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M2:Chapter 4=> Acids And Redox > 4.1-4.3 > Flashcards

4.1-4.3 Flashcards

1
Q

What is the Bronsted- Lowry definition of an acid

A
  • proton donors
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2
Q

What is the Bronsted- Lowry definition of a base

A
  • proton acceptors
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3
Q

When acids and bases react with water what do they form

A
  • a reversible reaction
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4
Q

What are alkalis

A
  • soluble bases that release OH- ions in aqueous solution
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5
Q

What do acids release in aqueous solutions

A
  • H+ ions
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6
Q

What do bases release in aqueous solutions

A
  • OH- ions
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7
Q

What do strong acids do

A
  • completely dissociate when dissolved in water
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8
Q

What do weak acids do

A
  • partially dissociate when dissolved in water, giving an equilibrium mixture
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9
Q

Give 3 examples of strong acids

A

1) Hydrochloric acid (HCl)
2) Sulfuric acid (H2SO4)
3) Nitric acid (HNO3)

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10
Q

Give 2 examples of a weak acids

A

1) Ethanoic acid ( CH3COOH)
2) And any other carboxylic acids

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11
Q

Give two examples of strong bases

A

1) NaOH
2) KOH

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12
Q

Give an example of a weak base

A
  • Aqueous ammonia (NH3)
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13
Q

Define polyprotic acids

A
  • an acids that can donate more than one proton
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14
Q

How many H+ ions will a monoprotic acid donate

A
  • 1 mole of H+ ions
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15
Q

How many H+ ions will a diprotic acid donate

A
  • 2 moles of H+ ions
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16
Q

How many H+ ions will a triprotic acid donate

A
  • 3 moles of H+ ions
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17
Q

What is a neutralisation reaction

A
  • a reaction where an alkali and base are reacted together to form a salt and water
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18
Q

What products are formed when you react an acid with a carbonate

A

Salt + water + carbon dioxide

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19
Q

When ammonia reacts with acids what isn’t formed

A
  • water
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20
Q

How does ammonia produce OH- ions

A
  • rectas with water first and accepts a proton to produce ammonium ions and OH- ions

E.g:
NH3(aq) + H2O(l) <=> NH4+(aq) + OH-(aq)

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21
Q

What is the equation for metals reacting with acids

A

Metal + Acid —> Salt + Hydrogen

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22
Q

What is the equation for metal oxides reacting with acids

A

Metal oxide + Acid —> Salt + Water

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23
Q

What is the equation for metal hydroxides reacting with acids

A

Metal Hydroxide + Acid —> Salt + Water

24
Q

What are titrations used for

A
  • to work out the concentration of an acid or alkali
25
Q

Briefly summaries what happens during titration

A

1) you have an acid or alkali in a burette with a known concetration
2) you also have an acid or alkali with an unknown concentration but known volume in the conical flask
3) you add a few drops of indicator (usually phenolphthalein)
4) you turn the knob of the burette horizontally to open it and the chemical will drop into the conical flask until the indicator changes colour (end point)

26
Q

How do you read how much chemical was added from the burette

A
  • by reading from the bottom of the meniscus
27
Q

How many decimal places do you always record everything in when doing a titration

A
  • 2 decimal places
28
Q

Which results do you look at when working out your average titration

A
  • the two concordant results (results within 0.10cm^3 of each other)
29
Q

When using phenolphthalein when the acids is in the conical flask what does it change to

A
  • Colourless
30
Q

When using phenolphthalein when the alkali is in the conical flask what does it change to

A
  • pink
31
Q

When using methyl orange when the acids is in the conical flask what does it change to

A
  • yellow
32
Q

When using methyl orange when the alkali is in the conical flask what does it change to

A
  • red
33
Q

What are standard solutions

A
  • solutions that are used in titration, they have a known concentration
34
Q

How do you make a standard solution

A

1) WEIGH: weigh out the amount of solid precisely using a balance and a plastic weighing boat
2) TRANSFER: transfer the solid from the weighing boat to a beaker. Wash any solid left behind into the beaker using deionised water
3) DISSOLVE: dissolve solid fully using deionised water. Stir to ensure the solid is dissolved fully
4) TRANSFER: transfer solution to volumetric flask. Use a funnel to avoid spillage and rinse the beaker and glass rod into the flaks to ensure most of the solution is transferred
5) FILL: use more deionised water to fill to the graduation line
6) MIX: invert the flask a few times to ensure your solution is thoroughly mixed

35
Q

Standard solution calculations:
What mass of solid NaOH is required to make 250cm^3 of 0.75moldm^-3 NaOH solution?

A

Mass= 7.5g

36
Q

Titration Calculation:
18.3cm^3 of 0.25moldm^-3 HCl was required to neutralise 25cm^3 of KOH. Calculate the concentration of KOH.

A

0.18moldm^-3

37
Q

Titration calculation:
15.7cm^3 of 0.450moldm^-3 H2SO4 was required to neutralise 0.120moldm^-3 of NaOH. Calculate the volume of NaOH being neutralised in cm^3

A

Volume = 117.75cm^3

38
Q

What is the value of uncertainty of a burette

A

+/- 0.10cm^3 because each uncertainty is +/- 0.05cm^3 but as you read the burette twice you multiple that value by 2

39
Q

What is the equation for percentage uncertainty

A

+ / - uncertainty
———————————— X 100
Measurements value

40
Q

Suggests two ways to lower the percentage uncertainty in the measurement of mass

A

1) use more accurate balance eg to 3dp instead of 2dp
2) measure a greater mass

41
Q

When are electrons transferred

A
  • when reduction and oxidation occurs
42
Q

What does the acronym OIL RIG stand for

A

Oxidation is Loss (of electrons)
Reduction is Gain (of electrons)

43
Q

Explain this REDOX reaction and identify what is being reduced and what is being oxidised
Ca + 1/2 O2 —> CaO

A

Ca is oxidised:
Ca —> Ca2+ + 2e-

O is reduced:
1/2 O2 + 2e- —> O2-

44
Q

What is a reducing agent

A
  • an element that looses electrons and are oxidised themselves
45
Q

What is an oxidising agent

A
  • an element that gains electron and are reduced themselves
46
Q

What is the oxidation number of uncombined elements like CL2, O2 or Fe

A
  • 0
47
Q

When is the oxidation number of Chlorine positive

A
  • in compounds with F and O like ClF3
48
Q

When is oxygen’s oxidation number -1

A
  • in peroxides (H2O2)
49
Q

When is oxygen’s oxidation number +2

A
  • in OF2
50
Q

What is oxidation number of N in NH3

A

-3

51
Q

What is the oxidation number of S in H2S

A

-2

52
Q

What is the oxidation number of S in SO4 2-

A

+6

53
Q

What is the oxidation number of Fe in Fe2O3

A

+3

54
Q

What is the oxidation number of V in VO2+

A

+4

55
Q

Are metals oxidised or reduced when they react with acids

A
  • oxidised

M2:Chapter 4=> Acids And Redox (1 decks)

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