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Chemistry > Test 12 > Flashcards

Test 12 Flashcards

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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

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

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

A

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

24
Q

What is isotonic

A

When concentrations on both sides of the membrane are equal

25
Q

Mixtures that contain larger particles that will eventually settle out of the mixture

A

Suspension

26
Q

Fog is a__

A

Colloid

27
Q

What phases can a colloid exist in

A

Solids, liquids, and gases

28
Q

Can a gas/gas colloid exist why or why not

A

No, they are always solutions

29
Q

List three types of colloids

A

Foams
Aerosols
Gels

30
Q

Completely describe the three steps involved in practical water treatment

A

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
Q

Gas/gas is

A

Only a solution

32
Q

What keeps particles smaller than 1000 nm in colloids from setting out

A

Intermolecular collisions

33
Q

M=

A

Mol/L

34
Q

K(b)

A

Molal boiling point

35
Q

Delta T(b)

A

The CHANGE in boiling point NOT The new boiling point!

ADD original to get new one

36
Q

Pertaining to two liquids that are not soluble in each other

A

Immiscible

37
Q

The process in which solvent particles surround and interact with solutes

The dissolving process in
solid-in-liquid solutions

A

Solvation

38
Q

A type of solvation in which water molecules surrounded interact with solute particles

A

Hydration

39
Q

A type of solvation in which an ionic compound forms ions when it dissolves in a solvent

A

Dissociation

40
Q

A type of solvation in which a covalent compound forms ions when it dissolves in a solvent

A

Ionization

41
Q

The inability of a solute to dissolve in a certain solvent

A

Insoluble

42
Q

A chemical equilibrium in which two or more opposing events occur at the same rate that results in no net change

A

Dynamic equilibrium

43
Q

A quantitative measure of concentration equal to the number of moles of solution per kilogram of solvent

A

Molality (m)

44
Q

A physical property of a solution that depends only on the number of solute particles present without regard to type

A

Colligative property

45
Q

A number that relates the change in boiling point of a particle solvent to the concentration of solute particles

A

Molal boiling point constant K(b)

46
Q

The diffusion of pure solvent molecules, such as water, through a semi permeable membrane

A

Osmosis

47
Q

A mixture of small particles that remain dispersed in a medium

A

Colloid

48
Q

In a colloidal mixture, the phase in which the particles are spread out

A

Dispersed phase

49
Q

The scattering of light by particles in a colloid

A

The Tyndall effect

50
Q

The random, chaotic movements of microscopic particles

A

Brownian motion

Chemistry (32 decks)

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