Moles, Molarity, & Balancing Equations Practice

Vocabulary and core concept flashcards created from the Moles, Molarity, & Balancing Equations practice transcript.

Moles

A fundamental unit in chemistry used to measure the amount of a substance, as used to calculate mass from $0.250\,mol$ of $NaCl$ or amount in moles from $25\,g$ of $H_2O$.

Molarity ($M$)

A measure of concentration defined as moles of solute per volume of solution, used in calculations such as finding the mass of $HCl$ needed to make $250\,cm^3$ of a $0.850\,M$ solution.

Dilution

The process of reducing the concentration of a solute in solution, such as adding water to $1.00\,dm^3$ of $2.00\,M\,H_2SO_4$ to yield $0.500\,M$, or diluting $50.0\,cm^3$ of $6.00\,M\,NaOH$ to $200.00\,cm^3$.

Significant Figures

The specific digits used to report answers with proper precision on Free Response Questions (FRQS) on the AP Exam.

Copper (II) Sulfate ($CuSO_4$)

An inorganic chemical compound featured in Section 1 practice to calculate the mass contained within $0.750\,mol$.

Sodium Carbonate ($Na_2CO_3$)

A chemical compound used in a Section 2 practice problem where a chemist prepares $2.5\,dm^3$ of a $0.100\,M$ solution.

Iron (III) Oxide ($Fe_2O_3$)

A reactant in the stoichiometry problem $Fe_2O_3 + 3\,CO \rightarrow 2\,Fe + 3\,CO_2$, where $0.750\,mol$ reacts with excess carbon monoxide.

Balancing Equations

The chemical skill of balancing reactant and product stoichiometric coefficients, such as balancing $KCIO_3 \rightarrow KCI + O_2$ or $C_5H_{12} + O_2 \rightarrow CO_2 + H_2O$.