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CHM > Ch.13 > Flashcards

Ch.13 Flashcards

1
Q

Solution

A

A homogenous mixture with at least two components.

Ex. Ocean Water (Salt and Water)

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2
Q

Solvent

A

The majority component in a solution; what the other component mixes into.
*The liquid is almost always the solvent regardless of ratio
CO2- Solute
H2O- Solvent

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3
Q

Solute

A

The minority component of the solution that ‘mixes in’.

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4
Q

Aqueous Solution

A

A solution with water as the solvent.

*Water is the most common solvent because of it’s abundance on Earth.

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5
Q

Like Dissolves Like

A

Polar solvents (such as water), dissolve other polar solute, while nonpolar solvents dissolve other nonpolar solutes.

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6
Q

Insoluble

A

Compounds, molecules etc. that do not dissolve in solvents.

Ex. Calcium Carbonate

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7
Q

How do solids dissolve in water?

A

The solvent-solute attraction must overcome that of the solvent-solvent and solute-solute attractions (usually intermolecular forces).
The negatively charged ions are attracted to positively charged dipoles and vice versa.

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8
Q

Solubility

A

The amount of the compound, in grams, that dissolves in a certain amount of liquid.

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9
Q

Saturated Solution

A

The maximum amount of solute is held, more solute added will not dissolve.

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10
Q

Unsaturated Solution

A

Less than the maximum amount of solute is held and more can be added.

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11
Q

Supersaturated solution

A

More than normal amount of solute is held and the solute will precipitate.

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12
Q

Electrolyte Solutions

A

Hold dissolved ions, charged particles, and conduct electricity.

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13
Q

Non-electrolyte Solution

A

Hold dissolved molecules, neutral particles, and do not conduct electricity.

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14
Q

Solubility of Solids and Temp.

A

The solubility of solids in a liquid is directly proportional to temp. As temperature rises, so does solubility.

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15
Q

Recrystallization

A

Solid is added to solvent at high temperature enough to make a saturated solution then allowed to cool slowly, reducing solubility steadily, causing the solid to precipitate as pure crystals.

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16
Q

Solubility of Gases and Temp.

A

The solubility of gas and temperature is inversely proportional, as temperature increases, solubility decreases.
Ex. Warm soda fizzes much more than cold soda.

17
Q

Henry’s Law

A

The higher the pressure of gas above a liquid, the higher the solubility.
Ex. This is why soda pops when opened. Pressure is released decreasing solubility and causing co2 to bubble out of the solution.

18
Q

Mass Percent

A

Concentration of a solution or the number of grams of solute per 100g of solution.

19
Q

Mass Percent Equation

A

Mass percent=
Mass Solute / (mass of solute + mass of solvent) x 100%.

Or

Mass Percent = g solute/ 100g solution

20
Q

Molarity

A

The number of moles of solute over liter of solution.

Molarity (M) = Moles of Solute/ Liters of Solution

21
Q

Concentration of a solution containing a Molecular Compound

A

Reflects the concentration of the solute as it actually exists in the solution.

22
Q

Concentration of a solution containing an Ionic Compound

A

Reflects the concentration of the solute before it is dissolved in the solution.

23
Q

Dilution

A

Adding water to a stock solution to make it less concentrated.

24
Q

Dilution Equation

A

M1V1=M2V2

Where M is molarity and V is volume.

25
Q

Colligative Properties

A

Properties that depend on the number of dissolved solute particles and not the type of solute particles.

26
Q

Non-volatile solute

A

A solute that does not readily evaporate.

27
Q

Freezing Point Depression

A

Adding a non-volatile solute to a solution in order to lower its freezing point.

28
Q

Boiling Point Elevation

A

Adding a non-volatile solute to a solution to make it’s boiling point higher.

29
Q

Molality (m)

A

Used to express the concentration of solution with freezing point depression and boiling point elevation.

Reflects the number of moles of solute per kilogram of SOLVENT.

30
Q

Freezing Point Depression Quantification

A

^Tf = m x Kf

Where: ^T is he change in temp. In C.
M is the molality
Kf is the constant 1.86 Ckg solvent/mol solute

31
Q

Boiling Point Elevation Quantification

A

^Tb=m x Kb

Kb= 0.512 Ckg solvent/mol solute

32
Q

Osmosis

A

The flow of solvent from a less concentrated solution to a more concentrated solutions.

33
Q

Osmotic Pressure

A

The pressure created when enough excess fluid crosses the semipermeable membrane. A colligative property; the more concentrated a solution to greater the osmotic pressure.

34
Q

Hypoosmotic

A

Solutions having osmotic pressures less than that of bodily fluids. Pump water into cells.

35
Q

Hyperosmotic

A

Solutions that have osmotic pressures greater than that of bodily fluids. Pump water out of cells.

36
Q

Isoosmotic

A

Solutions that have osmotic pressure equal to bodily fluids.

CHM (1 decks)

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