Unit 13 cem acid equlib

Practice flashcards covering acid-base definitions, naming conventions, pH/pOH calculations, buffers, and titration procedures.

Binary Acids

Acids with the formula $HX$ (where $X$ is another element) named using the format hydro____ic acid, such as hydrofluoric acid ($HF$).

Oxyacids

Acids with the formula $HXOY$ (where $XOY$ is a polyatomic ion); if the ion ends in "-ite" it becomes a "____ous acid" and if it ends in "-ate" it becomes an "____ic acid".

Properties of Acids

Substances that taste sour, are corrosive (irritating to skin), react with many metals in single replacement reactions, have a pH < 7, and act as electrolytes.

Properties of Bases

Substances that taste bitter, are caustic (irritating to skin), feel slippery to the touch, have a pH > 7, and act as electrolytes.

Arrhenius Theory (Acids/Bases)

Defines acids as substances starting with $H$ that produce $H^+$ ions in water and bases as substances ending in $OH$ that produce $OH^-$ ions in water.

Neutralization Reaction

A reaction where an Arrhenius acid and base react to form water ($H_2O$) and a salt.

Brønsted-Lowry Theory (Acids/Bases)

Defines acids as proton ($H^+$) donors that form hydronium ions ($H_3O^+$) and bases as proton acceptors that form hydroxide ions ($OH^-$) in water.

Conjugate Acid-Base Pairs

Two substances that differ only by one proton ($H^+$); the product formed after an acid donates a proton is the conjugate base, and the product formed after a base accepts a proton is the conjugate acid.

Buffer

A solution consisting of a weak acid and its conjugate base (or a weak base and its conjugate acid) that resists changes in $pH$ when $H_3O^+$ or $OH^-$ is added.

Self-Ionization of Water

The equilibrium reaction $H_2O(l) + H_2O(l) ightleftharpoons H_3O^+(aq) + OH^-(aq)$, where at $25^{ ext{o}}C$, $K_w = [H_3O^+][OH^-] = 1 imes 10^{-14}$.

pH

A measure of acidity calculated as $pH = - ext{log}_{10}[H_3O^+]$; every change of 1 in $pH$ represents a 10x change in concentration.

pOH

An alkalinity scale opposite to $pH$, calculated as $pOH = - ext{log}_{10}[OH^-]$, where $pH + pOH = 14$.

Strong Acids

Acids that completely dissociate or donate $H^+$; specifically the "Big 6": $HCl$, $HBr$, $HI$, $HNO_3$, $HClO_4$, and $H_2SO_4$.

Acid Dissociation Constant ($K_a$)

The equilibrium constant for a weak acid dissociation; a larger $K_a$ indicates a stronger acid that dissociates more.

Strong Bases

Bases that completely dissociate into $OH^-$ in water, including Arrhenius bases like $NaOH$, $LiOH$, $KOH$, and $Ba(OH)_2$.

Base Dissociation Constant ($K_b$)

The equilibrium constant for a weak base dissociation; a larger $K_b$ indicates a stronger base.

Equivalence Point

The point in a titration where the moles of acid ($H^+$) are stoichiometrically equal to the moles of base ($OH^-$).

End Point

The point in a titration where the chemical indicator changes color, signaling the titration is complete; in a good titration, this is approximately the equivalence point.

Indicator

A chemical that changes color based on the $pH$ of the solution, such as phenolphthalein which turns pink in basic conditions.

Burette Reading

A measurement procedure where volume is recorded to the $0.01 ext{,mL}$ place (estimating one digit beyond the $0.1 ext{,mL}$ marks) and the volume used is calculated as $ext{Final Volume} - ext{Initial Volume}$.