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General Chemistry II > Solutions & Colloids > Flashcards

Solutions & Colloids Flashcards

1
Q

Solution

A

A homogenous mixture of two or more substances, dispersed on a molecular scale, will not settle out or separate, composition of solution/concentrations vary continuously.

(*)If bubbles of gas are observed within a liquid, the mixture is not homogenous and thus, not a solution.

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2
Q

Solvent

A

The component of a solution which is present in a greater concentration.

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3
Q

Solute

A

The component of the solution which is present in lesser concentration.

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4
Q

Aqueous solution

A

A solution in which the solvent is water.

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5
Q

Dissolution

A

The process where a solute in gaseous, liquid or solid phase dissolved into a solvent to form a solution.

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6
Q

What impacts dissolution?

A

Nature of solvent and salute, temperature, pressure, degree of mixing and degree of saturation.

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7
Q

Spontaneous process

A

A process that occurs under specific conditions without the requirement of energy from some external source.

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8
Q

What are some things which are common for spontaneous processes?

A

A decrease in the internal energy of the system (exothermic change).

Increase dispersal of matter in the system (increase in entropy); entropy is the measure of random activity in the system meaning energy that cannot be used for any work.

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9
Q

Ideal solution

A

When strengths of intermolecular forces of attraction between solute and solvent species in a solution are no different than those present in the separated components, the solution is formed with no accompanying energy change.

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10
Q

Electrolytes

A

A chemical compound that dissociates into ions (i.e. solution which is capable of transporting electric charge).

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11
Q

Strong electrolyte

A

When all of the dissolved compound yields ions

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12
Q

Weak electrolyte

A

When a small fraction of dissolved substance undergoes ion-producing process

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13
Q

Ion-dipole attraction

A

The electrostatic attraction between an ion and a molecule with a dipole.

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14
Q

Dissociation

A

When ionic compounds dissolve in water, the ions in the solid separate and disperse uniformly throughout the solution; water molecules surround and solvate the ions, reducing the strong electrostatic forces between them.

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15
Q

Solubility

A

The maximum concentration that may be achieved under given conditions when the dissolution process is at equilibrium (i.e. when the rate of dissolution is equal to the rate of precipitation).

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16
Q

Saturated

A

When a solutes concentration is equal to its solubility.

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17
Q

Unsaturated

A

When a solutes concentration is less than it’s solubility.

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18
Q

Dilute

A

A solution that contains a relatively low concentration of solute.

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19
Q

Concentrated

A

When a solution has a relatively high concentration.

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20
Q

Supersaturated

A

When a solute concentration exceeds its solubility.

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21
Q

Henry’s law

A

The quantity of an ideal gas that dissolves in a definite volume of liquid is directly proportional to the pressure of the gas.

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22
Q

Miscible

A

Liquids which may be mixed in any proportion to yield solutions; infinite mutual solubility.

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23
Q

Immiscible

A

Two liquids that do not mix on an appreciable extent.

24
Q

Partially miscible

A

Two liquids which have moderate mutual solubility.

25
Q

What may impact the solubility of a solid in a liquid and how?

A

Solubility typically increases with temperature (though there are exceptions).

26
Q

Colligative properties

A

Physical changes that result from adding a solute to a solvent.

These include: vapor pressure lowering, boiling point elevation, freezing point depression and osmotic pressure.

27
Q

The mole fraction (X)

A

The ratio of its molar amount to the total number of moles of all solution components.

(mol A/total mol of all components)

28
Q

Molarity

A

A concentration unit defined as the ratio of the numbers of moles of solute to the mass of the solvent in kilograms.

(mol solute/kg solvent)

29
Q

Equilibrium vapor pressure of a liquid

A

The pressure exerted by its gaseous phase when vaporization and condensation are occurring at equal rates.

30
Q

What happens when a nonvolatile substance is dissolved into a volatile liquid?

A

A decrease in the liquids vapor pressure will occur.

31
Q

What is the effect of having a lower vapor pressure on boiling point?

A

Boiling point increases as vapor pressure decreases.

32
Q

Raoult’s law

A

The partial pressure exerted by any component of an ideal solution is equal to the vapor pressure of the pure component multiplied by its mole fraction in the solution.

33
Q

Dalton’s law of partial pressure

A

States that the total pressure of a mixture of gases is the sum of the partial pressures of its components.

34
Q

How do you calculate the vapor pressure of a solution containing a nonvolatile solute?

A

The vapor pressure of the solution is then dependent on the solvent alone.

P solution = X solvent✖️ P* solvent

35
Q

Distillation

A

A method of separating solutions whose components have significantly different vapor pressures.

Selective vaporization process.

36
Q

Boiling point elevation

A

The boiling point of a liquid (a solvent) will be higher when another compound is added.

37
Q

Boiling point elevation constant

A

The change in the boiling point for a 1 -molal solution of a nonvolatile molecular solute. Represented by Kb.

This constant depends on the identity of the solvent.

38
Q

Freezing point depression

A

The decrease in freezing point of a dilute solution compared to that of the pure solvent.

39
Q

Freezing point depression constant

A

Represented by Kf. AKA cryoscopic constant. Dependent on the chemical identity of the solvent.

40
Q

Semipermeable membranes

A

Membranes that only allow molecules or ions of a certain size, shape, polarity, charge to pass through.

41
Q

Osmosis

A

Diffusion-driven transfer of solvent molecules through a semipermeable membrane.

42
Q

Osmotic Pressure

A

The minimum pressure that must be applied to a solution to halt the flow of solvent molecules through a semipermeable membrane.

(Osmotic pressure) = (molar concentration of solute) (ideal gas constant) (temperature in kelvin)

43
Q

Reverse osmosis

A

When pressure greater than osmotic pressure is applied, the solvent will be pushed to the less concentrated (more pure) solution.

This is used to remove contaminants from water, thus purifying it.

44
Q

Isotonic

A

When a solution has the same concentration of solutes as another solution across the semipermeable membrane.

Solutions injected into the body must have the same osmotic pressure as blood serum.

45
Q

Hypotonic

A

A solution that has a lower concentration of solute compared to the cell— lower osmotic pressure.

This would cause a blood cell to expand and rupture.

46
Q

Hypertonic

A

A solution which has a greater concentration of solutes on the outside of the cell when compared to the inside of the cell.

This would cause a blood cell to wither and die.

47
Q

Hemolysis

A

The rupture or destruction of red blood cells.

48
Q

Crenation

A

The state of being or becoming shrunken with a notches or indented edge.

49
Q

Van’t Hoff Factor

A

The number of moles of particles formed in solution per mole of solute. Represented by i.

Van’t Hoff factors for electrolytes are for 0.05 m solutions.

i = (moles of particles in solution)/(moles of formula units dissolved)

50
Q

Activity

A

Effective concentration

51
Q

Suspensions

A

Heterogeneous mixtures composed of relatively large particles that are visible (or that can be seen with a magnifying glass). Suspended particles settle out after mixing.

This is another class of mixtures, diverse from solutions or colloids.

52
Q

Colloids (or colloidal dispersion)

A

Exhibit properties intermediate between those of suspensions and solutions.

Particles are larger than most simple molecules, but small enough that they do not settle out.

53
Q

Tyndall effect

A

The particles in a colloid that are large enough to scatter light.

Clouds are colloidal mixtures.

54
Q

“Colloid” origin

A

From Greek word, ‘kolla,’ meaning, “glue,” and, ‘eidos,’ meaning, “like”.

Was first used to classify mixtures such as starch in water and gelatin.

55
Q

Dispersed phase

A

The particulate component present in relatively minor amount in colloid.

56
Q

Dispersion medium

A

The substance of solution throughout which the particulate is dispersed.

General Chemistry II (2 decks)

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