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Gen Chem 2 > Chapter 13 > Flashcards

Chapter 13 Flashcards

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1
Q

Solutions

A

Homogenous mixtures of two or more substances

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2
Q

Solute

A

Lesser amount

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3
Q

Solvent

A

More in content

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4
Q

Natural tendency

A

-mixing of gas is spontaneous process
-each gas acts as it is alone
-increase of disorder
-formation of solution favors entropy

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5
Q

Entropy

A

Disorder

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6
Q

Crystallization

A

opposing processes of a solution

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7
Q

Saturated solution

A

When the opposing processes is equal , the additional solute will not dissolve unless some crystallizes from the solution.

Have the solute dissolved at the temp

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8
Q

Unsaturated solution

A

When the amount of crystallization is not reached

Any amount of solute less than the max amount dissolved in the solution

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9
Q

Solubility

A

The amount of solute that can dissolve in a given amount of solvent at a given temp

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10
Q

Supersaturated

A

The solvent holds more solute than normal at a possible temp

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11
Q

Factors that affect solubility

A

Solute - solvent interactions
Temperature
Pressure for gas solutes

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12
Q

Will it dissolve

A

Solvent and solvent have similar structures
Polar and ionic more soluble in polar solvent
Nonpolar more soluble in nonpolar solvents

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13
Q

Temperature effect relative to solubility

A

Solids - temp increases solubility increases
Gases- temp increases solubility decreases
- higher mass more solubility

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14
Q

Solubility of gases

A

Solubility of gas directly proportional to its partial pressure

Sgas= Kh * Pgas

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15
Q

Miscible and immiscible

A

Mix in all proportions
Do not mix

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16
Q

Mass percent

A

= (mass of component / total mass of soln) x 100

17
Q

PPM

A

Parts per million
10^6
=(mass of component in soln/total mass of soln) x 10^6

18
Q

PPB

A

Parts per billion
10^9
=(mass of component in soln/total mass of soln) x 10^9

19
Q

Mole fraction

A

=moles of component / total moles of all components

20
Q

Molarity

A

=mol of solute / liters of the solution

21
Q

Molality

A

=mol of the solute / Kg of solvent

22
Q

Colligative properties

A

Depend on quantity not the identity of solute
Vapor pressure lowering
Boiling point elevation
Freezing point depression
Osmotic pressure

23
Q

Electrolyte

A

Separates into ions when in water
Strong ones dissociate completely while weak ones dissociate very little

24
Q

Nonelectrolyte

A

Do not dissociate to form ions

25
Q

Vapor pressure
Relating to pure solutions and mixed solutions

A

Solvent must be greater for pressure to go up , when something is pure solvent the pressure goes up but adding a solute lowers the pressure.

26
Q

Raoult’s Law

A

Puré solvent
Psolvent=Xsolvent * Psolvent

Solute present
DeltaPsolvent = Xsolute * Psolvent

27
Q

Boiling Point elevation

A

Vapor pressure is lowered. Requires more tempt boiling point is increased

DeltaB = Tbsolution - Tbsolvent = iKbm

28
Q

Freezing Point depression

A

When the boiling point is raised the freezing point is lowered
DeltaTf= Tfsolution - Tf solvent = -iKfm

29
Q

Van’t Hoff factor

A

The ratio of moles of solute particle to moles of formula units dissolved , to find this first figure out if its an electrolyte if yes then the subscripts are the hoff factor and if not then its 1

30
Q

Ósmosis

A

net movement of solvent molecules from solution of low to high concentration of solute across a semipermeable membrane
[] = iMRT

31
Q

Isotonic
Hypotonic
Hypertonic

A

Same
Lower low P solvent will leave the solution at higher rate
Hyper higher p ,solvent will enter solution higher rate

32
Q

Colloids

A

Suspensión particles larger than ions but small enough for gravity not to settle them

33
Q

Tyndall effect

A

Colloidal suspensions can scatter rays of light

34
Q

Hydrophilic
Hydrophobic

A

Water loving
Water fearing

Gen Chem 2 (3 decks)

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