ACIDS AND BASES Chapters 15 and 16

Acids H (Hydronium – H3O+) pH less than 7 Sour taste Corrosive Conduct electric current Ionization Bases OH (Hydroxide) pH greater than 7 (alkaline) Bitter taste/slippery Corrosive Conduct electric current Dissociation

COMMON ACIDS Acetic acid – vinegar Juices/citrus fruit Sulfuric acid – car batteries Nitric acid - fertilizer/explosive Hydrochloric acid - Stomach - pool cleaner (muriatic acid) COMMON BASES Ammonia – NH3 KOH – soap NaOH – drain opener Antacids

Indicators Acid Base Litmus paper red blue Phenolphthalein (phth) clear bright pink Bromothymol blue yellow blue Universal indicator red-yellow blue-purple

Neutralization Reactions A reaction between an acid and a base Produces water and a salt.

Arrhenius acid – Increases concentration of Hydrogen (H+) or Hydronium ions (H3O+). Arrhenius base – Increases concentration of Hydroxide ions (OH-).

HCl + NH3 → NH4+ + Cl- Bronsted-Lowry acid – Proton donor Bronsted-Lowry base – Proton acceptor HCl + NH3 → NH4+ + Cl-

STRENGTH VS. How completely it ionizes or dissociates STRENGTH VS. How completely it ionizes or dissociates. (will not change) Acids – ionize Bases - dissociate CONCENTRATION Measurement of how much acid or base is in a solution. (can be changed)

pH is the potential of hydrogen – measures concentration of H+ in a solution [H+] Changes by a multiple of 10 pH scale of 0-14 – Logarithms are used to simplify scale Examples 10 versus 9 1 versus 3 6 versus 3

Acids **Balance charges **Do not name “Hydrogen” Hydro _____________ic __________________ic __________________ous “ide” like Cl “ate” like ClO3 “ite” like ClO2