Acids and Bases Lecture Notes

Comprehensive vocabulary flashcards covering the definitions, chemical properties, and reactions of acids, bases, and salts as presented in the lecture notes.

Acid (General Definition)

A substance with a pH lower than 7 that acts as a source of protons ($H^+$) and turns litmus red.

Alkali

A soluble base that dissolves in water to produce a solution with a pH higher than 7, turns litmus blue, and contains an excess of $OH^-$ ions.

pH Scale

A spectrum ranging from 0 to 14 used to determine acidity ($pH < 7$), neutrality ($pH = 7$), or alkalinity ($pH > 7$).

Mineral Acids

Inorganic acids including hydrochloric acid ($HCl$), nitric acid ($HNO_3$), sulfuric acid ($H_2SO_4$), carbonic acid ($H_2CO_3$), and phosphoric acid ($H_3PO_4$).

Organic Acids

Acids containing carbon, such as formic acid ($HCOOH$, methanoic acid), acetic acid ($CH_3COOH$, ethanoic acid), lactic acid, and citric acid.

pH Calculation

The negative logarithm (base 10) of the hydrogen ion concentration, defined as $pH = -\text{log}_{10}[H^+]$.

Strong Acid

An acid that 100% dissociates into ions in solution through an irreversible process, resulting in a very low pH (e.g., $HCl$).

Weak Acid

An acid that only partially dissociates into ions in solution through a reversible process, typically having a pH around 3.0 (e.g., $CH_3COOH$).

Strong Base

A base that 100% dissociates into ions in solution, such as sodium hydroxide ($NaOH$), resulting in a high pH of approximately 14.0.

Weak Base

A base that only partly dissociates into ions through a reversible process, such as ammonia ($NH_3$), typically having a pH around 12.0.

Neutralization Reaction

A reaction where an acid reacts with a base to produce a salt and water ($\text{ACID} + \text{BASE} \rightarrow \text{SALT} + H_2O$).

Amphoteric Oxide

Metal oxides that can act as both bases and acids, specifically oxides of Zinc ($Zn$) and Aluminum ($Al$).

Basic Oxide

Oxides formed by metals (e.g., $Na$, $Mg$, $Ca$, $Fe$, $Cu$) that react with water to produce bases/alkalis.

Acidic Oxide

Oxides formed by non-metals (e.g., $P$, $S$, $C$) that react with water to produce acids.

Neutral Oxide

An oxide that has a pH of 7.0, such as water ($H_2O$).

Titration

The chemical process of determining the concentration of a substance in a liquid by measuring the volume of another substance needed to react with it.

Methyl Orange

A pH indicator that is red in acidic solutions and yellow in alkaline solutions.

Thymolphthalein

A pH indicator that is colorless in acidic solutions and blue in alkaline solutions.

Spectator Ions

Ions that appear on both sides of a chemical equation and do not participate in the reaction, such as $Na^+$ and $Cl^-$ in the reaction between $NaOH$ and $HCl$.

Quicklime

The common name for the chemical compound calcium oxide ($CaO$).

Slaked Lime / Limewater

The common name for the chemical compound calcium hydroxide ($Ca(OH)_2$).

Limestone

The common name for the chemical compound calcium carbonate ($CaCO_3$).

Hydrogen Gas Test

A test where a burning splint is used; if the gas is present, it causes a squeaky "pop" sound.

Oxygen Gas Test

A test where a glowing splint is used; the splint will relight if the gas is present.

Antacid Reaction

The neutralization of stomach acid ($HCl$) using compounds like $CaCO_3$, $Mg(OH)_2$, or $Al(OH)_3$.

Precipitate Color: Iron (II) Hydroxide

A green solid produced when $Fe(II)$ reacts with sodium hydroxide ($NaOH$).

Precipitate Color: Iron (III) Hydroxide

A reddish-orange solid produced when $Fe(III)$ reacts with sodium hydroxide ($NaOH$).

Precipitate Color: Copper (II) Hydroxide

A blue solid produced when $Cu(II)$ reacts with sodium hydroxide ($NaOH$).

Precipitate Color: Zinc (II) Hydroxide

A white solid produced when $Zn(II)$ reacts with sodium hydroxide ($NaOH$).