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Chemistry > Chemistry Unit 7 > Flashcards

Chemistry Unit 7 Flashcards

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1
Q

What are the types of solutions?

A

Liquid-Liquid
Solid-Liquid
Liquid-Gas
Gas-Gas
Solid-Solid

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2
Q

Example of liquid-liquid solution

A

ethanol and water – ALC

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3
Q

Example of Liquid-Solid solution

A

water and salt – salt water

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4
Q

Ex. Liquid - gas solution

A

co2 and water – fizzy water

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5
Q

ex. of gas gas solution

A

n2 and o2 – air

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6
Q

ex. of solid solid solution

A

alloys – bronze steel etc

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7
Q

What does immiscible mean

A

parts of solution cant mix ( wont form a homogenous mixture together)

ex: oil and water

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8
Q

What does miscible solution mean

A

The parts of a solution can be mixed in any proportion

Ex. Water and ethanol

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9
Q

What does solubility mean

A

It is the ability of a solute to dissolve in a solvent to form a solution

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10
Q

What are intramolecular forces

A

strong forces within molecules
Ex: covalent bonds

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11
Q

What are intermolecular forces

A

forces between molecules

** due to dipoles

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12
Q

Why is water a good solvent

A

because its a very polar substance

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13
Q

How does water interact with other polar molcules?

A

by making h bonds or dipole dipole

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14
Q

What are the most polar substances?

A

Ionic compounds

ex: NaCl –> Na+ and Cl-

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15
Q

What happens to ionic compounds when they disolve

A

They DISSOCIATE into hydrated ions (aq)

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16
Q

what represents the Dissociation of ionic compounds

A

Dissociation equation

Ex: NaCl(s) –> Na+(aq) + Cl-(aq)

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17
Q

Do non polar molecules dissolve in polar solvents

A

NO – Like disolves like

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18
Q

Will molecules that have non polar and polar sections dissolve in water?

A

Yes, however the size of the non polar section decreases its ability to dissolve in water

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19
Q

Name of molecule thats both polar and non polar

A

Amphipathic

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20
Q

What three diff types of attractions must occur for something to dissolve

A
  • Attraction of solvent to solvent
  • Attraction of solvent to solute
  • Attraction of solute to solute
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21
Q

To dissolve 1 substance in another three things must occur:

A

forces holding solute particles together must break

forces holding solvent particles break

attractions between solvent and solute must form

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22
Q

What factors affect rate of dissolving

A

1) solubility
2) temperature
3) surface area
4) stirring

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23
Q

how does solubility affect dissolving rate

A

things that are more soluble will disolve faster than those less soluble

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24
Q

how does temperature affect dissolving rate

A

solid solutes will disolve faster in warmer water
** fast water molcules keep solid suspended

gas solute are less soluble in warm water
** fast moving gas molecules separate from solvent

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25
Q

how does surface area affect dissolving rate

A

when you increase surface are you increase solubility (exposes more solute to solvent)

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26
Q

how does stirring affect dissolving rate

A

dissolves faster because particles are moving faster

27
Q

what is molarity (M)

A

moles solute/1L solution

28
Q

Units of solubility

A

1) g solute/ml solution
2) g solute/ g solutoin
3) PPM: parts per million - typical in gases

29
Q

What is a precipitate

A

a solid that is formed in a chemical reaction

30
Q

What are spectator ions?

A

bystanders!

ions that dont participate in chemical reactions but are still there

31
Q

Example of a precipitation reaction

A

(aq) + (aq) –> (aq) + (s)

32
Q

why does precipitation reactions occur

A

when solute ions are more attracted to eachother than to the solvent molcules they stick together forming clusters (the precipitate)

33
Q

what is a total ionic equation

A

this shows all the things involved in a reaction

34
Q

what is a net ionic equation?

A

an equation that only shows the things that are involved in the solute reaction

35
Q

Steps to precipiate problems:

A

1) identify precipitate
2) find mass of precipitate
3) find concentration of excess ions
4) find concentration of spectator ions

36
Q

what does identifying precipitate entail

A

1) make balanced chemical equation

2) using solubility table find precipitate

37
Q

how to find mass of precipitate:

A

1) write net ionic equation
2) calculate moles of each ion
3) determine the limiting ion by calculating mass of precipitate

38
Q

how to determine the concentration of excess ion

A

1) find moles of ion in excess
2) calculate total volume of solution
3) calculate concentration of excess ions
(moles/volume= Molarity)

39
Q

how to determine the concentration of the spectator ions

A

1) calculate moles of each spectator ion in solution
2) calciulate concentration of the spectator ions (moles/volume=Molarity)

40
Q

All solutions have the qualities that they do because of 3 properties:

A

1) molecular structure
2) pressure
3) temperature

41
Q

what is molality (m)?

A

mol solute/kg solvent (mol/kg)

42
Q

What is mass precent

A

mass solute/mass solution * 100%

43
Q

Why does pop go flat faster on the counter than in fridge

A

it will have greater solubility in cooler temp therefore on counter the co2 will want to escape faster

44
Q

what order should you add acid and water

A

always add acid to water

45
Q

What is a saturated solution?

A

A solution that has dissolved as much solute as it can therefore if you add more it will not be dissolved

46
Q

what is a super-saturated solution

A

a solution that has more dissolved solute than there would typically be.

47
Q

What diff is there between an ionic substance dissolving in water and a polar one?

A

Ionic substances dissociate into individual ions whereas polar substances form either dipole dipole or h bonds

48
Q

what is a way to increase solubility in most substances

A

by increasing the pressure and the temp

49
Q

What does dilution involve

A

Adding more solvent into a solution

50
Q

What doesnt change during dilution?

A

The number of MOLES!

51
Q

What is the dilution calculation?

A

M1V1=M2V2

52
Q

What is conductivity

A

somethings ability to conduct electricity

53
Q

What are solutions that conduct electricity called?

A

electrolytes

54
Q

Why do some solutions carry electric charge

A

because they have charged particles

55
Q

What are two solutions that have high conductivity?

A

Ionic compounds and strong acids and bases

56
Q

What are solutions that dont conduct electricity called?

A

Nonelectrolytes – No ions are present

57
Q

What is a solution that wont conduct electricity

A

polar covalent compounds

Ex: ethanol and water

58
Q

What are colligative properties

A

These are things that only rely on the concentration of the solute rather than what the solute actually is

59
Q

name two colligative properties

A

1) Boiling point elevation
- adding solute to water increases boiling point
2) Freezing point depression
- adding solute to water decreases freezing point

60
Q

Which of the following would melt ice the best?
C6H12O6
NaCl
CaCl2

A

CaCl1 because it has most particles when dissolved

61
Q

What is titration

A

Titration is a process used to determine the concentration of an unknown solution

62
Q

How does titration work?

A

One reacts a measured amount with a known concentration until their concentrations are equal!

63
Q

When is titration commonly used?

A

During neutralization reactions to know the concentration of an acid or base

64
Q

How to do acid based titration

A

1) In Erlenmeyer flask put the accuratly measured unknown concentration
2) The solution you know put in a burette
3) Add indicator to unknown solution
4) Add known solution until reaction is complete
5) Using known solution calculate unknown concentration

Chemistry (6 decks)

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