Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

chemistry > Chemical Changes And Structure #4: Acids And Bases > Flashcards

Chemical Changes And Structure #4: Acids And Bases Flashcards

(80 cards)

Start Studying
1
Q

Acids have a pH of…

A

Less than 7

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Pure Water + Neutral Solutions have a pH…

A

of 7

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Alkalis have a pH of…

A

Greater than 7

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Why do chemists use electronic pH probes to accurately measure the pH of a solution?

A

Because using a colour chart is subjective

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

What do chemists use to accurately measure the pH of a solution?

A

pH probes

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Examples of Acids

A
  • Vinegar
  • Lemonade
  • Soda Water
  • Coke
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Examples of Alkalis

A
  • Baking Soda
  • Dishwasher Powder
  • Bleach
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Acids are compounds that produce ____ when dissolved in water

A

H+ (aq) ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Alkalis are compounds that produce ____ when dissolved in water

A

OH- (aq) ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Formula of Hydrochloric Acid

A

HCl

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Ions present in Hydrochloric acid (HCl)

A

H+ (aq) and Cl- (aq)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Formula for sulfuric acid

A

H2 SO4

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Ions Present in Sulfuric Acid (H2SO4)

A

2H+ (aq) and SO4 2- (aq)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Formula for Nitric Acid

A

HNO3

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Ions present in Nitric Acid (HNO3)

A

H+(aq) and NO3 - (aq)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Formula for sodium hydroxide

A

NaOH

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Ions Present in Sodium Hydroxide (NaOH)

A

Na+ (aq) and OH- (aq)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Ions present in Potassium Hydroxide (KOH)

A

K+ (aq) and OH- (aq)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Formula of Potassium Hydroxide

A

KOH

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

Formula for Calcium Hydroxide

A

CaOH2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Ions present in Calcium Hydroxide (CaOH2)

A

Ca 2+ (aq) and 2OH-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

How can you tell if something is an acid or alkali? ***

A
  • It has the word acid in its name if it’s an acid
  • It has the word hydroxide (OH-) in it if it’s an alkali
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

What is the concentration of H+ (aq) and OH- (aq) in neutral solutions?

A

It’s equal

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

Give an example of equal concentration in neutral solutions

A

H2O ⇌ H+ (aq) + OH- (aq)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
What is a reversible reaction?
One which can proceed in both directions: Reactant + Reactant ⇌ Product(s)
26
What is equilibrium? (2)
- Equilibrium is when the rates of the forward and reverse reactions are equal - At equilibrium, the concentrations of reactants and products remain constant, although not necessarily equal
27
What happens to the concentrations of reactants and products at equilibrium?
They remain constant, although not necessarily equal
28
Equilibrium in water (5)
1 - Water molecules are constantly breaking up to form ions which in turn are constantly combining to reform water molecules 2 - This equilibrium exits in water and all aqueos solutions 3 - H20 ⇌ H+ (aq) + OH- (aq) 4 - Only 1 in 55million water molecules break up into ions 5 - Therefore, water is a poor conductor of electricity
29
What are water molecules constantly doing?
Breaking up to form ions which in turn are constantly combining to reform water molecules
30
What does the equilibrium of molecules breaking up to form ions and then combining to reform molecules exist in?
Water and all aqueos solutions
31
Why is water a poor conductor of electricity?
Only 1 in 55million water molecules break up into ions
32
What is pH a measure of?
The hydrogen ion concentration p = potens (power) H = Hydrogen (H+)
33
Acidic solutions contain more ___ than ___
H+ (aq) ions , pure water
34
Alkaline solutions contain more ___ than ___
OH- (aq) ions, pure water
35
Neutral solutions contain ___ concentrations of ___
H+ (aq) and OH- (aq) ions
36
What do concentrated acids and alkalis contain?
A lot of acid or alkali in a small volume of water
37
What do dilute acids and alkalis contain?
A small amount of acid or alkali in a large volume of water
38
The effects of dilution (adding water) to an acid?
It increases the pH of the solution as the concentration of H+ (aq) ions decreases
39
The effects of dilution (adding water) to an alkali?
It decreases the pH of the solution as the concentration of OH- (aq) ions decreases
40
What do non-metals burn in oxygen to produce?
Non-Metal Oxides. C(s) + O2 (g) -> CO2 (g)
41
What do non-metal oxides dissolve in water to form? Give an example.
Acidic Solutions. CO2 (g) + H2O (l) -> H2CO3 (aq)
42
What do metals burn in oxygen to produce? Give an example.
Metal oxides. (All of which are bases) 2Mg (s) + O2 (g) -> 2MgO (s)
43
All metal oxides are…
Bases
44
What happens if a metal oxide (metals burned in the presence of oxygen) is soluble in water? Give an example.
An alkali. MgO (s) + H2O (l) -> Mg(OH)2 (aq)
45
What do all soluble metal hydroxides do?
Dissolve in water to produce alkaline solutions
46
What do insoluble oxides and hydroxides not do?
Affect the pH of water (because they don’t dissolve in it)
47
What page is the solubility of compounds found?
8
48
What is ammonia the common name for?
Nitrogen Hydride
49
What does ammonia do (as a gas)? What does this make it?
Neutralise acids, making it a base
50
What is ammonia (as a covalent molecule)?
It dissolves in water to produce an alkaline solution
51
Formula of ammonia dissolving in water to produce an alkaline solution
NH3 (g) + H2O ⇌ NH4 + (aq) + OH - (aq)
52
What is the formula of ammonium?
NH4
53
What is the formula of ammonia?
NH3
54
What is a neutralisation reaction?
The reaction of acids with bases
55
What happens to the pH in a neutralisation reaction?
It moves toward 7
56
What is a base? ***
Compounds which react with H+ (aq) ions to produce water (A SOLUBLE ALKALI)
57
Bases include:
- Metal Oxides - Metal Hydroxides - Metal Carbonates - Ammonia (kind of an exception but still a base)
58
What are the 4 main neutralisation reactions?
Acid + Metal hydroxide -> salt + water Acid + Metal oxide -> salt + water Acid + Metal carbonate -> salt + water + carbon dioxide Acid + metal -> salt + hydrogen
59
What are salts?
Ionic compounds that are formed during neutralisation
60
What happens during neutralisation?
The hydrogen ions of the acid are replaced by metal ions or ammonium ions
61
What do salts contain?
- a positive metal ion (or ammonium ion) from the base - a negative ion from the acid
62
How are salts named?
- positive metal ion of the base (ammonia becomes ammonium) - negative ion present in the acid (hydrochloric acid makes chloride salts) (nitric acid makes nitrate salts) (sulphuric acid makes sulfate salts)
63
What is the form for HCl (aq) + NaOH (aq) -> NaCl (aq) + H20
Acid + alkali -> salt + water
64
What is a spectator ion?
An ion which appears on both sides of the ionic equation. It is present in the reaction mixture but takes no part in the reaction.
65
n =
CV
66
n stands for
Number of moles
67
C stands for
Concentration (l-1)
68
V stands for
Volume (l)
69
c =
n/v
70
v =
n/c
71
What is a standard solution?
One whose concentration is known accurately
72
Why is knowing the exact concentration in a standard solution important?
If you are going to carry out calculations involving that equation
73
Procedure of making standard solution
1. Accurately weigh the substance in a small beaker 2. Add a small volume of deionised water and stir to dissolve 3. Transfer to a standard flask along with the washings from the beaker 4. Make up to the mark carefully using distilled water 5. Invert several times to mix thoroughly
74
What is a volumetric titration?
An experiment in which the volumes of reacting liquids are accurately measured
75
How is the alkali/acid measured in acid/alkali titrations?
Alkali = pipettes Acid = burette
76
How can we calculate the concentration of an acid or alkali?
If the concentration of the alkali is known or vice versa
77
Procedure of volumetric titration
1. Pipette 25ml of alkali into the conical flask. 2. Add universal indicator and swirl 3. Fill the burette with acid, zero, and remove funnel Then proceed to rough titration: 4. Add 1ml of acid at a time and swirl after each addition. Note the end-point volume Proceed to Accurate Titration: 5. Add the acid until 1ml from the rough end point. Carefully add the acid drop-wise and swirl after each addition. 6. Continue titrating until you have 2 concordant results that agree within 0.2ml.
78
Soluble metal oxides form
Alkalis
79
Soluble non-metal oxides form
Acids
80
Neutralisation
The reaction of an acid with a base (to produce water)

chemistry (11 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions