Introduction to Acids and Bases - (Chemistry)

Arrhenius theory (acid)

produces H+ ions in aqueous solution

Arrhenius theory (base)

produces OH- ions in aqueous solutions

Bronsted-Lowry (acid)

proton donor

Bronsted-Lowry (base)

proton acceptor

Lewis theory (acid)

electron-pair acceptor

Lewis theory (base)

electron-pair donor

Amphoteric substances

(like water) can act as both acids and bases depending on the reaction

Acids

Bases

substances that have a bitter taste, feel slippery, and also conduct electricity when in aqueous solution

Strong acids

ionize completely in aqueous solutions, like HCl, HNO, and H_2SO_4

in these acids, the bonds to hydrogen are weak enough to break easily in water

Weak acids

Ionize only partially in water, like CH_3COOH and most molecules remain in-ionized in solution

Strong bases

dissociate completely in water to produce OH- ions

ex: NaOh and KOH

Weak bases

dissociate partially in water

ex: NH_3 which reacts with water to produce NH_4 and OH- but not completely

strength (ionization ability) doesn’t equal

concentration (amount dissolved)

Acid solutions

pH < 7

Neutral solution

pH = 7

Basic solution

pH > 7

pH =

-log[H+]

pOH =

-log[OH-]

At 25 degrees:

pH + pOH = 14

Indicators

substances that change color with pH (litmus, phenolphthalein, methyl orange)

pH meters

electronic instruments that give a direct digital pH reading with high precision

Neutralization reaction

occurs when an acid reacts with a base to form salt and water

General form of neutralization reaction

Acid + Base → Salt + Water

Example of neutralization reaction

HCl + NaOH → NaCl + H2O