coffee Urine, Saliva Pure Water Blood Sea Water Baking Soda Milk of Magnesia Ammonia Soap Bleach Drain Cleaner

Strength of Acids and Bases Based on the amount of ions in solution Strong acids/bases - completely ionize in aqueous solutions - great conductors of electricity (electrolytes) Weak acids/bases - do NOT completely ionize (some molecules of that compound do not ionize)

Acid Nomenclature (Naming) Binary acids:  contain only 2 different elements and hydrogen must be the first element Use “hydro” as prefix and “ic” as suffix + the word “acid” at the end Example: HBr =  Oxyacids: contain a polyatomic ion If ion ends in –ate, acid name ends in –ic If ion ends in –ite, acid name ends in –ous Examples: H3PO4 (contains ) = H2SO3 (contains ) = hydrobromic acid “I ate something icky, all nite I was nauseous” phosphate phosphoric acid sulfite sulfurous acid NO “hydro” in the name!!

Base Nomenclature (Naming) element + hydroxide Example: Ca(OH)2 = calcium hydroxide

Neutralization Reactions acid + base → water + salt Acid and Base completely ionize. Ex: HCl + NaOH → H+1 + Cl-1 + Na+1 + OH-1 Hydrogen and hydroxide ions combine to form water (H+1 + OH-1 → H2O) The remaining ions and will always be the salt. (Na+1 + Cl-1 → NaCl) HCl + NaOH → H2O + NaCl

Depending on the strengths of the acids and bases in the reaction, different types of salts can be made: Strong acid and weak base → water + acidic salt Weak acid and strong base → water + basic salt Strong acid and strong base → water + neutral salt Weak acid and weak base → water + neutral salt