Solutions and Mixtures - AP Chemistry

The suppression of solubility due to a common ion in solution. Shared ion reduces solubility of ionic compound.

Mass percent = 5%. Using $\frac{5g}{100g} \times 100%$.

The substance in which the solute is dissolved. The major component that does the dissolving.

A solution that conducts electricity due to dissociated ions. Ions enable current flow through solution.

The substance dissolved in the solvent. The minor component that gets dissolved.

A solution that conducts electricity due to dissociated ions. Ions enable current flow through solution.

The suppression of solubility due to a common ion in solution. Shared ion reduces solubility of ionic compound.

Mass percent = 5%. Using $\frac{5g}{100g} \times 100%$.

The substance in which the solute is dissolved. The major component that does the dissolving.

Gas solubility decreases as temperature increases. Higher temperature reduces gas-liquid attractions.

Gas solubility increases with increasing pressure. Follows Henry's Law for gas-liquid equilibrium.

The suppression of solubility due to a common ion in solution. Shared ion reduces solubility of ionic compound.

Mass percent = 5%. Using $\frac{5g}{100g} \times 100%$.

The substance in which the solute is dissolved. The major component that does the dissolving.

$\triangle T_b = i \times K_b \times m$. Boiling point rises with solute concentration.

A mixture where dispersed particles do not settle out. Intermediate size between solutions and suspensions.

Smaller particles dissolve faster due to larger surface area. Greater surface contact increases dissolution rate.

Molarity = 0.5 M. Using $M = \frac{2 \text{ mol}}{4 \text{ L}}$.

Mass percent = $\frac{\text{mass of solute}}{\text{mass of solution}} \times 100$. Percentage concentration by mass composition.

Solid solubility generally increases with temperature. More thermal energy overcomes lattice forces.

$\triangle T_f = 3.72$ °C. Using $\triangle T_f = i \times K_f \times m = 2 \times 1.86 \times 1$.

A solution in which no more solute can dissolve at a given temperature. Equilibrium reached between dissolving and crystallizing.

$X$ represents the mole fraction of the solvent. Mole fraction shows proportion of solvent molecules.

A solution that can dissolve more solute at a given temperature. More solute can still be added and dissolved.

Mole fraction = $\frac{\text{moles of component}}{\text{total moles of all components}}$. Dimensionless ratio expressing relative amounts.

A homogeneous mixture of two or more substances. Components are uniformly distributed at molecular level.

$\triangle T_b = 1.024$ °C. Using $\triangle T_b = i \times K_b \times m = 1 \times 0.512 \times 2$.

A solution that contains more solute than it can theoretically hold at a given temperature. Unstable solution beyond normal solubility limit.

Molarity (M) = $\frac{\text{moles of solute}}{\text{liters of solution}}$. Concentration measured as moles per liter of solution.