Solutions

Question 1

Solution

Answer 1

Homogenous mixture. Solvent particles surround solute particles via electrostatic interactions.

Question 2

Solvation or Dissolution

Answer 2

The process of dissolving a solute in solvent. Most dissolutions are endothermic, although dissolution of gas into liquid is exothermic.

Question 3

Solubility

Answer 3

Maximum amount of solute that can be dissolved in a solvent at a given temp.

Question 4

Molar Solubility

Answer 4

Molarity of the solute at saturation.

Question 5

Complex Ions

Answer 5

Cation bonded to at least one ligand which is the electron pair donor. It is held together with coordinate covalent bonds. Formation of complex ions increases solubility.

Question 6

Solubility in Water

Answer 6

Polar molecules are attracted to water molecules and are hydrophilic. Nonpolar molecules are repelled by water and are hydrophobic.

Question 7

Soluble Elements

Answer 7

Na+, K+, NH4+, NO3-, SO42-, Cl-, Br, I-

Question 8

Insoluble Elements

Answer 8

S2-, O2-, OH-, CrO42-, PO43-, and CO32-

Question 9

Concentration % by mass

Answer 9

mass solute / mass solution x 100%

Question 10

Mole Fraction

Answer 10

XA = moles solute/total moles

Question 11

Molarity

Answer 11

M = moles solute / liters of solution

Question 12

Molality

Answer 12

Cm = moles solute / kg of solvent

Question 13

Normality

Answer 13

N = # of equivalents / liters of solution

Question 14

Dilutions

Answer 14

M1V1 = M2V2

Question 15

Solutions Equilibria

Answer 15

Saturated solutions are in equilibrium at that particular temperature.

Question 16

Colligative Properties

Answer 16

Physical properties of solutions that depend on the concentration of dissolved particles but not on their chemical identity.

Question 17

Raoult’s Law

Answer 17

Vapor pressure depression. The presence of other solutes decreases evaporation rate of solvent, thus decreasing Pvap.
PA = XAPA

Question 18

Boiling Point Elevation

Answer 18

Delta Tb = i Kb Cm
i = ionization factor
Kb = boiling point depression constant
Cm = molal concentration

Question 19

Freezing Point Depression

Answer 19

Delta Tf = i KfCm

Kf = freezing point depression constant

Question 20

Osmolarity

Answer 20

The number of individual particles in solution. Ex. NaCl dissociates completely in water, so 1 M NaCl = 2 osmol/liter

Question 21

Osmotic Pressure

Answer 21

"Sucking" pressure generated by solutions in which water is drawn into solution. 
pi = i MRT
i = van't Hoff factor
M = molar concentration of solute
R = gas constant
T = temp.

Question 22

Solubility Product Constant

Answer 22

Equilibrium expression for something that dissolves. For substance AaBb, Ksp = [A]^a[B]^b

Question 23

Ion Product

Answer 23

IP = [A]^a[B]^b

Question 24

IP < Ksp

Answer 24

unsaturated

Question 25

IP = Ksp

Answer 25

saturated at equilibrium

Question 26

IP > Ksp

Answer 26

supersaturated, precipitate

Question 27

Formation or Stability Constant

Answer 27

Kf. The equilibrium constant for complex formation. Usually much greater than Ksp.

Question 28

Common Ion Effect

Answer 28

Lower solubility of a compound in a solution that already contains one of the ions in the compound. The presence of that ion shifts the dissolution reaction to the left, decreasing its dissociation.

Question 29

Chelation

Answer 29

When a central cation is bonded to the same ligand in multiple places. Chelation therapy sequesters toxic metals.