Chapter 4 - Acids and REDOX Flashcards

1
Q

all acids contain what?

A

hydrogen in their formulae

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2
Q

when dissolved in water, acids release ?

A

hydrogen ions as protons - H (^+)

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3
Q

strong acid def

A

releases all hydrogen atoms into solution as H plus ions and COMPLETELY DISSOCIATES in aqueous solutuion

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4
Q

weak acid def?

A

only releases a small proportion of its available H atoms into solution as H plus ions. PARTIALLY DISSOCIATES in aqueous sol

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5
Q

weak acid have ?

A

a forwards/ backwards arrow (equilibrium sign) which indicates that the forwards reaction is incomplete

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6
Q

most organic acids, like ethanoic acid are ____ acids

A

weak

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7
Q

a base…

A

neutralises an acid to form a salt

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8
Q

what is an alkali?

A

a base that dissolves in water realising hydroxide ions into the solution

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9
Q

how do strong acids containing more than one H atom behave?

A

strong acid for only one H atom

next H acts as weak acid

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10
Q

What is a titration?

A

a technique used to accurately measure the volume of one solution that reacts exactly with another solution

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11
Q

what can titrations be used for?

A
  • finding the conc of a solution
  • identification of unknown chemicals
  • finding the purity of a substance
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12
Q

burette readings always have ___ decimal places

A

2 - with the last place being either 0 or 5

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13
Q

concordant results

A

are within 0.1cm (^3) of each other

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14
Q

acids are?

A

proton donors bc they donate H(+) ions to bases

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15
Q

ammonia is a ?

A

weak base and forms a weakly alkaline solution when dissolved in water

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16
Q

strength of acids - what is strength?

A

a measure of dissociation

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17
Q

a strong acid easily gives up ?

A

protons, but a weak acid does not easily give up protons

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18
Q

strong base definition

A

is fully ionic.

100% splits up into metal ions and hydroxide ions in solution

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19
Q

weak base definition

A

doesn’t convert fully into hydroxide ions in solution

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20
Q

in neutralisation, the h(+) ion is replaced by?

A

a metal ion or any other + ion

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21
Q

interesting cases - acidic salts?

A
  • formed from polyprotic acids

e. g. salts of sulphuric acid

22
Q

what is a polyprotic acid?

A
  • an acid that dissociates more than once - it donates more than 1 proton
23
Q

interesting cases - ammonium salts?

A
  • formed when acids are neutralised by aqueous ammonia

- salts formed contain the NH four (+) ion

24
Q

Explain how OH minus acts as a base?

A

the Oh minus ion accepts a proton

25
explain why Kcl can be referred to as a salt?
the H plus ion in Hcl has been replaced by a metal ion
26
Common acids and their uses?
Hcl - stomach acid Sulphuric acid - car batteries Nitric acid - fertiliser
27
Bases are _____, _______, ________
Oxides, hydroxides and carbonates of metals
28
When converting into ionic equations,
Discount unchanged ions as tgesd re spectator ions
29
2 H[^+] + 2 OH [^-]
-> 2H (two) 0
30
Solute definition
The solid that is being dissolved
31
Solvent definition
The liquid that the solute is dissolved in
32
Solution definition
A mixture of the solute and solvent
33
How many sig figures?
Usually 3sf but look at data and use smallest amount as if bigger no. Of sig figs, you're saying your data is more accurate
34
Scaling equation?
Moles × (volume scaling to / volume we have)
35
oxidation can occur both in terms of ____ and ______
oxxygen, electrons
36
oxidation (oxygen)?
gain of oxygen
37
reduction (oxygen)?
loss of oxygen
38
oxidation (electrons)?
loss of electrons
39
reduction (electons)?
gain of electron s | OIL RIG
40
roman numerals are used to?
represent the oxidation state pf an element | espec. important when element has more than 1 possible oxidation no.
41
what can have more than one possible oxidation number?
- Transition elements - Oxyanions - end in ATE, composed of an element and oxygen - e.g. nitrate
42
what is a redox reaction?
a reaction where both oxidation and reduction are occurring in the same reaction
43
oxidation is an _____ in oxidation number
increase
44
reduction is a _____ in oxidation number
decrease
45
disproportionation reduction?
reactions where the same elements are both oxidised and reduced
46
oxidation rules - elements?
oxdiation state of element = 0
47
oxidation rules - monatomic ions?
have lost or gained electrons
48
oxidation rules - hydrogen?
is +1 except in hydrides
49
oxidation rules- bonds in a molecule between the same element?
IGNORE
50
oxidation rules - oxygen?
-2 except in peroxides (a compound containing two oxygen atoms bonded together in its molecule or as the anion O22−) and if bonded to fluorine
51
oxidation rules - which atom is negative?
the most electronegative (closest to fluorine)
52
the sum of all ON =?
0