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Physical Pharmacy > HOMOGENOUS SYSTEM > Flashcards

HOMOGENOUS SYSTEM Flashcards

1
Q

consist of at least two phases ÿith one or more internal/disperse phases contained in a single continuous/external phase

A

Dispersion

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2
Q

suspended particles are completely dissolþed; not large enough to scatter light but are small enough to be disperses = homogenous

A

True Solution

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3
Q

mixture of two or more components that form a homogenous molecular dispersion/one-phase sāstem.

A

True Solution

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4
Q

scattering of light

A

Tyndall effect

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5
Q

solution composed of only two substances: solute & solvent

A

Binary Solution

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5
Q

independent of the amount of the substances in the system

A

Intensive Properties

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6
Q

dependent on the quantity of the matter in the system

A

Extensive Properties

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7
Q

depend on the total contribution of the atoms in the molecule or on the sum of the properties of the constituents in a solution
* Molecular weight

A

Additive Properties

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8
Q

depend on the arrangement, and number and kind of atoms within a certain molecule.
* Refraction of light/ refraction
* Electric Properties
* Surface & Interfacial tension
* Solubility of drugs

A

Constitutive Properties

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9
Q

The triple point of air-free water, at which solid, liquid, and vapor are in equilibrium, lies at a pressure of 4.58 mmHg and a temperature of 0.0098C

delta Tf = Kfm

A

Depression of Freezing Point

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9
Q

HOMOGENOUS SYSTEM

A

Dispersion
True Solution
Binary Solution
Additive Properties
Constitutive Properties
Colligative Properties

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10
Q

depend mainly on the number of particles in a solution:
* Vapor pressure lowering
* Boiling point elevation
* Freezing point depression
* Osmotic Pressure

A

Colligative Properties

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11
Q

Raoult’s Law states that the vapor pressure of a solvent above a solution is equal to the vapor pressure of the pure solvent at the same temperature:

Psolution = (Xsolvent)(Psolvent)

A

Lowering of Vapor Pressure

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12
Q

“melting point” of a pure compound; the temperature at which the solid and liquid phases are inequilibrium under a pressure of 1 atm.

A

Freezing point

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12
Q

temperature at which vapor pressure of the liquid becomes equal to an external pressure of 1 atm

A

Boiling point

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13
Q

states that the vapor pressure of a solvent above a solution is equal to the vapor pressure of the pure solvent at the same temperature:

Psolution = (Xsolvent)(Psolvent)

A

Raoult’s Law

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14
Q

passage of the solvent into a solution through a semipermeable membrane; tends to equalize the “escaping tendency” of the solution on both sides of the membrane

A

Osmosis

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14
Q

The BP of a solution of a nonvolatile solute is higher than of the pure solvent as the solute lowers the VP of the solvent.

delta Tb = Kbm

A

Elevation of Boiling Point

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15
Q

Van’t Hoff Equation for OP

A

PoV = nRT

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16
Q

WHAT ARE THE TWO MAIN CLASSES OF SOLUTES?

A

Electrolytes
Non-electrolytes

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17
Q

substances (an acid, a base, or a salt) that in an aqueous solution ionize to “anions & cations.”

have greater freezing point depression and
boiling point elevation than non-electrolytes
of the same concentration.

→ NaCl

A

Electrolytes

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18
Q

substances that do not ionize when dissolved in water, and therefore do not conduct electricity through the solution.

→ sucrose, glycerin, naphthalene, and
urea

A

Non-electrolytes

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19
Q

“M” , “L”

–> Moles of solute in 1L of solution

A

Molarity

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20
Q

“N”

–> Gram equiþalent weights of solute in 1L of solution

A

Normality

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21
Q

“m”

–> Moles of solute in 1000 g of solþent

A

Molality

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22
Q

“N”, “x”

–> Ration of the moles of one constituent

(solute) of a solution to the total moles of all constituents (solute & solvent)

A

Mole fraction

23
Q

mg of solute in 100 ml of solution

A

Milligram percent

24
Q

“w/v”

–> g of solute in 100 mL of solution.

A

Percent weight-in-volume

24
Q

–> grams of solute in 100 g of solution.

“w/w”

A

Percent by weight

24
Q

–> mL of solute in 100 mL of solution

“v/v”

A

Percent by volume

25
Q

→No change in the ppts. of the components when they are mixed to form solution

A

Ideal Solutions

25
Q

Moles of one constituent in 100 moles of the solution; obtained by multiplying mole fraction by 100

A

Mole percent

25
Q

The partial vapor pressure of each volatile constituent = vapor pressure of the pure constituent x its mole fraction in the solution

A

Ideal Solutions

26
Q

Psolution = (Xsolvent)(Psolvent)

A

Lowering of Vapor Pressure

26
Q

No heat is evolved/ absorbed during the mixing process

A

Ideal Solutions

26
Q

PA= (VpA)(X)

A

Ideal Solutions

27
Q

No shrinkage/ expansion when the substances
are mixed

A

Ideal Solutions

28
Q

delta Tb = Kbm

A

Elevation of Boiling Point

29
Q

delta Tf = Kfm

A

Depression of Freezing Point

30
Q

→ (in gas) complete absence of attractive forces; (in solution) complete uniformity of attractive forces

A

Ideality

30
Q

→ does not adhere to Raoult’s law throughout the entire range of composition

A

Real Solution

31
Q

law applies to the solvent –
in dilute solutions of real liquid pairs

A

Raoult’s law

31
Q

law applies to the solute;

A

Henry’s law

31
Q

→When the adhesive attractions between molecules of different species exceed the cohesive attractions between like molecules, the vapor pressure of the solution is less than that expected from Raoult’s ideal solution.

A

Real Solution

32
Q

When, under a potential of several volts, a direct current flows through an electrolytic cell, a chemical rxn occurs.

A

Electrolysis

33
Q

[addition] of electrons to chemical species. Occurs at the cathode where electrons enter from external circuit, and are added to chemical species.

A

Reduction

34
Q

[removal]of electrons from chemical species. Occurs at the anode, where electrons are removed from the chemical species in solution and go into the external circuit.

A

Oxidation

34
Q

The fraction of total current carried by the cations/ anions; related to the velocities of the ions, the faster-moving ion = greater fraction of current.

A

Transference numbers

35
Q

Current =

A

Resistance (ohms)

“A, ampere”

35
Q

Velocities of ions are dependent on:

A
  • Hydration
  • Ion size & charge
35
Q

quantity of electricity in coulombs flowing per unit time.

A

Current

36
Q

The passage of 96, 500 coulombs of electricity through a conductivity which produces a chemical change of 1 g equivalent wt. of any substance.

A

Faraday’s Law

37
Q

Faraday, F

A

= 96,486 coulomb/ Eq. wt.
= 23,000 cal/volt Eq. wt.

38
Q

When electrolytes are dissolved in water, the solute exists in the form of ions in the solution.

A

ARRHENIUS THEORY

39
Q

Resistance in Ohms (Ω) of any uniform metallic/ electrolytic conductor
= directly proportional to its length
= inversely prop. to its cross-sectional
area (cm2)

A

Electrolytic Conductance

39
Q

NaCl exists as ions in the crāstalline state. Addition of later dissolves the crystals = dissociation of ions

A

ARRHENIUS THEORY

40
Q

H2O + HCl –> ?

A

H3O, Cl-

41
Q

H2O + NaCl –> ?

A

Na+, Cl-, H2O

42
Q

exists as a neutral molecules rather than ion. Addition of water = ionization

A

HCl

43
Q

→ NaOH, KOH, Ba(OH)2, Ca(OH)2

A

Inorganic bases

44
Q

Inorganic acids → HCl, HNO3, H2SO4, HI

Inorganic bases → NaOH, KOH, Ba(OH)2, Ca(OH)2

A

Strong electrolytes:

45
Q

→ HCl, HNO3, H2SO4, HI

A

Inorganic acids

46
Q

Acetic acid, Boric acid, Carbonic acid, Ammonium OH, Pb acetate HgCl2, HgI, HgBr

A

Weak electrolytes

47
Q

Strong electrolytes are completely ionized in dilute solution and that the derivations of electrolytic solutions from ideal behavior are du to the electrostatic effects of the oppositely charged ions.

A

DEBYE-HUCKEL THEORY

Physical Pharmacy (3 decks)

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