Chapter 13: solutions

Question 1

Define the components of a solution: solute(s) and a solvent

Answer 1

A solution is a mixture of two or more pure substances. Solvent is the component that has the greatest amount. Solute is the component that has the lesser amount and is dissolved by solvent

Question 2

Define aqueous solution

Answer 2

when a substance is dissolved in water

Question 3

Describe a homogenous solution

Answer 3

a solution or mixture that has uniform composition throughout

Question 4

Define soluble and insoluble

Answer 4

soluble is when something can be dissolved by solvent. Insoluble is when something cannot be dissolved by a solvent.

Question 5

Define miscible and immiscible.

Answer 5

Miscible is when two or more liquids are mixed together. Immiscible is when liquids don’t mix together.

Question 6

Describe how intermolecular forces affect the solubility of a solute in a solvent.

Answer 6

The stronger attraction between solute and solvents, the greater the solubility. Polar solutes dissolves in polar solvents. Non-polar solutes dissolve in non-polar solvents.

Question 7

In terms of the amount of solute present, explain the difference between an unsaturated
solution and a saturated solution.

Answer 7

Unsaturated solutions do not have the max amount of solute. Saturated is the max amount of solute a solution can have based on volume and temperature.

Question 8

In terms of the amount of solute present, explain the difference between a dilute solution
and a concentrated solution.

Answer 8

Dilute solution has little amounts of solute present. Concentrated solution has big amounts of solute present.

Question 9

Define an electrolyte solution. Give an example of an electrolyte solution.

Answer 9

Contains dissolved ions and conduct electricity. An example is salt and water solution.

Question 10

Define a nonelectrolyte solution. Give an example of a nonelectrolyte solution.

Answer 10

Does not contain dissolved ions. A glucose solution is an example of this.

Question 11

Describe what takes place when an ionic compound dissolves in water

Answer 11

water molecules pick off ions to dissolve

Question 12

Tell the general relationship between temperature and solubility of solids in water.

Answer 12

When increasing temp in solids, it increases solubility

Question 13

Explain how temperature and pressure affect the solubility of gases.

Answer 13

Increasing temperature in gases, decrease solubility. Increasing pressure increases solubility

Question 14

Remember the general formula for percent calculations

Answer 14

Part/Whole x 100

Question 15

Solve, using unit conversions when necessary, solution percent concentration questions.
The basic algebraic equation has three variables. If any two of the variables are known,
the third can be calculated.

Answer 15

Solution concentrations to calculate include:
Mass/mass % (% m/m). Mass/volume % (% m/v). Volume/volume % (% v/v) Parts per million (ppm) Parts per billion (ppb)

Question 16

Define molarity

Answer 16

Molarity is a concentration unit and is the number of moles of a solute divided by the number of liters in a solution

Question 17

In terms of chemical reactions, explain the reason measuring solution concentration in
molarity is important

Answer 17

Important for sociometry calculations of reactions in solutions.

Question 18

Define dilution

Answer 18

decreasing concentration of solute in a solution

Question 19

Explain the fact that when a solution is diluted by adding more solvent, the amount (not
the proportion) of solute present does not change.

Question 20

What are the three common colligative properties

Answer 20

freezing point depression, boiling point elevation, and osmotic pressure

Question 21

Tell what solution component influences the colligative properties of a solution.

Answer 21

The solute influences colligative properties

Question 22

Choose one colligative property and give an example of its application

Answer 22

(freezing point depression): antifreeze solutions are designed to have lower freezing points, allowing car engines to function in subfreezing conditions