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Chemistry 11 + 12 > FINAL 11 EXAM FINALLY DONE WITH CHEM > Flashcards

FINAL 11 EXAM FINALLY DONE WITH CHEM Flashcards

:O (69 cards)

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1
Q

Mole Ratio

A

ratio between the amount of moles of any two compounds involved in a chemical reaction

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2
Q

Excess reactant

A

the reactant is left after the reaction has stopped, not all reactants have been consumed in reactions

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3
Q

Limiting reactant

A

the reactant runs out first in a reaction, limits product formed

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4
Q

Mol Ratio equation steps

A
  • write balanced equation
  • write variable values under equation
  • calculate number of known moles using n = m/M
  • find the number of unknown moles using mole ratios
  • Calculate mass of unknown using the formula m = n x M
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5
Q

Aliquot

A

small measured amount of homogenous liquid that is added to a solution of unknown concentration

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6
Q

Titre

A

total volume of solution delivered by burette to reach endpoint

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7
Q

Equivalence

A

the point in which the reaction occurs (neutralisation/titration occurs)

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8
Q

Endpoint

A

the point in which a change in colour is observed that indicates titration is complete

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9
Q

PH Curve

A

also called a titration curve, a group showing the pH change during titration, x-axis volume of titrant, y-axis pH of solution

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10
Q

Concordant

A

when the volume of two or more titres are similar in quantity

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11
Q

Meniscus

A

the curve seen at the top of a liquid in response to its container

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12
Q

Volumetric flask

A

used to prepare standard solution

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13
Q

Pipette

A

(used to accurately measure aliquot)

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14
Q

Burette

A

used to accurately measure known volumes of solution known as titre

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15
Q

Volumetric analysis steps

A
  • write a balanced equation
  • write variables
  • calculate known moles using n = CV
  • use mole ratio o find unknown moles
  • calculate the unknown concentration using C = n/V
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16
Q

Strong acid

A

readily donates a proton

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17
Q

Weak acid

A

partially donates a proton

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18
Q

Acid

A

donates a proton

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19
Q

Base

A

accepts/retrieves a proton

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20
Q

Neutral

A

equal OH- and H+

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21
Q

pH

A

measure of acidity produced of H

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22
Q

Colorimetry colours absorbed vs colour of sample solution
(I don’t know if you need to learn this)

A

violet - green/yellow
violet/blue - yellow
blue - orange

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23
Q

Calibration curve x and y axis

A

x - Concentration
y - Absorbance

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24
Q

Oxidation reaction

A

a substance loses electrons

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25
Reduction reaction
a substance gains electrons
26
Reducing agent
a substance that loses electrons and causes reduction
27
Oxidising agents
a substance that gains electrons and causes oxidation
28
Metal reactivity series
a list of metals ordered by their ability to react with acids
29
Standard electrode potential
measure of the tendency of a half-reaction to gain electrons (get reduced)
30
OIL RIG
oxidation is loss reduction is gain
31
Half equation electrons
reduction - electron on left side oxidation - electron on right side
32
Potable
water that is safe enough to drink
33
Hydrogen bonding
when hydrogen bonds with either oxygen, nitrogen or fluorine (H-NOF)
34
Polar
significant differences in the electronegative between two or more atoms
35
Dispersion forces
the temporary force when shared electrons are unbalanced
36
Specific heat capacity
the quantity of energy needed to increase the temperature of a certain amount of substance by 1 degree Celsius
37
Specific heat capacity formula
Q=mcΔT Q = heat energy (J) m = mass(g) c = specific heat capacity ΔT = change in temperature (degrees C)
38
What is the specific heat capacity of water?
4.18
39
Density
how much space a substance takes up in volume compared to mass
40
Is ice or water more dense and why?
water is more dense as ice forms a hexagonal pattern that takes up more space this allows ice to float in water
41
Latent heat of vaporisation
heat energy required to change 1 mole of substance from liquid to gas
42
Latent heat of fusion
heat energy required to change 1 mole of substance from solids to liquid
43
Latent heat formula
Q = mL m - mass (kg) L - specific latent heat value (kg/mol)
44
Amphiprotic substance
a substance that can act as both an acid and a base, for example water
45
Polyprotic
acid that can donate more than 1 proton
46
General neutralisation equation equation
acid + base -> salt + water
47
General acid and metal hydroxide
acid + metal hydroxide -> salt + water
48
General acid and metal carbonate equation
acid + metal carbonate -> salt + water + carbon dioxide
49
Ionic product formula
Kw = [H3O+] x [OH-] = 1.0 x 10*(-14) x M*(2)
50
PH formula
pH = -log10[H3O+]
51
Concentration of acid formula
H3O+ = (10*(-14))/(OH-)
52
Concentration of base formula
OH- = (10*(-14))/(HO3+)
53
Concentration of neutral formula
OH- = H+ = 10*(-7) x M
54
Indicator
when a substance changes colour due to a pH change
55
Alkalinity
ability to neutralise an acid
56
Ppm to g/L formula
ppm = (g/L) x 10*(3)
57
Density formula
density = mass/volume
58
Salinity
dissolved salt content of a body of water
59
Celsius to Kelvin
273 Celsius = 0 Kelvin
60
Gas equation formula
PV=nRT P = pressure (kPa) V = volume (L) n = number of mols (mol) R = 8.31 T = temperature (K)
61
Pa to kPa to atm conversion
100 000 Pa = 100 kPa = 0.987 atm
62
3 Mole formulas
n = N/NA n = m/M c = n/v
63
Dilution formula
C1 x V1 = C2 x V2
64
Unsaturated
a solution that contains less solute than is needed to make the solution saturated
65
Saturated
a solution in which no more solute can be dissolved
66
Supersaturated
an unstable solution that contains more dissolved solute than a saturated solution
67
Anode
part in galvanic cell where oxidation occurs
68
Cathode
part in galvanic cell where reduction occurs
69
Displacement reaction
when an atom or atoms are displaced by one another (oxidation and reduction occurs), top is reduced and bottom is oxidised

Chemistry 11 + 12 (15 decks)

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