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Unit 2 Chem > REDOX > Flashcards

REDOX Flashcards

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1
Q

Reduction

A

The gaining of electrons

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2
Q

Oxidation

A

The loss of electrons

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3
Q

Oxidant

A

Gains electrons

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4
Q

Reductant

A

Loses electrons

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5
Q

Eg of Reduction (Including Oxidant)

A

Cu 2+ (aq) + 2e- -> cu (s) Cu 2+ is oxidant

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6
Q

Eg of Oxidant (Including Reductant)

A

Fe (S) -> Fe 2+ (aq) + 3e- Fe is reductant

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7
Q

Electrolyte

A

Solutions that allows ion movments

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8
Q

Anode

A

A Postive Electrode

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9
Q

Cathode

A

A negative Electrode

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10
Q

3 types of observations which may be made to indicate that a spontaneous redox reaction has occured

A

Bubbles at electrode
Colour Change
Deposit of metal on electrode

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11
Q

Conjugate redox pairs (ZN as a reductant)

A

Zn2+

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12
Q

Conjugate redox pairs (Fe2+ as a reductant)

A

Fe3+

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13
Q

Would it be sensible to store copper (II) sulfate in an iron tank?

A

Cu 2+ (aq) + Fe -> Cu (s) + Fe 2+
Cu 2+ is the strongest oxidant and Fe is the strongest reductant. Fe will decompose into Fe 2+ allowing cu2+ to break out. It would not be sensible

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14
Q

Conjugate of bases

A

loses Hydrogen atoms

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15
Q

Conjugate of Acids

A

gains Hydrogen atoms

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16
Q

Amphiprotic

A

Able to act as both an acid and base

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17
Q

What is a weak/ Tiprotic acid?

A

When its weak it means that it does not release H+ readily and Triprotic means that it is ready to donate 3H+ from the substance.

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18
Q

State the Bronsted- Lowry definitions of both an acid and base.

A

Acids donate Protons and base accepts protons

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19
Q

What is it meant by a strong acid

A

Low on the Ph scale and they are more ready to donate protons. They also have high amount of H+ atoms. eg h2so4

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20
Q

What is it meant by a strong base

A

Higher Ph and are more ready to accept protons. and with more OH-. eg is Nacl2

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21
Q

Show that H3PO4 is polyprotic

A

H3Po4+ H2o -> H2Po4 + H3O (INCLUDE STATES)

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22
Q

Water has a high surface tension

A

The water molecules attract one another due to the water’s polar property. Insects can walk on the surface of water because of surface tension of water

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23
Q

Water has a high heat of vaporisation.

A

a high input of energy is required to transform one gram of liquid water into water vapor, an energy requirement called the heat of vaporisation

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24
Q

Copper (II) Carbonate crystals are added to dilute sulphuric acid

A

CuCo3 (s) + H2So4 (aq) -> Co2(g) + Cuso4 (aq) + H20 (l)

Co2 bubbles forming would of seen the solution turn blue

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25
Q

Show that a reaction between mg and hcl is a redox equation

A

The Mg reductant is oxidised by H+

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26
Q

Q=mc^T

100 g of water at 25.00 degrees absorbs 100J of heat. What is its final temp?

A

100 divided by (100x 4.18) = 0.24 Degrees

25 degrees plus 0.24 equals 25.2 degrees

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27
Q

Q= mc^T
80g of acetone was heated from 25.5 degrees to 63.4 degrees. how much energy was transferred to the acetone during heating?
SHC of acetone = 2.13jg -1

A

80 x 2.13 x 37.9 = 6458.16 j

= 6.46 KJ of enegry

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28
Q

C=

A

n divided by v

29
Q

Properties of a acid

A

Tastes sour, Molecular in structure, Forms conducting soloutions

30
Q

What is least likely to act as an acid

A

A Structure that has non polar bonds

31
Q

When an alkaline solution with a pH of 8 has a large volue of water added to it , the pH will

A

Fall as the concentration of the OH- ion has decreased

32
Q

Which of the following lists the solutions in order of increasing pH

A

H2sO4, HNo3, Ch3COOH, H2O, NH3, NaOh

33
Q

The pH of 25.0ml of solution of nitric acid (HNo3) is closest to

A

[h3o+] = -log(0.002)

34
Q

Hydrolysis

A

One which a substance reacts with water to form OH- or H3O+ ions.

35
Q

Acid- Base

A

Protons are being donated to OH- Ions

36
Q

Ionisation

A

when a substance reacts with to produce.

37
Q

[ OH-]

A

10^-14 divided by 10^ pH

38
Q

[H30+]

A

M= 9,2x 10^14

M+ -log(9.2x10^-14 =3

39
Q

Why is Ethanoic acid (CH3C00H) Monoprotic even though it has 4 hydrogen atoms

A

Because one hydrogen is in a polar bond which can be donated and 3 are not in a polar bond therefor cannot be donated

40
Q

Equation and observation of MgO powder being added to dilute HCL

A

MgO (s) + 2HCl (aq) -> H2O (l) + Mgcl2 (aq)

The solid powder would disappear

41
Q

the Ph of a 0.010M solution of a strong DIprotic acid will be

A

between 1.7 and 2.0 as the second proton is only partially donated.

  • log(0.01) =2
  • log (0.02) = 1.7
42
Q

Neutralisation

A

The process of an acid reacting with a base. the properties of the acid and base can be cancelled out.

43
Q

Pepitte (Aliquot)

A

used to transfer fixed volume of solution to conical flask. Rinse with solution that it will transfer

44
Q

Conical Flask

A

Receives the aliquot. Add 1-2 drops of indicator. Rinse with distilled water

45
Q

Standard Flask

A

Always used to prepare solution of known concentration.

Rinse with distilled water

46
Q

Burette

A

Delivers variable volume. Rinse with solution that it will contain

47
Q

Polyprotic Acids

A

An acid that can donate more than one proton.

48
Q

Self Ionisation of water

A

Since water can act as both an acid and base, it can also react with itself according to the equation
H2O (l) + H2O (l) -> H3O= + OH-

49
Q

Why is a nuetral solution a pH of 7

A

Because it has an equal amount of [H+] and [OH-] Ions.

50
Q

Dilution: calc volume of

A

0.250x 2.15 Divided by 12

51
Q

Standerd Solution

A

It must have a high state of purity
It must have an accurately known formula
It must be stable

52
Q

Calculate Concentration in gL-1 and mgL-1 for

0.425g Barium Nitrate in 25 ml of solution

A

25 divided by 1000 = 0.055
0.425 divided by 0.055.
= 480gL-1 and or 4.8x10^-14 mgL-1

53
Q

Corrosion

A

Oxidation of metals by materials in their enviroment

54
Q

Dry Corrosion

A

When a metal reacts differently with oxygen. K and Na combine readily with oxygen so they undergo dry corrosion quickly

55
Q

Wet Corrosion rusting

A

When a metal reacts with oxygen in the presence of water. Water can speed up corrosion reactions.
Fe (s) -> Fe 2+ (aq) +2e-

56
Q

Adverse effects of corrosion

A

A severly corroded metal cannot conduct electricity.
Products of corrosion are brittle and flake off.
Metal oxides have less tensile strength.

57
Q

Corrosion Protection

A

Surface Protection
Alloying
Electrochemical Protection

58
Q

Surface Protection + equation

A

A metal surface being prevented from being into contact with oxygen, such as using oil.

59
Q

Alloying + equation

A

Iron can be alloyed with small quantities of metals such as chronium, nickel, manganse to produce stainless steel

60
Q

Electrochemical Protection + equation

A

placing a more reactive metal in a electrical contact with the metal that needs protection

61
Q

Zinc and Copper2+ Displacement reaction

A

When zinc was placed in copper sulfate solution a reaction occurs, causing copper metal to form Zinc.
Zn (s) + Cu2+ (aq) -> Zn2+ (aq) + Cu (s)

62
Q

Concentration dosent determine strength. it is based on

A

the amount of ions and how much acid in the solution

63
Q

Chemical equation of ethonaic acid reacting h20

A

Ch3CooH+ H20 -> Ch3COO- + H30+

64
Q

Nuetralisation equation

A

HCL (aq) + NaOH (aq) -> NaCl (aq) + h20

65
Q

Ionic equation of nuetralisation

A

H3O + (aq) + OH- (aq) - 2H20 (l)

66
Q

Corrosion of Iron

A

2Fe(s) + O2 (g) +2h2o (l) -> 2Fe(OH)2 (s)

67
Q

Copper and Zinc 2+ reaction

A

No reaction would occur. this makes zinc more reactive

68
Q

Calculate pH of solution Ca(OH)2

A

10^-14 divided 0.02 then -log( )

Unit 2 Chem (13 decks)

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