General Chemistry Chapter 9: Solutions

Question 1

Solutions

Answer 1

homogeneous mixtures composed of two or more substances. - Combine to form a single phase, generally liquid

Question 2

Solvation/Dissolution

Answer 2

solvent particles surround solute particles via electrostatic interactions

Question 3

Hydration

Answer 3

solvation in water

Question 4

What are most dissolutions - exo or endo - thermic? exception?

Answer 4

Most are endothermic, but gas into liquid = exothermic

Question 5

Solubility

Answer 5

the maximum amount of a solute that can be dissolved in a given solvent at a given temperature; it is often expressed as molar solubility - the molarity of the solute at saturation.

Question 6

Complex ions/coordination compounds

Answer 6

composed of metallic ions bound to various neutral compounds and anions, referred to as ligands.

Question 7

Formation of complex ions increases __

Answer 7

the solubility of otherwise insoluble ions (the opposite of the common ion effect)

Question 8

How do you form a complex ion?

Answer 8

Electron donors and electron pair acceptors, such as those seen in coordinate covalent bonding.

Question 9

Percent concentration by mass

Answer 9

used for aqueous solutions and solid-in-solid solutions.

Question 10

Mole fraction

Answer 10

used for calculating vapor pressure depression and partial pressures of gases in a system

Question 11

Molarity

Answer 11

is the most common unit for concentration and is used for rate laws, the law of mass action, osmotic pressure, pH and pOH and the Nernst equation.

Question 12

Molality

Answer 12

used for boiling point elevation and freezing point depression

Question 13

Normality

Answer 13

molarity of the species of interest and is used for acid-base and oxidation reduction reactions

Question 14

Saturated solutions are:

Answer 14

at equilibrium at a particular temperature

Question 15

Solubility product constant

Answer 15

the equilibrium constant for a dissolution reaction

Question 16

Comparison of the ion product to Ksp determines

Answer 16

The level of saturation and behavior of the solution

Question 17

IP

Answer 17

the solution is unsaturated and if more solute is added, it will dissolve.

Question 18

IP = Ksp

Answer 18

the solution is saturated, and there will be no change in concentrations

Question 19

IP > Ksp

Answer 19

the solution is supersaturated and a precipitate will form

Question 20

What does a complex ion do to solution?

Answer 20

greatly increases solubility of other salts containing the same ions because it uses up the products of those dissolution reactions, shifting the equilibrium to the right (the opposite of the common ion effect)

Question 21

Formation or stability constant

Answer 21

the equilibrium constant for complex formation. Its value is usually much greater than Ksp.

Question 22

The common ion effect

Answer 22

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

Question 23

Colligative properties

Answer 23

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

Question 24

Vapor pressure depression follows

Answer 24

Raoult’s law

Question 25

Vapor pressure depression

Answer 25

the presence of other solutes decreases the evaporation rate of a solvent without affecting its condensation rate, thus decreasing its vapor pressure - Also explains boiling point elevation.

Question 26

Freezing point depressing and boiling point elevation

Answer 26

shifts in the phase equilibria dependent on the molality of the solution.

Question 27

Osmotic pressure

Answer 27

primarily dependent on the molarity of the solution.

Question 28

Van’t Hoff Factor

Answer 28

used in freezing point depression, boiling point elevation, and osmotic pressure calculations