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Acids Flashcards

(101 cards)

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1
Q

What’s the formula for carbonic acid

A

H2CO3

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2
Q

What is the formula for sulphuric acid

A

H2SO4

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3
Q

What do all acids contain

A

Hydrogen atoms - one of which is replaceable

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4
Q

Is everything that contains H acidic

A

No - there has to be a replaceable H

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5
Q

What ions are produced when acids dissolve in water

A

H+

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6
Q

What are acids a source of (ions)

A

H+

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7
Q

What are alkalis a source of (ions)

A

H+

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8
Q

What are alkalis

A

Bases that are soluble in watger

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9
Q

What are some bases (3)

A
  1. Metal oxides
  2. Metal hydroxides
  3. Ammonia
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10
Q

What colour is red litmus paper in acid and alkali

A

Acid - stays red
Alkali - goes blue

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11
Q

What colour is blue litmus paper in acid and alkali

A

Acid - turns red
Alkali - stays blue

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12
Q

What colour is litmus solution in acid and alkali

A

Acid - red
Alkali - blue

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13
Q

What colour is methyl orange in acid and alkali

A

Acid - red
Alkali - colourless

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14
Q

What colour is phenolphthalein in acid and alkali

A

Acid - Colourless
Alkali - pink

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15
Q

How to spell the indicator that is coliourless in acid and pink in alkali

A

Phenol-ph-thal-ein

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16
Q

Which acid should you write in questions for titration and why

A

Methyl orange - easier to spell than phenolphthalein

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17
Q

Give the colour spectrum for universal indicator

A

Red yellow (acid) green (neutral) blue purple (alkaline)

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18
Q

What ph is a strong acid

A

0-3

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19
Q

What ph is a weak acid

A

4-6

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20
Q

What ph is a neutral solution

A

7

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21
Q

What ph is a weak alkali

A

8-10

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22
Q

What ph is a strong alkali

A

11-14

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23
Q

What are the products of base + acid

A

Base + acid -> salt + water

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24
Q

What is the reaction of alkali + acid

A

Alkali + acid -> salt + water

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25
How is the reaction of ammonia with acid written Use sulphuric acid as the example
NH3 + H2SO4 -> (NH4)2 SO4 +H+ Note that the 2 after the ammonium is in subscript
26
27
Metal + acid =
Salt + hydrogen
28
Carbonate + acid =
Salt + water + carbon dioxide
29
What is H+ simply
A proton - hydrogen normally has 1 proton, 1 electron and 0 neutrons, but since the electron has been lost (+ charge), it is now only a proton
30
Is an acid a proton donor or acceptor
Donor
31
Is a base a proton donor or acceptor
Acceptor
32
What is the reaction of HCl + H2O and what’s the proton donor and acceptor
H3O+ + Cl- Proton donor is HCl Proton acceptor is H2O Note that in H3O+, the **WHOLE** compound has the + charge, a bit like how a carbonate ion (CO3 2-) has an overall charge of -2
33
How is H3O+ formed
One hydrogen is bonded to the oxygen by 2 electrons that originally came from the oxygen. The H2O donates a pair of electrons to the H+ ion
34
Is water an acid or alkali
Both - depending on the situation HCl + H2O -> H3O+ + Cl- it is a base as it is a proton acceptor NH3 + H20 -> NH4+ + OH- It is an acid as it is a proton donor
35
What is a carbonate ion
CO3 2-
36
Define an acid
A proton donor A substance with PH less than 7
37
Define a base in terms of protons and PH
1. A proton acceptor 2. PH of more than 7
38
Difference between an alkali and a base
An alkali is a soluble base that is dissolved in water. A base doesn’t have to be soluble, but it can be. Therefore, all alkalis are bases but not all bases are alkalis
39
What is the general equation for acid + base (2 possibilities)
HA + B -> A- + BH+ Or HA + B- -> A- + BH
40
Are SAP salts soluble
Yes
41
Are nitrates soluble
Yes - ALL NITRATES ARE SOLUBLE
42
Are all common chlorides soluble
Yes, except silver chloride and lead(ll) chloride
43
Are all common sulfates soluble
Yes, except for barium sulphate, calcium sulphate and lead(II) sulphate
44
Are all carbonates soluble
Only SAP carbonates are soluble, all other common carbonates are not
45
Are all hydroxides soluble
SAP hydroxides are soluble, calcium hydroxide is slightly soluble, but all other common hydroxides are not
46
Is ammonium hydroxide soluble and what is it known as
Yes - ammonium solution
47
Are metal oxides soluble in water
Most are not, but those that are e.g. sodium oxide dissolve to form alkalis
48
What is calcium hydroxide
Limewater
49
What is calcium carbonate
Marble chips
50
Which is marble chips and which is limewater: Calcium carbonate Calcium hydroxide
Calcium carbonate - marble chips Calcium hydroxide - limewater
51
How to do a titration steps
1. Use pipette to add set volume of acid to conical flask 2. Add 3 drops of suitable indicator (not Universal indicator) 3. Fill a **burette** with alkali - measure initial reading 4. Add alkali from burette until indicator just changes colour 5. Record amount of alkali used 6. Repeat with these measurements but with no indicator 7. Heat salt solution in evaporating basin until saturation point 8. Allow to cool and crystallise 9. Filter off crystals 10. Dry in warm oven
52
How to test for saturation point
Dip a glass rod in the solution. If crystals form quickly, then the solution is saturated
53
Why is universal indicator not used in titration
Because it doesn’t provide a sharp colour change so the **colour change is harder to spell**
54
Which is used in chemistry (for titration: Burette or Biurette
Burette No i Bi for bio
55
56
What is titration used for
SAP salts
57
What is the method you know as neutralisation known as and why do you not put neutralisation
Adding excess base All of the methods involve neutralisation reactions
58
Give the method for excess base
1. Heat acid 2. Add base and keep heating 3. Keep stirring and adding base until there is base left over (base is in excess) 4. Filter off excess base 5. Heat solution in evaporating basin until saturation point 6. Allow to cool and crystallise 6. Filter off crystals 7. Dry crystals in warm oven
59
What is the method adding excess based used for
Soluble salts that are not SAP
60
Why do you not evaporate off all the water quickly with a Bunsen
Because then only very small crystals will form
61
How can you tell when excess has been added to a carbonate + metal reaction
Fizzing will stop and then the thing in excess will be left over
62
In an excess base reaction, which does require heating out of these: oxide, metal, carbonate
Oxide
63
What is the method for metal carbonate + acid
Same as excess base method except it is not heated in step 1, instead we see that the reaction has stopped due to no more fizzing
64
What is precipitation used for
Forming an insoluble salt
65
What is added to a precipitation reaction
Solutions of two **soluble** salts
66
What is the method for precipitation
1. Mix the solutions 2. Stir the solutions 3. Filter off the reaction mixture 4. Wash the crystals with distilled water 5. Dry in a warm oven MSFWD mix stir filter wash dry
67
What must you NEVER do to salts that you produce
**WASH WITH DISTILLED WATER** - THE CRYSTALS WILL DISSOLVE!!!!!!!! (unless it is precipitation in which case this is the WASH part of the process - make sure to say distilled water here)
68
Do metals conduct electricity
Yes
69
Do non metals conduct electricity
Generally no, but graphite is an exception
70
Name a non metal that conducts electricity
Graphite
71
Why does graphite conduct electricity
It has delocalised electrons due to the carbons forming in hexagonal 3D shapes, so each carbon has 3 covalent bonds, leaving 1 delocalised electron which is free to move
72
What PH are metal oxides
Basic
73
What PH are non-metal oxides
Acidic
74
What are basic oxides
Bases
75
What do basic oxides react with
Bases
76
Give the reaction for sodium oxide (base) turning into an alkali
Na2O + H2O -> 2NaOH
77
Are most metal oxides soluble in water and what does this mean
No, meaning that there are not a lot of alkalis
78
Group 1 metal ions charge
+1
79
Group 2 metal ions charge
2+
80
Group 3 metal ions charge
3+
81
Carbon ion charge
+4 or -4
82
Iron ion charge
Fe(II) = 2+ Fe(III) = 3+
83
Aluminum ion charge
3+
84
Group 7 ions charge
-1
85
Hydroxide formula and charge
OH^- -1
86
Nitrate ion formula and charge
NO3^- Note that it is NO3 , with an overall charge of -1, NOT NO with a charge of -3
87
Oxide ion charge
O^2- Charge of -2 O with a charge of -2, NOT O2 with a charge of -1
88
Sulphide ion charge
S^2- 2-
89
Carbonate ion formula and charge
CO3^2- CO3 with a charge of -2
90
Sulphate ion formula and charge
SO4^2- Charge of -2
91
Nitride ion charge
-3
92
Nitrate vs nitride: give 1. Their formulas and 2. Their charges
Nitrate: NO3^- Nitride: N3^- Nitride is lower in the alphabet (i vs a) so it has a more negative charge
93
Give an example of an acidic oxide and a basic oxide
Acidic oxide - SO2, CO2, NO2 Basic oxide - Na2O, CuO, K2O
94
What do acidic oxides form when they 1. React with bases 2. Dissolve in water
1. Salts 2. Acids
95
Silver ion
Ag+
96
Ammonium ion
NH4+
97
Hydrogen ion
H+
98
Group 2 metals charge
2+
99
Group 1 metals charge
1+
100
Group 3 metals charge
3+
101
Carbon ion charge

Chemistry (7 decks)

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