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chem 20 > unti c- topic one > Flashcards

unti c- topic one Flashcards

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
like dissolves in like means
nonpoplar does not dissolve in water, since water is a polar so polar dissolves in water, since water is a polar
26
dissociation
electyolyte dissolves and seperates into component ions | example* Ca(OH)2(aq) --> Ca2+(aq) + 2OH-(aq)
27
what are acids when pure, verses in water
molecular | in water they dissosciate
28
qualitative
physical observation, something you can describe | example*state, color, smell
29
slective preccipitation
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
filtrate
liquid left over in the beaker
31
precipatate
solid remaining on filter paper
32
filtration
separate precipitate from the liquid
33
molecular compounds DO NOT
dissosciate
34
acids/bases are classfied as strong or weak using
the chart
35
strong acids
dissosciate
36
weak acids
do not dissosciate
37
gases and halogens
are soluable
38
any other element
is not soluable
39
selective precipitation
way to figure out what is actually soluable | -type of qualitative analysis
40
how does selective precipitation work
getting the intial ion out of the solution | -finding what the intial ion is NOT soluable with
41
solubility means it
stays in solution
42
no soluable means it
falls out of solution (forms a precipitate)
43
concentration
how much of a solvent per given amount of solvent mol/L | eg how many students in a room
44
highly conecntrated
lots of solute in smaller solvent
45
concentration depends on
volume
46
formula for concentration
c=n/v
47
percent by volume formula
volume of a solute/volume of solution X 100
48
concentration as a unti
mol/L
49
concentration as a percentage (units)
mL, g
50
solution - solute
=solvent
51
solubility
maximum concentration of a solute for that temperature
52
unsaturated
has not reached saturation, more solute can dissolve
53
saturation
so much solute that it cannot dissolve anymore
54
higher heat means (sol)
take in more solute (a higher saturation)
55
supersaturated
contains more solute than it can normally hold at a given temperature -happens by cooling previously hot saturated solution very slowly
56
miscible
dissolve many proportions. have no maximum concentration | -is mixable
57
immiscible
do not dissolve in water at all, but form a separate layer | -is unmixable
58
halogens + oxygen dissolve well in...
water! | -eg marine life need certain oxygen levels in lakes to survive
59
open system
ambient enviroment has an effect on whats going on in the system -matter+energy can enter and leave
60
closed system
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
equilibrium
closed system where all measurable properties are constant
62
dynamic quilibrium
constant switching between being dissosciated and reassosciating ions, forward + backwards -but is still equal
63
solubility curve
graphical representation of a certain substance over temperature range -physical property
64
volumetric flask
very accurate beaker, used to easily ensure the amount of the solution, since measurement is in neck
65
(solubility of ___ water) solids
solubility increases as temperature increases | -solublity is not affected by pressure changes
66
(solubility of ___ water) liquids
difficult to generalize - solubility is not affected by temperatures - solubility is not affected by pressure
67
(solubility of ___ water) gas
solubility decreases as temperature increases | -solubility increases as pressure increases
68
preperation of a standard solution
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
dillution
taking a solution of higher concentration, and making it of lower concentration- by adding more solvent
70
the amount of solute is (dillution)
unchanged | -orignal number of moles stays the same
71
formula for dilluting
c1v1=c2v2

chem 20 (7 decks)

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