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Chemistry > Test 12 > Flashcards

Test 12 Flashcards

(50 cards)

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1
Q

Homogeneous mixtures of variable composition in a single phase

A

Solutions

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2
Q

The most abundant substance in a solution

A

Solvent

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3
Q

Dissolved substances in a solution

A

Solute

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4
Q

A solution containing mercury

A

Amalgam

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5
Q

What is the only permanent gas solution at ordinary pressures

Why

A

Gaseous solvents dissolve and gaseous solutes.

Gases cannot dissolve liquid or solid particles because gas particles are so much smaller than liquid or solid particles

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6
Q

What is the governing principle in solutions

A

Like dissolves like

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7
Q

What is the maximum amount of a solute that can dissolve in a specific solvent under specific conditions, such as temperature and pressure

A

Solubility

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8
Q

What accounts for the different solubility

A

The strength of ionic attractions within compounds

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9
Q

Are supersaturated solution stable

A

No

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10
Q

What can affect the frequency of collisions with solvent particles

A

Temperature, stirring, and the amount of surface area of the solute exposed to the solvent

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11
Q

The escape of a gas from a liquid gas solution

A

Effervescence

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12
Q

What are the most common ways to express concentration

A

Percent by mass, molarity, and molality

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13
Q

What is the formula for percent by mass

A

Percent by mass =

(mass of solute/mass of solution) x100%

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14
Q

What is the formula for percent by volume

A

Percent by volume = (volume of solute/volume of solution) x100%

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15
Q

What’s the formula for molarity

A

Molarity (M) = mol solute/L solution

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16
Q

What four things change because of the presence of solutes instead of just a pure solvent

A

Freezing points
Boiling points
Vapor pressures
Osmotic pressures

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17
Q

The more concentrated a solution is, the___ the boiling point elevation will be

A

Greater

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18
Q

Solutions freeze at___temperatures than their pure solvents

A

Lower

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19
Q

What is osmotic pressure of a solution

A

The amount of pressure required to prevent osmosis from occurring

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20
Q

Why is osmotic pressure of a solution a colligative property

A

Because it depends on the number of particles in a solution

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21
Q

Why should the solution surrounding a cell be kept at the same osmotic pressure as a solution inside the cell

Study These Flashcards
A

If the equilibrium is disturbed, water could leave the cell in sufficient quantities and cause dehydration
OR water could enter the cell and cause the membrane to burst

22
Q

What happens if a cell is placed in a hypertonic solution

Study These Flashcards
A

Water will flow out of the cell into the surrounding solution

23
Q

What happens if a cell is placed in a hypotonic solution

Study These Flashcards
A

Water will flow into the cell, causing it to swell and possibly burst

24
Q

What is isotonic

Study These Flashcards
A

When concentrations on both sides of the membrane are equal

25
Mixtures that contain larger particles that will eventually settle out of the mixture
Suspension
26
Fog is a__
Colloid
27
What phases can a colloid exist in
Solids, liquids, and gases
28
Can a gas/gas colloid exist why or why not
No, they are always solutions
29
List three types of colloids
Foams Aerosols Gels
30
Completely describe the three steps involved in practical water treatment
1- pathogens are killed by chlorinating the water with chlorine dioxide or similar compounds 2- other compounds are added to clump impurities together causing coagulation 3- The water is passed through a filter under pressure to quickly remove impurities
31
Gas/gas is
Only a solution
32
What keeps particles smaller than 1000 nm in colloids from setting out
Intermolecular collisions
33
M=
Mol/L
34
K(b)
Molal boiling point
35
Delta T(b)
The CHANGE in boiling point NOT The new boiling point! ADD original to get new one
36
Pertaining to two liquids that are not soluble in each other
Immiscible
37
The process in which solvent particles surround and interact with solutes The dissolving process in solid-in-liquid solutions
Solvation
38
A type of solvation in which water molecules surrounded interact with solute particles
Hydration
39
A type of solvation in which an ionic compound forms ions when it dissolves in a solvent
Dissociation
40
A type of solvation in which a covalent compound forms ions when it dissolves in a solvent
Ionization
41
The inability of a solute to dissolve in a certain solvent
Insoluble
42
A chemical equilibrium in which two or more opposing events occur at the same rate that results in no net change
Dynamic equilibrium
43
A quantitative measure of concentration equal to the number of moles of solution per kilogram of solvent
Molality (m)
44
A physical property of a solution that depends only on the number of solute particles present without regard to type
Colligative property
45
A number that relates the change in boiling point of a particle solvent to the concentration of solute particles
Molal boiling point constant K(b)
46
The diffusion of pure solvent molecules, such as water, through a semi permeable membrane
Osmosis
47
A mixture of small particles that remain dispersed in a medium
Colloid
48
In a colloidal mixture, the phase in which the particles are spread out
Dispersed phase
49
The scattering of light by particles in a colloid
The Tyndall effect
50
The random, chaotic movements of microscopic particles
Brownian motion

Chemistry (32 decks)

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