Pharmaceutical Inorganic Chemistry: Solutions and Gas Laws

Vocabulary flashcards covering pharmaceutical inorganic chemistry notes on solutions, solubility terms, concentration units, and gas laws.

Solute

The substance that is dissolved in a solution.

Solvent

The dissolving medium in a solution.

Solution Components Diagram

Visual diagram illustrating the solute being added into the liquid solvent inside a container.

Solubility

The amount of solute that dissolves in a given amount of solvent to produce a saturated solution.

Very soluble

Descriptive solubility term indicating that less than 1 part of solvent is required per part of solute.

Freely soluble

Descriptive solubility term indicating that 1 to 10 parts of solvent are required per part of solute.

Soluble

Descriptive solubility term indicating that 10 to 30 parts of solvent are required per part of solute.

Sparingly soluble

Descriptive solubility term indicating that 30 to 100 parts of solvent are required per part of solute.

Slightly soluble

Descriptive solubility term indicating that 100 to 1000 parts of solvent are required per part of solute.

Very slightly soluble

Descriptive solubility term indicating that 1000 to 10,000 parts of solvent are required per part of solute.

Practically insoluble

Descriptive solubility term indicating that 10,000 parts and over of solvent are required per part of solute.

Gas-Gas Solution

A solution where both the solute and solvent are gases, such as air.

Liquid-Gas Solution

A solution where a liquid solute is dissolved in a gas solvent, such as water in oxygen.

Solid-Gas Solution

A solution where a solid solute is dissolved in a gas solvent, such as iodine vapor in air.

Gas-Liquid Solution

A solution where a gas solute is dissolved in a liquid solvent, such as carbonated water.

Liquid-Liquid Solution

A solution where a liquid solute is dissolved in a liquid solvent, such as alcohol in water.

Solid-Liquid Solution

A solution where a solid solute is dissolved in a liquid solvent, such as aqueous sodium chloride solution.

Gas-Solid Solution

A solution where a gas solute is dissolved in a solid solvent, such as hydrogen in palladium.

Liquid-Solid Solution

A solution where a liquid solute is dissolved in a solid solvent, such as mineral oil in paraffin.

Solid-Solid Solution

A solution where both solute and solvent are solids, such as a gold-silver mixture or mixture of alums.

Saturated solution

A solution that contains the maximum amount of solute that a solvent can dissolve.

Unsaturated solution

A solution that contains less amount of solute than the solvent can dissolve.

Supersaturated solution

A solution that contains more amount of solute than the solvent can dissolve.

Saturation Classification Diagram

Visual demonstration comparing unsaturated, saturated, and supersaturated solutions in test tubes.

Miscible

Property of liquid solutions where all components dissolve in each other in all proportions.

Immiscible

Property of liquid solutions where components are completely insoluble in one another regardless of proportions.

Isotonic

Condition when two solutions have the same amount of solute concentrations.

Hypotonic solution

A solution that has a lower solute concentration than that of another solution.

Hypertonic solution

A solution that contains a higher solute concentration than that of another solution.

Concentration

The amount of solute dissolved in a given amount of solution.

Concentrated solution

A solution that contains a large amount of solute in relation to the solvent in the solution.

Diluted solution

A solution that contains a small amount of solute in relation to the solvent in the solution.

Weight/Volume Percent (% W/V)

Concentration expressed as $\%\,\text{W/V} = \left(\frac{\text{grams solute}}{\text{milliliters solution}}\right) \times 100$.

Weight/Weight Percent (% W/W)

Concentration expressed as $(\text{W/W}\%) = \left(\frac{\text{grams solute}}{\text{grams solvent}}\right) \times 100$.

Molarity (M)

The number of moles of solute per liter of solution, calculated as $M = \frac{\text{moles of solute}}{\text{Liter solution}}$.

Molality (m)

The number of moles of solute per kilogram of solvent, calculated as $m = \frac{\text{moles of solute}}{\text{kilogram solvent}}$.

Normality (N)

The gram-equivalent weight of solute per liter of solution, calculated as $N = M \times \text{valency}$.

Pressure (P)

The force exerted by a gas per unit area.

Temperature (T)

The measure of the average kinetic energy of gas particles.

Standard Pressure

Gas pressure baseline defined as $1\,\text{atm} = 760\,\text{mmHg}$.

Standard Temperature

Gas temperature baseline defined as $273\,\text{K} = 0\,^\circ\text{C} = 32\,^\circ\text{F}$.

Molar Volume of Gas at STP

The volume occupied by $1\,\text{mol}$ of gas at standard conditions, equal to $22.4\,\text{L}$.

Avogadro's Number

The number of particles in $1\,\text{mol}$ of gas, equal to $6.02 \times 10^{23}\,\text{particles}$.

Boyle's Law

Gas law stating that pressure and volume are inversely proportional at constant temperature and amount of gas ($P_1V_1 = P_2V_2$).

Charles' Law

Gas law stating that Kelvin temperature and volume are directly proportional at constant pressure and amount of gas ($\frac{V_1}{T_1} = \frac{V_2}{T_2}$).

Gay-Lussac's Law

Gas law stating that pressure is directly proportional to Kelvin temperature at constant volume and amount of gas ($\frac{P_1}{T_1} = \frac{P_2}{T_2}$).

Combined Gas Law

Gas law used to solve for changes in pressure, volume, and temperature ($\frac{P_1V_1}{T_1} = \frac{P_2V_2}{T_2}$).

Standard Temperature & Pressure (STP)

Standard baseline conditions defined as $0\,^\circ\text{C}$ ($273\,\text{K}$) and $1\,\text{atm}$ ($101.325\,\text{kPa}$).

Avogadro's Law

Gas law stating that gas volume is directly related to the number of moles at constant temperature and pressure ($\frac{V_1}{n_1} = \frac{V_2}{n_2}$).

Ideal Gas Law

Gas law combining Boyle's, Charles', and Avogadro's laws into $PV = nRT$.