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Chemistry 143 > Chapter 14: Solutions > Flashcards

Chapter 14: Solutions Flashcards

1
Q

Solution

A

Homogenous mixture of two or more substances

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2
Q

Solvent

A

Major component in solution

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3
Q

Solute

A

Minor component in solution

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4
Q

Aqueous Solution

A
  • Water is solvent
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5
Q

Solubility

A

Amount of substance that will dissolve in given amount of solute

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6
Q

Entropy

A
  • Measure of energy randomization/dispersal in a system - Tendency is for energy to spread out/disperse whenever unrestrained
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7
Q

Intermolecular Forces

A
  • Dispersion: Weak - Dipole-Dipole: Separation of charges lead to electrostatic attraction - Hydrogen bond: Observe what H is bonded to; different in electronegativity - Ion dipole: Electrostatic force between ion and neutral molecule with dipole
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8
Q

Solution Interactions

A
  • Solute-Solvent: Interactions between solvent particles and solute particles - Solvent-Solvent: Interactions between solvent particle and another solvent particle
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9
Q

Interactions and Formation

A
  • Solvent-Solute > Solvent Solvent and Solute-Solute Interactions = Solution Formation - Solvent-Solute = Solvent-Solvent and Solute-Solute = Solution formation - Solvent-Solute < Solvent-Solvent and Solute-Solute = may or may not form
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10
Q

Polar Solvent Examples

A
  • Water, acetone, methanol, ethanol
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11
Q

Non polar solvent examples

A
  • hexane, diethyl ether, toluene, carbon tetrachloride
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12
Q

Hess’s Law

A

Overall enthalpy change upon solution formation is sum of enthalpy ∆Hsoln = ∆Hsolute + ∆Solvent + ∆Hmix (endothermic) - If ∆Hmix is more than the remaining, heat of solution is negative (exothermic)

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13
Q

Heat of Hydration

A
  • Enthalpy change when 1 mol of gaseous solute ions are dissolve in H2O - Typically negative ∆Hsoln = ∆Hsolute + ∆Hydration - Take absolute value of ∆Hsoln and ∆Hhydration to compare; if solute is more, amount of E to separate solute into constituent ions is less than energy given off when an ion is hydrate (process is exothermic)
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14
Q

Dynamic Equilibrium

A
  • Rates of dissolution and recrystallization become equal
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15
Q

Saturated solution

A
  • Solution in which dissolved solute is in dynamic equilibrium with solid solute (undissolved)
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16
Q

Unsaturated solution

A

Solution containing less than equilibrium amount of solute

17
Q

Supersaturated solution

A

One containing more than equilibrium amount of solute; often unstable and excess solute precipitates out

18
Q

Effect of temperature on solids in H2O?

A
  • Solubility of most solids in water increases with increasing temperature
19
Q

Factors affecting solubility of gases in H2O?

A
  • Temperature: Solubility of gases in liquids decrease with increasing temperature - Pressure: Higher the pressure of a gas above a liquid, the more soluble it becomes
20
Q

Henry’s Law

A

Sgas = kHpgas

21
Q

Dilute solution

A

Contains small quantities of solute relative to amount of solvent

22
Q

Concentrated solution

A

Contains large quantities of solute relative to amount of solvent

23
Q

Molarity

A

(M) amount of solute (mol) / volume solution (L)

24
Q

Molality

A

(m) amount solute (mol) / mass solvent (kg) - Temperature independent

25
Q

Mole fraction (X)

A

amount solute (mol) / total amount solute + solvent (mol)

26
Q

Mole %

A

amount solute (mol) / total amount solute + solvent (mol) x 100%

27
Q

Parts by mass

A

mass solute / mass solution x multiplication factor

28
Q

Colligative properties

A

Properties that depend on number of particles dissolve in solution

29
Q

Vapor Pressure Lowering

A

VP of liquid = P of gas above the liquid when the two are in dynamic equilibrium

30
Q

Raoult’s Law

A

Psolution = XsolventP˚solvent

31
Q

Two Component Solution

A

PA = XAP˚A

PB = XbP˚B

Total Pressure = Ptot = PA + PB

32
Q

Nonideal Solution

A
  • Solute-solvent interactions are either stronger or weaker than solvent-solvent interactions
  • If solute-solvent stronger: Solute tends to prevent solvent from vaporizing readily
  • Solution is dilute: Effect = small
  • Solution is not dilute = effect is significant
33
Q

Freezing Point Depression

A

∆Tf = m x Kf

  • Tf = change in temp in celsius
  • m = molality
  • Kf = freezing point depression
34
Q

Osmosis

A
  • Flow of one solvent from solution of lower solute concentration to one of higher concentration
35
Q

Semipermeable Membrane

A
  • Membrane that selectively allows some substances to pass through but not others
36
Q

Osmotic Pressure Equation

A

π = MRT

  • M - molarity
  • T - Temperature in Kelvin
  • R - Ideal gas constant (0.08206…)
37
Q

van Hoff Factor

A
  • (i) Ratio of moles of particles in solution to moles of formula units dissolved

i = moles of particles in soln. / moles formula units

38
Q

van Hoff Factor Equations

A

∆Tf = im x Kf

∆Tb = im x Kb

π = iMRT

Chemistry 143 (9 decks)

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