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chem 20 > unti c- topic one > Flashcards

unti c- topic one Flashcards

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1
Q

solution

A

homogenous mixture composed of at least one solvent and on solute

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2
Q

homogenous

A

uniformed all the way through, can’t see what it is made of

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3
Q

hetrogenous

A

can see distinct things inside

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4
Q

solute

A

small quantities, whats being dissolved

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5
Q

solvent

A

larger quantities, whats dissolving

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6
Q

____ dissolves in the _____

A

solute dissolves in the solvent

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7
Q

dissolved

A

doesn’t mean that molecule breaks apart

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8
Q

what does the (aq) mean in NaCl(aq)

A

what the compound is dissolved in

does not mean liquid

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9
Q

aqueous solutions

A

water as the solvent

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10
Q

dissolution

A

the act/process of dissolving

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11
Q

three types of energy in dissolution

A

1) energy required to break bonds in solute
add 2) energy require to break bonds in solvent
take away 3) energy released from bonds between solute and solvent
= total energy

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12
Q

electrolytes

A

compounds that form conducting solutions

example*salt water

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13
Q

non electrolytes

A

compounds that form solutions that don’t conduct electrcity

example*sugar water

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14
Q

litmus

A

tells about charges in pH

red>acid blue>base

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15
Q

neutral molecular

A

-composed all of non-metals
-does not dissosciate in solution
-nonelectrolyte
-red stays red blue stays blue
-always colorless
example*sugar water, methonal

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16
Q

neutral ionic

A

-composed of metal and nonmetla
-does dissosciate in solution
-electrolyte
-red satys red blue stays blue
-can be colored
example*NaCl, MgSO4

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17
Q

attributes of an acid

A

-compound begins with Hydrogen
-ionizes in solution produces hydroxide ions
-electrolyte
-red stays red blue turns red
-can be colored
example*HCl, HNO3

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18
Q

basic

A

-contains hydroxide ion
-ionizes in solution to produce hydroxide ions
-electroltye
-red turns blue blue stays blue
examples*NaOH, Ba(OH)2

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19
Q

what is everything made up of

A

matter

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20
Q

what two categories does matter branch off into

A

pure substances, mixtures

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21
Q

what do pure substances branch off into

A

compounds and elements

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22
Q

what do mixtures branch off into

A

homogenous and hetrogenous

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23
Q

compound

A

can be identified by a single chemical formula

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24
Q

element

A

cannot be broken down into simpler substances

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25
Q

like dissolves in like means

A

nonpoplar does not dissolve in water, since water is a polar

so polar dissolves in water, since water is a polar

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26
Q

dissociation

A

electyolyte dissolves and seperates into component ions

example* Ca(OH)2(aq) –> Ca2+(aq) + 2OH-(aq)

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27
Q

what are acids when pure, verses in water

A

molecular

in water they dissosciate

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28
Q

qualitative

A

physical observation, something you can describe

example*state, color, smell

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29
Q

slective preccipitation

A

to detect if there is an ion in a solution, adding an ion that is not soluable

basically (questionable ion) + (ion that isn’t souluable)

30
Q

filtrate

A

liquid left over in the beaker

31
Q

precipatate

A

solid remaining on filter paper

32
Q

filtration

A

separate precipitate from the liquid

33
Q

molecular compounds DO NOT

A

dissosciate

34
Q

acids/bases are classfied as strong or weak using

A

the chart

35
Q

strong acids

A

dissosciate

36
Q

weak acids

A

do not dissosciate

37
Q

gases and halogens

A

are soluable

38
Q

any other element

A

is not soluable

39
Q

selective precipitation

A

way to figure out what is actually soluable

-type of qualitative analysis

40
Q

how does selective precipitation work

A

getting the intial ion out of the solution

-finding what the intial ion is NOT soluable with

41
Q

solubility means it

A

stays in solution

42
Q

no soluable means it

A

falls out of solution (forms a precipitate)

43
Q

concentration

A

how much of a solvent per given amount of solvent mol/L

eg how many students in a room

44
Q

highly conecntrated

A

lots of solute in smaller solvent

45
Q

concentration depends on

A

volume

46
Q

formula for concentration

A

c=n/v

47
Q

percent by volume formula

A

volume of a solute/volume of solution X 100

48
Q

concentration as a unti

A

mol/L

49
Q

concentration as a percentage (units)

A

mL, g

50
Q

solution - solute

A

=solvent

51
Q

solubility

A

maximum concentration of a solute for that temperature

52
Q

unsaturated

A

has not reached saturation, more solute can dissolve

53
Q

saturation

A

so much solute that it cannot dissolve anymore

54
Q

higher heat means (sol)

A

take in more solute (a higher saturation)

55
Q

supersaturated

A

contains more solute than it can normally hold at a given temperature
-happens by cooling previously hot saturated solution very slowly

56
Q

miscible

A

dissolve many proportions. have no maximum concentration

-is mixable

57
Q

immiscible

A

do not dissolve in water at all, but form a separate layer

-is unmixable

58
Q

halogens + oxygen dissolve well in…

A

water!

-eg marine life need certain oxygen levels in lakes to survive

59
Q

open system

A

ambient enviroment has an effect on whats going on in the system
-matter+energy can enter and leave

60
Q

closed system

A

surrounding enviroment has no effect
-energy can enter+leave
-matter cannot enter + leave
eg- closing a bottle traps substance inside but doesn’t secure temperature or pressure

61
Q

equilibrium

A

closed system where all measurable properties are constant

62
Q

dynamic quilibrium

A

constant switching between being dissosciated and reassosciating ions, forward + backwards
-but is still equal

63
Q

solubility curve

A

graphical representation of a certain substance over temperature range
-physical property

64
Q

volumetric flask

A

very accurate beaker, used to easily ensure the amount of the solution, since measurement is in neck

65
Q

(solubility of ___ water) solids

A

solubility increases as temperature increases

-solublity is not affected by pressure changes

66
Q

(solubility of ___ water) liquids

A

difficult to generalize

  • solubility is not affected by temperatures
  • solubility is not affected by pressure
67
Q

(solubility of ___ water) gas

A

solubility decreases as temperature increases

-solubility increases as pressure increases

68
Q

preperation of a standard solution

A

rough steps

  1. weigh out needed amount of substance (in grams)
  2. dissolve substance in half of given water
  3. pour dissolved substance into volumetric beaker and then rinse other beaker out several times
  4. then fill with rest of water and mix in slowly with volumetric beaker
  5. transfer solution to bottle and lable
69
Q

dillution

A

taking a solution of higher concentration, and making it of lower concentration- by adding more solvent

70
Q

the amount of solute is (dillution)

A

unchanged

-orignal number of moles stays the same

71
Q

formula for dilluting

A

c1v1=c2v2

chem 20 (7 decks)

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