Chemistry Exam 2 (Chapters 13 & 14)

Front 1

A solution forms when...

Back 1

One substance evently disperses through another

Front 2

Which of the intermolecular forces can operate between the solute and solvent particles in a solution?

Back 2

All of them.

Front 3

What is a major factor in the formation of the solution?

Back 3

The relative strength of intermolecular forces

Front 4

Solutions form when the intermolecular forces between the solute-solvent particles are comparable to...

Back 4

To those that exist between the solute particles themselves and the solvent particles themselves

Front 5

What is solvation?

Back 5

The clustering of solvent particles around a solute particle

Front 6

What is hydration?

Back 6

When the solvent in solvation is water

Front 7

Processes in which the energy of the system decreases tend to occur...

Back 7

Spontaneously.

Front 8

Are spontaneous processes generally endothermic or exothermic?

Back 8

Exothermic.

Front 9

What is enthropy?

Back 9

The thermodynamic process that measures disorder in a system

Front 10

Processin which a system increases in randomness tend to be spontaneous if...

Back 10

They occur at a constant temperature

Front 11

What are the two processes that are factors in the solution process?

Back 11

Changes in enthalpy and entropy

Front 12

Formation of solutions is favored by the increase in entropy that accompanies...

Back 12

Mixing!

Front 13

What relative forces will cause a solution to not form?

Back 13

Solute-solute interactions or solvent-solvent interactions are too strong relative to solvent-solute interactions

Front 14

What does it mean for a substance to be saturated?

Back 14

As a solute begins to dissolve in a solvent the chances of the solute particle colliding with the surface of the solute and rejoining (crystalization) increases. When the process of dissolving and rejoining are equal, the solution is said to have come to equilibrium.

Front 15

What is the solubility?

Back 15

The amount of solute needed to form a saturated solution in a given quantity of solvent

Front 16

What does it mean for a solution to be undersaturated?

Back 16

It means there is less solute than needed for the solution to be saturated.

Front 17

what does it mean for a solution to be supersaturated?

Back 17

It means there is more solute than needed for the soltion to be saturated.

Front 18

Stronger attractions between the solute and solvent molecules tend to make what greater?

Back 18

The solubility.

Front 19

Polar liquids tend to dissolve quickly in...

Back 19

Polar solvents

Front 20

Are nonpolar liquids soluble in polar liquids?

Back 20

No.

Front 21

Increasing the number of polar groups a substance contains will do what to the solubility?

Back 21

Enhance it.

Front 22

Do substances with similar molecular forces tend to be soluble in each other?

Back 22

Yes.

Front 23

The solubility of a gas increases in direct proportion to...

Back 23

It's partial pressure above the solution

Front 24

What law describes the relationship between gas and pressure?

Back 24

Henry's Law

Front 25

The solubility of most solid substances in water ________ as teh temperature increases

Back 25

Increases.

Front 26

The solubility of most gas substances in water ________ as the temperature increases

Back 26

Decreases

Front 27

What are the qualitative ways of expressing cncentration?

Back 27

Dilute and Concentrated

Front 28

What are colligative properties?

Back 28

the properties that depend on the quantity of the solution but not the kind/type

Front 29

What are some examples of colligative properties?

Back 29

Melting point, freezing point, vapor pressure, osmotic pressure

Front 30

What is vapor pressure?

Back 30

The pressure exerted by a vapor when it reaches equilibrium with a liquid in a closed container

Front 31

What is a nonvolatile substance?

Back 31

A substance with no notable vapor pressure

Front 32

What is a volatile substance?

Back 32

A substance with a notable vapor pressure

Front 33

what does adding a nonvolatile solute into a solvent do?

Back 33

Lower the vapor pressure.

Front 34

What is Raoult's law?

Back 34

The partial pressure exerted by solven vapor above a solution equals the product of the mole fraction of the solvent in the solution times the vapor pressure of pure solvent

Front 35

What is an ideal solution?

Back 35

One that obeys Raoult's law

Front 36

The boiling point of a solution is ________ than that of a pure liquid.

Back 36

Higher

Front 37

The freezing point of a solution is _______ than that of a pure liquid

Back 37

Lower

Front 38

What is osmosis?

Back 38

The net movement of solvent molecules from the less concentrated solution into the more concentrated solution

Front 39

What is osmotic pressure?

Back 39

The amount of pressure needed to prevent osmosis by a pure solvent

Front 40

What does it mean if two solutions are isotonic?

Back 40

They have the same osmotic pressure

Front 41

What does it mean if a solution is hypotonic?

Back 41

It has a lower osmotic pressure with respect to the more concentrated solution

Front 42

What does it mean if a solution is more hypertonic?

Back 42

It has a higher osmotic pressure with respect to the less concentrated solution

Front 43

What is active transport?

Back 43

A cell moving something from an area of low concentration to an area of high concentration.

Front 44

What is crenation?

Back 44

The shriveling of a cell in hypotonic solution

Front 45

What is hemolysis?

Back 45

The exploding of a (blood) cell in a hypertonic solution

Front 46

What is a colloid?

Back 46

Mixtures containing particles larer than norma solutes but small enough to remain suspended in dispersing medium

Front 47

What is the Tyndall effect?

Back 47

The scattering of light by colloid particles

Front 48

How can you stablize a hydrophobic colloid?

Back 48

Adding ions to their surface via adsorption