Acids, Bases, and Salts

Arrhenius Theory

Everything happens in water.

Acid (Arrhenius)

Increases $H^+$ concentration.

Base (Arrhenius)

Increases $OH^-$ concentration.

Brønsted-Lowry Theory

Focuses on proton ($H^+$) movement.

Acid (Brønsted-Lowry)

Proton donor.

Base (Brønsted-Lowry)

Proton acceptor.

Lewis Theory

Focuses on electron pairs.

Acid (Lewis)

Electron pair acceptor.

Base (Lewis)

Electron pair donor.

Self-Ionization of Water

Water breaks into $H^+$ and $OH^-$.

Constant ($K_w$)

$[H^+][OH^-] = 1.0 imes 10^{-14}$.

pH Calculation

$ ext{pH} = - ext{log}[H^+]$.

pOH Calculation

$ ext{pOH} = - ext{log}[OH^-]$.

Relationship of pH and pOH

$ ext{pH} + ext{pOH} = 14$.

Acidic Solution

$ ext{pH} < 7$ ($[H^+] > 10^{-7} ext{ M}$).

Neutral Solution

$ ext{pH} = 7$.

Basic Solution

$ ext{pH} > 7$ ($[H^+] < 10^{-7} ext{ M}$).

Neutralization Reaction

$ ext{Acid} + ext{Base}

ightarrow ext{Salt} + ext{Water}$.

Salt Hydrolysis (Acidic Solutions)

Positive ions release protons to water.

Salt Hydrolysis (Basic Solutions)

Negative ions attract protons from water.

Buffers

A solution containing a weak acid/base and its salt that resists pH changes.

Amphoteric Substance

Substance that can act as both an acid and a base (like $H_2O$).

Conjugate Acid/Base

Substances that differ by exactly one $H^+$.

Monoprotic Acid

Acid with 1 ionizable hydrogen.

Diprotic Acid

Acid with 2 ionizable hydrogens.

Triprotic Acid

Acid with 3 ionizable hydrogens.

Titration

Finding the concentration of an unknown by neutralizing it.

Indicators

Weak acids/bases that show different colors depending on the pH.

Taste of Acids

Sour.

Taste of Bases

Bitter.

Feel of Acids

Stinging.

Feel of Bases

Slippery.

Litmus Test (Acids)

Red.

Litmus Test (Bases)

Blue.

Ion Produced in Water (Acid)

$H^+$.

Ion Produced in Water (Base)

$OH^-.$

Electrolytes (Acids)

Yes.

Electrolytes (Bases)

Yes.