Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

Chemistry > Mod. 6 > Flashcards

Mod. 6 Flashcards

1
Q

What did Lovoiser suggest?

A
  • An acid contains oxygen
  • Non-metal oxides react with water to form acidic solutions
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What did Darvy suggest?

A
  • Acids contain hydrogen
  • Metal oxides = bases
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What was Arrhenius’s proposal?

A

Acids produce H+ ions in water and bases produce OH- ions in water, in aqueous solutions
- Arrhenius explained neutralisation

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

What were the limitations of Arrhenius’s proposal?

A
  • Could not explain why certain compounds do not contain hydroxide ions, despite displaying basic properties, e.g. 2HCI + CaCO3 → CaCl2 + H2O + CO2 [calcium carbonate is basic but doenst contain OH]
    -Could not explain acid-base reaction that do not occur in aqueous solutions, e.g.
    NH3(g)+ HCI(g)→ NH4Cl(s)
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

What did Bronsted Lowry’s proposal?

A
  • acid donates H+ protons
  • bases accept H+ protons
  • acids have high concentrations of H+
  • bases have lower concentrations of H+
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What were the limitations of B-L theory?

A
  • Doesn’t explain the acidity of acidic oxides ( SO2)/ basicity of basic oxides ( MgO)
  • Doesn’t explain reaction between acidic and basic oxides that don’t involve proton transfer, e.g. SO3(g)+ CaO(s)→ CaSO4(s)
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

What’s an inorganic acid?

A

a substance with an ion attached to 1 or more hydrogen

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

What’s an inorganic base?

A

a substance that releases OH- in solutions

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

What’s the equation for acid-carbonate reactions?

A

carbonate + acid –> salt + carbon dioxide + water

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

Provide an example of an acid-carbonate reaction.

A

2HI(aq) + Na2CO3 –> NaCl ( aq) + CO2( g) + H20 (l)

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

What’s the equation for acid-metal reactions?

A

acid + metal hydroxide –> salt + water

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

Provide an example of an acid-metal reaction.

A

Na(s) + HCI( aq) –> NaCl (aq) + 1/2 H20(l)

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

What does neutralisation mean?

A

when the concentration of hydronium and hydroxide ions becomes equal

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

What’s the equation for a neutralisation reaction?

A

acid + base → salt + water

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

Provide an example of a neutralisation reaction.

A

NaOH(aq) + HNO3(aq) –>Na NO3(aq)+H2O(l)

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

Name 3 strong acids

A

HCI, H2SO4, HNO3

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

Name 3 weak base.

A

CH3COOH, H2CO3, H3PO4

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

Name 3 strong bases.

A

NaOH, KOH, H3PO4

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

Name 3 weak bases

A

NH3, C5H5N, CH3NH2

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

Define hydrolysis.

A

the reaction of a salt with water that results in a pH change

21
Q

Explain the hydrolysis of acidic salts.

A

acidic salts contain conjugate acids of weak bases which hydrolise to produce acidic solutions.

22
Q

Explain the hydrolysis of basic salts

A

basic salts contain conjugate bases of weak acids which hydrolise to produce an alkaline

23
Q

Explain the hydrolysis of neutral salts

A

typically formed from the neutralisation between strong acids and strong bases ( do not hydrolyse)

24
Q

What happens to the volume and concentration when diluted?

A

the volume increases and the concentration decreases

25
What happens to the pH during dilution?
- for acids the pH increases -for bases the pH decreases
26
What is a primary standard?
a solution that is prepared using chemicals that are pure that are used o prepare a solution accurately of known concentration
27
What are the properties of a primary standard?
- high level of purity - free of moisture - stable and unaffected by air during weighing
28
What are examples of some primary standards? Provide an acid and a base.
- potassium hydrogen phthalate ( acid) - sodium carbonate ( base)
29
What are two examples of non-primary standards?
- Sulfuric acid→ absorbs water from the atmosphere -Sodium hydroxide → absorbs moisture from the air
30
Define the word titration.
volumetric analysis used to determine the concentration of an unknown solution
31
Define endpoint
the point at which the colour of the indicator changes
32
Define equivalence point
the point at which enough titrant has reacted with all the substances that the experiment comes to an end
33
If initial pH is below 2 the curve indicates its a...
strong acid
34
If the initial pH is 4-7 the curve indicates its a...
weak acid
35
If initial pH is 10 or 11 the curve indicates its a...
weak base
36
if initial pH is higher than 13 the curve indicates its a...
strong base
37
Why do weak acid + weak base titrations not work?
they don't have a clear indication of the equivalence point as there is no shape rise around the equivalence point
38
What indicator is used for strong acids/ strong bases? Describe the colour change.
Bromyothyl blue. When acidic turns yellow when basic turns blue.
39
Methyl Orange turns red to yellow. What acid and base is this applied to?
Strong acid/ weak base
40
What indicator is used for strong base/ weak acid titrations? Describe the colour change.
Phenolphthalein it changes from colourless ( acidic) to pink (basic)
41
What's the substance used to rinse the conical flask? Justify your answer.
distilled water → doesn't leave residue chemicals that can affect the measurements
42
What's the substance used to rinse pipettes? Justify your answer.
distilled water, then with the solution they will measure and transfer → ensures that any water or solution from previous use is completely removed.
43
Define diprotic.
diprotic means the substance has 2 acidic hydrogen protons.
44
What's the difference in pH between a monoprotic and diprotic substance?
Diprotic substances will have a lower pH. This is because when diprotic substances ionise, they produce a higher concentration of hydrogen ions, compared to monoprotic ones.
45
Why is it important during titrations to keep the amount of indicator added to a minimum?
- Addition of large amount of indicator can change H+ concentration - Can change the equivalence point or the accuracy/ validity of reading - Weak acid and conjugate base can absorb or release H+ ions resulting in addition of acid or base
46
What's the formula for indicators?
Hln --> H + In
47
How do indicators impact the equilibrium of an acid?
when an acid is added, [H+] increases, equilibrium shift to the left
48
How do indicators impact the equilibrium of a base?
when a base is added OH- bonds with H+ to form H20. As [H+] decrease, the equilibrium shifts to the right

Chemistry (3 decks)

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