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9th Grade > Solubility > Flashcards

Solubility Flashcards

1
Q

Solutions

A
  • Formed when substances dissolve in other substances.
  • Homogeneous mixtures.
  • Single phase.
  • Remain mixed; particles do not settle out.
  • Cannot be separated by filtration.
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2
Q

Solvent

A
  • Present in larger amount.

- Dissolves the solute to make the solution.

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3
Q

Solute

A
  • Present in smaller amount.

- Dissolved in the solvent.

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4
Q

Liquid Solutions (Types of Solutions)

A
  • Liquid solvent in which a gas, solid, or liquid is dissolved.
    • Ex: carbonated drink.
  • Liquid in liquid.
    • Ex: antifreeze in water.
  • Solid dissolved in a liquid.
    • Ex: salt water.
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5
Q

Miscible

A
  • Two liquids mix.
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6
Q

Immiscible

A
  • Two liquids don’t mix.
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7
Q

Solid Solutions (Types of Solutions)

A
  • Alloys: solid mixtures of metals (brass is a mixture of copper and zinc).
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8
Q

Gas Solutions (Types of Solutions)

A
  • Gases dissolved in each other (air is most common example).
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9
Q

Aqueous

A
  • Water is the solvent.
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10
Q

Tincture

A
  • Alcohol is the solvent.
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11
Q

Suspension

A
  • A heterogeneous mixture.
  • Particles in the solvent are thousands of times larger than molecules and ion.
  • Particles will settle out upon standing.
  • Can be separated by filtration.
  • Exhibit the Tyndall Effect – the scattering of light in all directions.
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12
Q

Colloid

A
  • Particles are intermediate in size between those of suspension and true solutions.
  • Particles do not settle out upon standing.
  • Can not be separated by filtration.
  • Exhibit the Tyndall Effect.
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13
Q

Emulsion

A
  • Colloidal dispersion of liquids in liquids.
  • Emulsifying agent is necessary for maintaining stability.
    • Ex: Soap.
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14
Q

Electrolyte

A
  • Dissolves in water to form a solution that conducts electric current.
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15
Q

Non-electrolyte

A
  • Dissolves in water to form a solution that does not conduct electric current.
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16
Q

Surface Area (Factors Affecting the Rate of Solution)

A
  • Increasing the surface area of the solute by crushing speeds up dissolving by increasing the number of collisions between the solute and the solvent surface.
17
Q

Agitation (Factors Affecting the Rate of Solution)

A
  • Stirring or shaking helps to disperse solute particles, increasing the number of collisions between the solute and the solvent surface.
18
Q

Heating (Factors Affecting the Rate of Solution)

A
  • Increases the average kinetic energy of the solvent molecules so that collisions between the solvent molecules and the solute are more frequent.
19
Q

Saturated

A
  • Solution containing all the dissolved solute possible at given conditions of temperature and pressure.
20
Q

Unsaturated

A
  • Solution containing less dissolved solute that the maximum amount that can be dissolved at given conditions of temperature and solution.
21
Q

Supersaturated

A
  • Unusual solution containing more dissolved solute than is normally possible at given conditions of temperature and pressure.
22
Q

Solubility

A
  • A measure of how much solute can dissolve in a given amount of solvent at a specific temperature.
23
Q

Dilute Solution

A
  • The amount of solute dissolved is small in relation to the amount of solvent present.
    • Ex: A teaspoon of salt would dissolve in a gallon of water.
24
Q

Concentrated Solution

A
  • The amount of solute dissolved is large in relation to the amount of solvent present.
    • Ex: A teaspoon of salt would dissolve in a cup of water.
25
Q

Nature of Solute and Solvent (Factors Affecting Solubility):

A
  • “Like dissolves like.”

- Ex: Polar solutes dissolves in polar solvents; non-polar solutes dissolves in non-polar solvents.

26
Q

Temperature (Factors Affecting Solubility)

A
  • Generally, increasing the temperature of the solution increases the solubility of a solid solute.
  • Increasing the temperature of the solution decreases the solubility of a gaseous solute.
27
Q

Pressure (Factors Affecting Solubility)

A
  • Only affects the solubility of a gaseous solute.
  • Increasing pressure increases solubility.
  • Decreasing pressure decreases solubility.
28
Q

Henry’s Law

A
  • The mass of a gas dissolved in a given volume of liquid is directly proportional to the pressure of the gas.
29
Q

Molarity

A
  • Expresses solution concentration.
  • Molarity = moles of solute/liters of solution
  • Molarity, molar, M, and mol/liter all represent the same ratio.
30
Q

Colligative Properties

A
  • Any of the properties of a solution that change when the concentration of the solution changes.
  • Depend on the number of particles dissolved in a given mass of solvent.
31
Q

Vapor Pressure Depression (Examples of Colligative Properties)

A
  • The lowering of the vapor pressure of a liquid that occurs when substances are dissolved in the liquid.
  • Vapor Pressure: the pressure of a vapor in equilibrium with its liquid.
32
Q

Freezing Point Depression (Examples of Colligative Properties)

A
  • The lowering of the freezing point of a liquid that occurs when substances are dissolved in the liquid.
    • Ex: using antifreeze in car radiators and salt on icy roads.
33
Q

Boiling Point Elevation (Examples of Colligative Properties)

A
  • The raising of the boiling point of a liquid that occurs when substances are dissolved in the liquid.
  • Boiling occurs when vapor pressure equals external/atmospheric pressure.
    • Ex: antifreeze in a car acts as a coolant in the summer.)
34
Q

More Examples of Colligative Properties

A

Color, taste, and density.

9th Grade (2 decks)

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