Stoichiometry and Solution Concentration

These flashcards cover the fundamental concepts of stoichiometry, units of solution concentration including molarity and molality, and the calculation of theoretical and percentage yields based on the provided lecture transcript.

Mole Concept Formula (Mass)

$$\text{No. of Moles} = \frac{\text{Mass (g)}}{\text{molar mass (g/mol)}}$$

Avogadro’s Number

The number of particles contained in $1\text{ mole}$, equal to $6.022 \times 10^{23}$.

Mole Concept Formula (Molarity)

$$\text{No. of Moles} = \text{Molarity (mol/L)} \times \text{volume (L)}$$

Molarity (M)

Molar concentration defined as the number of moles of a solute contained in $1\text{ liter}$ of solution, calculated as $\frac{\text{Amount of solute (Mol)}}{\text{Volume of solution (L)}}$.

Molality (m)

The number of moles of solute per kilogram ($1000\,g$) of solvent, calculated as $\frac{\text{Amount of solute (Mol)}}{\text{Mass of solvent (kg)}}$.

Weight percent (% w/w)

$$\frac{\text{mass of solute (g)}}{\text{weight of solution (g)}} \times 100\%$$

Volume percent (% v/v)

$$\frac{\text{volume of solute (ml)}}{\text{volume of solution (ml)}} \times 100\%$$

Weight to volume percent (% w/v)

$$\frac{\text{mass of solute (g)}}{\text{volume of solution (ml)}} \times 100\%$$

Parts per million (ppm)

The grams of solute per million grams of total solution or mixture, calculated as $\frac{\text{mass of solute}}{\text{mass of sample}} \times 10^6$. Common units include $mg/kg$ or $mg/L$.

Parts per billion (ppb)

The grams of solute per billion grams of total solution or mixture, calculated as $\frac{\text{mass of solute}}{\text{mass of sample}} \times 10^9$. Common units include $\mu g/kg$ or $\mu g/L$.

Stoichiometry

The relationship between the quantities of chemical reactants and products based on the principle of the conservation of matter.

Law of The Conservation of Matter

A principle stated by Lavoisier (1788) that matter can be neither created nor destroyed, meaning a chemical equation must have the same number of atoms of the same kind on both sides.

Theoretical Yield

The calculated maximum quantity of product that can be obtained from a chemical reaction based on the given quantities of reactants.

Actual Yield

The quantity of product that is actually obtained in a laboratory or chemical plant, which is typically less than the theoretical yield.

Percentage (%) Yield

A measure of the efficiency of a reaction calculated as $\frac{\text{actual yield}}{\text{theoretical yield}} \times 100\%$.

Stoichiometric Factor

The mole ratio used to convert moles of reactant to moles of product, derived from the coefficients in a balanced chemical equation.

Limiting Reactant

The reagent that is completely used up in a reaction and limits the quantity of product that can be formed.