Chemistry Final Exam Review: Moles, Solutions, Acids, Bases, and Thermochemistry

Comprehensive vocabulary flashcards covering basic stoichiometry, solution chemistry, pH, acid-base theories, and thermochemistry definitions from the lecture notes.

Molar mass

The mass of one mole of a substance, reported in grams per mole or $g/mol$.

Molar mass of $H_2O$

$18.02\,g/mol$ (calculated as $2 \times 1.01\,g/mol + 1 \times 16.00\,g/mol$).

Percent composition formula

$$\text{Percent composition}\% = \frac{\text{Atom Mass}}{\text{Molar Mass}} \times 100\%$$

Molecular Formula Mass factor ($n$)

The factor used to multiply the subscripts in the Empirical Formula, calculated as $\frac{\text{Molecular Formula Mass}}{\text{Empirical Formula Mass}}$

Mole Ratio

A ratio that comes from the coefficients of a balanced equation used in stoichiometry.

Solute

The substance that dissolves in a solution.

Solvent

The substance in higher quantity that dissolves the solute.

Solution

A mixture of a solute and a solvent.

Factors affecting the solubility of a solid

Temperature, agitation (stirring), surface area, and the type of solute.

pH Scale

A measure of $H^+$ icons (acidity) ranging from 0 to 14, also known as the "power of hydrogen."

pH calculation formula

$$pH = -\log[H^+]$$

Hydronium ion

Identified as $H^+$.

Hydroxide ion

Identified as $OH^-$.

Strong acids and bases

Substances like $HCl$ and $NaOH$ that dissociate completely and can conduct electricity.

Neutralization Reaction

$\text{Strong acid} + \text{Strong Base} \rightarrow \text{Salt} + \text{Water}$, resulting in a neutral $pH = 7$ if mixed in proper mole ratios.

Arrhenius Acid

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

Arrhenius Base

A substance that produces $OH^-$ ions when dissolved in water.

Brønsted-Lowry Acid

A proton ($H^+$) donor.

Brønsted-Lowry Base

A proton ($H^+$) acceptor.

$$q = m \times c \times \Delta T$$

The formula for heat transferred in Joules or Calories, where $m$ is mass, $c$ is specific heat ($J/g \cdot ^\circ C$), and $\Delta T$ is temperature change ($T_f - T_i$).

Endothermic (TTB)

"Takes To Break"; energy is required to break bonds, indicated by a positive change in enthalpy ($+\Delta H$).

Exothermic (FTF)

"Frees To Form"; energy is released when bonds are formed, indicated by a negative change in enthalpy ($-\Delta H$).