Chapter 13 - Solutions

Question 0

Ion-dipole

Answer 0

Must be strong enough to compete with ionic and hydrogen/d-d/LDF forces

Question 1

Solution

Answer 1

Homogenous mixtures of two or more pure substances

Question 2

How does a solution form

Answer 2

Solvent pulls solute particles apart and surrounds them

Question 3

Three processes that affect energetics of solution

Answer 3

Separation of solute particles
Separation of solvent particles
New interactions between solvent and solute

Question 4

Heat is absorbed in dissolution of NH4NO3 in water because

Answer 4

Increasing entropy leafs to lower energy of system

Question 5

Saturated solution

Answer 5

Solvent holds as much solvent as possible. Dissolves solute is in dynamic equilibrium with solid solute particles

Question 6

Unsaturated solution

Answer 6

Less solute than can dissolve in the solvent is dissolved

Question 7

Supersaturated solution

Answer 7

Solvent holds more solute than normally possible (unstable)

Question 8

Factors that affect solubility

Answer 8

Polar dissolves polar

Forces soluble by like forces

Question 9

Gases in solution

Answer 9

Solubility of gas in water increases with mass
Larger molecules have stronger dispersion forces
Solubility of gas in liquid is directly proportional to its pressure

Question 10

Henry’s law

Answer 10

Sg=kPa

Question 11

Temperature

Answer 11

Solubility of solid solutes in liquid solvent increase with temperature.

Opposite for gas

Question 12

Five ways of expressing concentration

Answer 12

Mass percentage
Parts per million
Mole fraction
Molarity
Molality

Question 13

Colligative properties

Answer 13

Changes depend only on number of solute particles present

Ex: vapor pressure, boiling pt elevation, freezing pt depression, and osmotic pressure

Question 14

Vapor pressure

Answer 14

Vapor pressure of a solution is lower than that of pure solvent b/c of solute solvent intermolecular attraction

Question 15

Boiling pt and freezing pt

Answer 15

Nonvolatile solute solvent interactions also cause solutions to have higher boiling pts and lower freezing pts than the pure solvent

Question 16

Colligative properties of electrolytes

Answer 16

Depen on number of particles dissolved

Show greater changes than those of non electrolytes

Question 17

Osmosis

Answer 17

Semipermeable membranes

Question 18

Hypertonic

Answer 18

Concentration outside cell is greater
Flow of water out of the cell
Crenation results

Question 19

Hypotonic

Answer 19

Concentration outside cell is less
Water flows into cell
Hemolysis results

Question 20

Isotonic

Answer 20

Same concentration on both sides of membrane

Question 21

Colloids

Answer 21

Suspension of particles larger than individual ions or molecules but too small to be settles by gravity

Question 22

Tyndall effect

Answer 22

Colloid suspensions can scatter light

Ex: milk can look blue

Question 23

Colloids in biological system

Answer 23

Polar/hydrophilic end
Non polar/hydrophobic end
Protein folding if bad can result in cystic fibrosis
Can aid in emulsification of fats and oils in aqueous solutions

Question 24

If Ionic salt is soluble in water

Answer 24

It’s because the ion-dipole interactions are strong enough to overcome the lattice energy of salt crystal

Question 25

Why do endothermic processes occur

Answer 25

Enthalpy may increase but the total energy of the system can still decrease if the system becomes more disordered

Question 26

Glucose

Answer 26

Very soluble in water

Question 27

Cyclohexane

Answer 27

Not soluble in water

Dispersion forces

Question 28

Vitamin A

Answer 28

Soluble in non polar compounds (like fats)

Question 29

Vitamin C

Answer 29

Soluble in water

Question 30

Vant hoff factor

Answer 30

Delta T = Kf * m * i