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A IB Chemistry SL > 8,9 - Acids & Base, Redox > Flashcards

8,9 - Acids & Base, Redox Flashcards

1
Q

oxidation number of elements (eg.O2, Cl2, N2)

A

0

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2
Q

oxidation number of ions (eg.Zn2+, Cl-)

A

same as their charge

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3
Q

G1 metals have oxidation state of

A

+1

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4
Q

G2 metals have oxidation state of

A

+2

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5
Q

O has oxidation state of

A

-2

except in peroxides (e.g. H2O2), where it is −1

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6
Q

H has oxidation state of

A

+1

except in certain metal hydrides (e.g. NaH), where it is −1

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7
Q

F and Cl have oxidation state of

A

-1

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8
Q

the sum of oxidation number in a compound is

A

0

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9
Q

in a compound/ion, the negative oxidation number is always given to

A

the more electronegative element

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10
Q

oxidizing agent

A

gets reduced (gains electrons)
= ox.no. decrease

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11
Q

reducing agent

A

gets oxidized (lose electrons)
= ox.no. increases

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12
Q

transition metals are characterized by

A

having variable oxidation states

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13
Q

more reactive metals act as

A

reducing agents (get oxidized, lose electrons to less reactive metal ions)

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14
Q

more reactive metals can do what to less reactive metals?

A

displace less reactive metals from their compounds (more reactive metals like to be in ion form!)

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15
Q

In redox titrations, an ____ is titrated against a ____

A

oxidizing agent
is titrated against
reducing agent

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16
Q

How is endpoint indicated in the Manganate(VII) Titrations?

A

purple color disappears

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17
Q

How is endpoint indicated in the **Iodine-Thiosulfate ** Titrations?

A
  1. light brown of the iodine turns paler as it is converted to colorless iodide ions
  2. add starch to clarify endpoint → blue/black
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18
Q

The Winkler Method is used to measure

A

concentration of dissolved oxygen in freshwater systems

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19
Q

Voltaic cells: what materials should the external connection and salt bridge be made of? why?

A
  • external: metallic wire; to allow electron to flow
  • salt bridge: aqueous electrolyte; to allow ions to flow
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20
Q

Electrolysis happens when

A

flow of current causes ionic compound to split up and form new substances

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21
Q

applications of electrolysis

A
  • purifying copper
  • plating metals with silver/gold
  • extracting reactive metals (eg. Al)
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22
Q

electrolyte is

A

the substance passed by current and splits up

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23
Q

What happens to ions during electrolysis?

A
  • -ions move to the anode → lose e-
  • +ions move to the cathode → gain e-
  • Electrically neutral molecules are released
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24
Q

how is current conducted in an electrolytic cell?

A
  • e- move by external circuit
  • ions move through the electrolyte
25
**ox**idation always occurs at the
**an**ode
26
**red**uction always occurs at the
**cat**hode
27
Brønsted-Lowry acid
proton donor
28
Brønsted-Lowry base
proton accepter
29
conjugate acid-base pair
two species **different by a H+ ion** eg. H2O and H3O+
30
a strong acid always has a
weak conjugate base
31
amphiprotic vs amphoteric
amphi**pro**tic: can act both as **proton** donors and acceptors amphoteric: can act as both acid and base all amphiprotic are amphoteric, but not all amphoteric are amphiprotic (eg. Al2O3)
32
acid + metal →
salt + H
33
acid + metal oxide →
salt + H2O
34
acid + metal hydroxide →
salt + H2O
35
acid + metal carbonate →
salt + water + CO2
36
acid + base →
salt + water
37
How can you compare the strength of acids?
1. **pH value** 2. **Reactivity**: put the same metal into same concentration of different acid solutions - stronger acids have a higher H+ concentration thus will **react more vigorously with metals** than weak acids. This can be seen as: more effervescence, more exothermic, metal dissolves faster... 3. **Electrical conductivity**: stronger acid has a higher H+ concentration → **conducts electricity better**
38
describe the color of **litmus** indicator
acid = pink base = blue
39
describe the color of **methyl orange** indicator
acid = red base = yellow
40
describe the color of **phenophthalein** indicator
acid = colorless base = pink
41
pH
measures the **concentration of H+ ions** pH = **-log [H+]**
42
10.0 cm3 of nitric acid solution of pH = 1.0 is mixed with 990.0 cm3 of distilled water. What is the pH of the final solution?
volume increase by a factor of 10^2 (from 10 to 1000) → concentration decrease by a factor of 10^2 → pH increase by 2 units
43
a change by 1 pH unit =
a change by 10-fold in H+
44
Kw =
[H+] [OH-]
45
Determine the pH of a solution made by dissolving 5.00 g of KOH in 250 cm3 of distilled water.
1. **[KOH] = [OH-] =** (5/56.1)/0.25 = 0.357 mol/dm3 2. **[H+] = Kw/[OH-] =** 1x10-14/0.357 = 2.8x10-14 3. **pH = -log[H+] =** 13.55
46
strong acid
**completely dissociates** in aqueous solutions; **irreversible** reaction as the equilibrium position is far over to the right
47
weak acid
**partially dissociates** in aqueous solutions; **reversible** reaction as the equilibrium position more over to the left
48
examples of strong acid
基本常见的都是: **HCl, HNO3, H2SO4**
49
examples of weak acid
most **organic acids**, HCN, H2S,H2CO3
50
examples of strong base
**G1 metal hydroxides**
51
examples of weak base
**NH3, amines,** some transition metal hydroxides
52
HCl → **H+** + Cl- can also be written as
HCl + **H2O** → **H3O+** + Cl-
53
acid rain
rain with a pH below **5.6**
54
Rain is naturally acidic because
**dissolved CO2** in the atmosphere form **carbonic acid** H2O (l) + CO2 (g) ⇌ H2CO3 (aq)
55
acid deposition - sulfur
from burning fossil fuel... 1. S + O2 → **SO2** 2. SO2 + O2 → **SO3** 3. SO2 + H2O → **H2SO3** SO3 + H2O → **H2SO4**
56
acid deposition - nitrogen
from internal combustion engine... 1. N2 + O2 → **NO** 2. NO + O2 → **NO2** 3. NO2 + H2O → HNO2 + **HNO3**
57
effects of acid rain
* **corrosion of limestone buildings**: CaCO3 + H2SO4 → CaSO4 + CO2 + H2O CaCO3 + 2HNO3 → Ca(NO3)2 + CO2 + H2O * **important ions leach from soil** → plants die, eutrophication (excessive algal growth that results in oxygen depletion)
58
methods to reduce SO2 emission
pre-combustion: * use renewable energy sources or fuel with less sulfur content * sulfur is removed by **reacting with hydrogen** (hydrodesulfurization) → make H2SO4 post-combustion: * pass waste gases through a **wet slurry of CaO and CaCO3**, which react with the SO2 and produce CaSO4 → make plaster

A IB Chemistry SL (9 decks)

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