Chapter 9 Solutions

Question 1

What is solvation/dissolution?

Answer 1

The breaking of intermolecular bonds in solvent and solute and new bonds forming.

Question 2

Are dissolutions endo or exothermic?

Answer 2

Endothermic.

Gas into liquid is exothermic

Question 3

What is solubility?

Answer 3

Max amount of a solute that can be dissolved in a given solvent at a given temperature.

Question 4

Which compounds are soluble in water?

Answer 4

• ammonium (NH4+)
• nitrate (NO3−)
• acetate (CH3COO−)
• Alkali metal (Group 1)

Question 5

What is a complex ion/coordination compound?

Answer 5

metallic ions bound to neutral compounds and anions (ligands)

Question 6

What is the mole fraction?

Answer 6

moles of solute per total moles

used for calculating vapor pressure depression and partial pressures of gases

Question 7

What is Molarity?

Answer 7

moles of solute per liters of solution

used for rate laws, the law of mass action,
osmotic pressure, pH and pOH, and the Nernst equation

Question 8

What’s molality?

Answer 8

moles of solute per kilograms of solvent

used for boiling
point elevation and freezing point depression.

Question 9

What’s normality?

Answer 9

molarity of the stuff of interest in a rxn.

the molarity of the species of interest and is used for acid–base and Oxidation–Reduction reactions.

Question 10

What is the ratio of volume of solution and solvent in dilute solutions?

Answer 10

volume of solution and solvent are approximately equal

Question 11

Difference between Keq and Ksp?

Answer 11

No denominator b/c of solid salt reactant.

Question 12

What is the Ion Product (IP)?

Answer 12

Solubility outside equilibrium conditions. (Keq out of eq.)

Question 13

What does it mean if IP < Ksp?

Answer 13

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

Question 14

What does it mean if IP = Ksp?

Answer 14

the solution is saturated (at equilibrium), and there will be no change in concentrations

Question 15

What does it mean if IP > Ksp?

Answer 15

the solution is supersaturated, and a precipitate will form

Question 16

What is the formation/ stability constant (Kf)?

Answer 16

Measures Eq. for complex formation in solution.

usually greater than Ksp

Question 17

How does formation of a complex increase solubility?

Answer 17

By shifting by forming complexes with those ions and therefore taking them out of solution.

Question 18

What is the common ion effect?

Answer 18

decreases the solubility of a compound in a solution that already contains one of the ions in the compound. (by decreasing its dissociation)

Question 19

What are colligative properties?

Answer 19

The presence of a solute can affect the properties of a solution.
B/c of amount of solute not properties

Question 20

What is Raoult’s Law (vapor pressure depression)?

Answer 20

Presence of solutes decreases evaporation rate of solvent but condensation is same.

Question 21

What is freezing point depression?

Answer 21

Solute interferes with formation of lattice arrangement of solvent.

Question 22

What is Boiling point elevation?

Answer 22

Decrease in vapor pressure due to increase in nonvolatile solute (group 1).
Raises boiling point.

Question 23

What is Vapor Pressure?

Answer 23

measure of the tendency of a material to change into the gaseous or vapour state

Question 24

What is the van’t Hoff factor?

Answer 24

number of particles into which a compound dissociates in solution.