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

FINAL 11 EXAM FINALLY DONE WITH CHEM Flashcards

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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
Q

Reduction reaction

A

a substance gains electrons

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26
Q

Reducing agent

A

a substance that loses electrons and causes reduction

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27
Q

Oxidising agents

A

a substance that gains electrons and causes oxidation

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28
Q

Metal reactivity series

A

a list of metals ordered by their ability to react with acids

29
Q

Standard electrode potential

A

measure of the tendency of a half-reaction to gain electrons (get reduced)

30
Q

OIL RIG

A

oxidation is loss reduction is gain

31
Q

Half equation electrons

A

reduction - electron on left side
oxidation - electron on right side

32
Q

Potable

A

water that is safe enough to drink

33
Q

Hydrogen bonding

A

when hydrogen bonds with either oxygen, nitrogen or fluorine (H-NOF)

34
Q

Polar

A

significant differences in the electronegative between two or more atoms

35
Q

Dispersion forces

A

the temporary force when shared electrons are unbalanced

36
Q

Specific heat capacity

A

the quantity of energy needed to increase the temperature of a certain amount of substance by 1 degree Celsius

37
Q

Specific heat capacity formula

A

Q=mcΔT

Q = heat energy (J)
m = mass(g)
c = specific heat capacity
ΔT = change in temperature (degrees C)

38
Q

What is the specific heat capacity of water?

A

4.18

39
Q

Density

A

how much space a substance takes up in volume compared to mass

40
Q

Is ice or water more dense and why?

A

water is more dense as ice forms a hexagonal pattern that takes up more space
this allows ice to float in water

41
Q

Latent heat of vaporisation

A

heat energy required to change 1 mole of substance from liquid to gas

42
Q

Latent heat of fusion

A

heat energy required to change 1 mole of substance from solids to liquid

43
Q

Latent heat formula

A

Q = mL

m - mass (kg)
L - specific latent heat value (kg/mol)

44
Q

Amphiprotic substance

A

a substance that can act as both an acid and a base, for example water

45
Q

Polyprotic

A

acid that can donate more than 1 proton

46
Q

General neutralisation equation
equation

A

acid + base -> salt + water

47
Q

General acid and metal hydroxide

A

acid + metal hydroxide -> salt + water

48
Q

General acid and metal carbonate equation

A

acid + metal carbonate -> salt + water + carbon dioxide

49
Q

Ionic product formula

A

Kw = [H3O+] x [OH-] = 1.0 x 10(-14) x M(2)

50
Q

PH formula

A

pH = -log10[H3O+]

51
Q

Concentration of acid formula

A

H3O+ = (10*(-14))/(OH-)

52
Q

Concentration of base formula

A

OH- = (10*(-14))/(HO3+)

53
Q

Concentration of neutral formula

A

OH- = H+ = 10*(-7) x M

54
Q

Indicator

A

when a substance changes colour due to a pH change

55
Q

Alkalinity

A

ability to neutralise an acid

56
Q

Ppm to g/L formula

A

ppm = (g/L) x 10*(3)

57
Q

Density formula

A

density = mass/volume

58
Q

Salinity

A

dissolved salt content of a body of water

59
Q

Celsius to Kelvin

A

273 Celsius = 0 Kelvin

60
Q

Gas equation formula

A

PV=nRT

P = pressure (kPa)
V = volume (L)
n = number of mols (mol)
R = 8.31
T = temperature (K)

61
Q

Pa to kPa to atm conversion

A

100 000 Pa = 100 kPa = 0.987 atm

62
Q

3 Mole formulas

A

n = N/NA
n = m/M
c = n/v

63
Q

Dilution formula

A

C1 x V1 = C2 x V2

64
Q

Unsaturated

A

a solution that contains less solute than is needed to make the solution saturated

65
Q

Saturated

A

a solution in which no more solute can be dissolved

66
Q

Supersaturated

A

an unstable solution that contains more dissolved solute than a saturated solution

67
Q

Anode

A

part in galvanic cell where oxidation occurs

68
Q

Cathode

A

part in galvanic cell where reduction occurs

69
Q

Displacement reaction

A

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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