Types of Solutions

Comprehensive practice flashcards covering the definition, components, and classifications of solutions based on solvent phase, saturation, and concentration.

What is the general scientific definition of a solution?

A homogeneous mixture of two or more pure substances that appears as one phase.

What fundamental relationship between components in solution formation is depicted in the diagram?

$$\text{Solvent} + \text{Solute} = \text{Solution}$$

What two essential components make up any solution?

A solute and a solvent.

In a solution, what is the solute?

The pure substance present in a lesser amount that is dissolved in the solvent.

In a solution, what is the solvent?

The more abundant substance in which the solute particles are dissolved.

What are the three main criteria used to classify solutions?

The phases of its components (or phase of the solvent), saturation, and concentration.

What defines a liquid solution?

A solution where the solvent is a liquid.

Which type of solution is identified as the most common based on solvent phase?

Liquid solutions.

What naturally occurring body of water is cited in the notes as an example of a liquid solution?

Seawater.

What are the three possible combinations of solute and solvent phases for liquid solutions?

Solid-liquid, liquid-liquid, and gas-liquid solutions.

What solute and solvent make up the solid-liquid solution brine?

Solid salt (solute) dissolved in liquid water (solvent).

What solute and solvent make up rubbing alcohol?

Liquid ethanol (solute) dissolved in liquid water (solvent).

What type of solution is a carbonated drink based on solute and solvent phases?

A gas-liquid solution (gas solute dissolved in a liquid solvent).

What defines a solid solution?

A solution where the solvent is a solid.

What three combinations of solute and solvent phases form solid solutions?

Solid-solid, liquid-solid, and gas-solid solutions.

What type of solid solution is brass, and what are its components?

A solid-solid solution consisting of zinc (solute) dissolved in copper (solvent).

What type of solid solution is amalgam, and what are its components?

A liquid-solid solution consisting of liquid mercury (solute) dissolved in solid gold (solvent).

What example of a gas-solid solution is given in the lecture?

Hydrogen gas ($H_2$) trapped in palladium metal.

What defines a gaseous solution?

A solution where the solvent is a gas.

What three combinations of solute and solvent phases constitute gaseous solutions?

Solid-gas, liquid-gas, and gas-gas solutions.

What example of a solid-gas solution is cited in the lecture?

Camphor in nitrogen gas.

What example of a liquid-gas solution is cited in the lecture?

Water vapor in the air.

What common example is cited for a gas-gas solution?

Air.

What does classifying solutions based on saturation describe?

Classifying solutions based on the amount of solute dissolved in a given amount of solvent at a specific temperature.

What specific factor must be considered when classifying a solution based on saturation?

Solubility at a specific temperature.

What is an unsaturated solution?

A solution in which the amount of solute is less than the solute's solubility (or solubility capacity of the solvent) at a given volume and temperature.

What specific combination is illustrated as an unsaturated solution in this figure?

$30.0\,\text{g}\text{ NaCl}$ completely dissolved in $100\,\text{ml}\text{ H}_2\text{O}$.

What is a saturated solution?

A solution in which the amount of solute is equal to the solute's solubility (or solubility capacity of the solvent) at a given volume and temperature.

What occurs when $40.0\,\text{g}\text{ NaCl}$ is added to $100\,\text{ml}\text{ H}_2\text{O}$, as illustrated in this figure?

A saturated solution forms containing $36.0\,\text{g}\text{ NaCl}$, and the additional $4.0\,\text{g}\text{ NaCl}$ remains undissolved at the bottom.

What is the maximum solubility limit of $\text{NaCl}$ in $100\,\text{ml}\text{ H}_2\text{O}$ indicated by the lecture diagrams?

$36.0\,\text{g}\text{ NaCl}$.

What is a supersaturated solution?

A solution in which the amount of solute is greater than the solute's solubility (or solubility capacity of the solvent) at a given volume and temperature.

How is a supersaturated solution prepared?

By dissolving a solute at a higher temperature and subsequently cooling the solution down.

Why is a supersaturated solution considered unstable?

Because agitation or the addition of a seed crystal causes the excess solute to crystallize out.

In the crystallization process shown in this figure, what initiates precipitate formation from the supersaturated solution?

Adding a seed crystal or applying mechanical agitation.

What is a concentrated solution?

A solution that contains an excessively large amount of solute.

What is the most common unit of concentration used when discussing concentrated solutions?

Molarity ($M$).

What molarity threshold generally characterizes a concentrated solution?

Molarities greater than $1\,M$ ($> 1\,M$).

How are concentrated solutions typically utilized in laboratory preparation?

They are used as stock solutions in preparing diluted solutions.

What is the molarity of concentrated sulfuric acid as specified in the lecture?

$18\,M$.

What is the molarity of glacial (concentrated) acetic acid as specified in the lecture?

$17\,M$.

What characteristic physical phenomenon is displayed by highly concentrated solutions, as pictured here?

Highly concentrated solutions emit visible fumes.

What is a diluted solution?

A solution of low concentration that contains a lower amount of solute relative to the stock solution.

What are the two steps in preparing a diluted solution from a stock solution?

1. Taking an aliquot (a portion of the stock solution), and 2. Adding more solvent to lower the concentration.

What is an aliquot in the context of solution preparation?

A measured portion taken from the stock solution.

How does the concentration of an aliquot compare to the concentration of the stock solution from which it was drawn?

An aliquot has the exact same concentration as the stock solution.

True or False: A carbonated drink is an example of a liquid-liquid solution.

False (it is a gas-liquid solution).

True or False: Amalgam is a solution of liquid mercury in gold.

True.

How is air classified based on the phase of the solvent?

Gaseous solution.

How is a $0.5\,M$ potassium permanganate ($\text{KMnO}_4$) solution classified based on concentration?

Diluted solution (because its molarity is less than $1\,M$).

Why does the number of moles of solute remain the same upon dilution even though the concentration decreases?

Because dilution only involves adding more solvent; no solute particles are added or removed from the aliquot.