Chapter 19 Acids and Bases Lecture Notes

Comprehensive vocabulary flashcards covering the properties, theories, and calculations related to acids and bases from Chapter 19.

Acid

A compound that produces $H^+$ ions when dissolved in water.

Vinegar

A common household substance that contains acetic acid.

Tea

A common beverage that contains tannic acid.

Lemon juice

A common food item that contains citric acid.

Ant venom

A biological substance that contains formic acid.

Electrolytes

Substances that, in aqueous solution, can conduct electricity; both acids and bases fall into this category.

Strong acids

Acids that completely ionize in water, such as binary acids $HCl$, $HBr$, and $HI$, or ternary acids where the number of $O$ atoms minus $H$ atoms is $\geq 2$.

Weak acids

Acids that ionize only slightly in aqueous solution; includes binary acids not listed as strong and ternary acids where the number of $O$ atoms minus $H$ atoms is $\leq 1$.

Base

A compound that produces $OH^-$ (hydroxide) ions when dissolved in water.

Milk of Magnesia

A substance used to neutralize stomach acid that contains magnesium hydroxide.

Drain cleaner

A strong household base that contains sodium hydroxide.

Strong bases

Bases that completely ionize in water, including all hydroxides formed with Group 1 and Group 2 metals, except for $Be$.

Arrhenius Acid

A substance that contains hydrogen and ionizes in water to produce $H_3O^+$.

Arrhenius Base

A substance that contains a $OH$ group and dissociates in water to produce $OH^-$.

Bronsted-Lowry Acid

Any substance that can donate a $H^+$ ion.

Bronsted-Lowry Base

Any substance that can accept a $H^+$ ion.

Conjugate acid

The particle formed when a base accepts a $H^+$ from an acid.

Conjugate base

The particle that remains after an acid gives up a $H^+$.

Conjugate acid-base pair

Two substances related to each other by the accepting or donating of a single $H^+$.

Monoprotic

An acid that can donate exactly one $H^+$ ion, such as $HNO_3$.

Diprotic

An acid that can donate two $H^+$ ions, such as $H_2SO_4$.

Triprotic

An acid that can donate three $H^+$ ions, such as $H_3PO_3$.

Amphoteric

A substance that can act as both a Bronsted-Lowry acid and a Bronsted-Lowry base, such as water.

Ion Product Constant for Water ($K_w$)

The product of the concentrations of hydrogen and hydroxide ions in water, which equals $1 \times 10^{-14}$ ($[H^+] \times [OH^-] = 1 \times 10^{-14}$).

pH

The negative logarithm of the hydrogen ion concentration, calculated as $pH = -\log([H^+])$; the scale ranges from $0$ to $14$.

pOH

The negative logarithm of the hydroxide ion concentration, calculated as $pOH = -\log([OH^-])$; it is related to pH by the formula $pH + pOH = 14$.

Buffer

A solution that resists changes in $pH$ when limited amounts of acids or bases are added.

Buffer Capacity

The amount of acid or base a buffer can neutralize before the $pH$ begins to change significantly.

Neutralization reaction

A double replacement reaction between an acid and a base that produces a salt and water ($H_2O$).

Salt

A compound composed of a metal and a nonmetal that is produced during a neutralization reaction.

Titration

A process in which an acid-base neutralization reaction is used to determine the concentration of a solution.