Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

chem org > inorganic chemistry > Flashcards

inorganic chemistry Flashcards

(67 cards)

Start Studying
1
Q

What is the Arrhenius definition of an acid?

A

An Arrhenius acid is a substance that increases the concentration of hydrogen ions (H+) in aqueous solution.

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

True or False: According to the Brønsted-Lowry theory, an acid is a proton donor.

A

True

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

Fill in the blank: According to the Lewis theory, an acid is an electron _______.

A

acceptor

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

Which of the following is a characteristic of a Brønsted-Lowry base? A) Proton donor B) Proton acceptor C) Electron acceptor

A

B) Proton acceptor

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

What is the primary distinction between Arrhenius acids and bases?

A

Arrhenius acids produce H+ ions, while Arrhenius bases produce OH- ions in solution.

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

Name one limitation of the Arrhenius definition of acids and bases.

A

It only applies to aqueous solutions and does not account for acid-base reactions in non-aqueous solvents.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

True or False: All Brønsted-Lowry acids are also Lewis acids.

A

True

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

What is a conjugate acid?

A

A conjugate acid is the species formed when a Brønsted-Lowry base accepts a proton.

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

Identify the conjugate base of HCl.

A

Cl-

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

Which theory expands the concept of acids and bases beyond proton transfer?

A

Lewis acid-base theory

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

What are electrolytes?

A

Electrolytes are substances that dissociate into ions in solution and conduct electricity.

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

Which ions are commonly considered electrolytes?

A

Common electrolytes include sodium (Na+), potassium (K+), calcium (Ca2+), magnesium (Mg2+), chloride (Cl-), bicarbonate (HCO3-), and phosphate (PO4^3-).

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

True or False: All electrolytes are acids or bases.

A

False

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

What is the primary function of electrolytes in the body?

A

Electrolytes help regulate nerve and muscle function, hydrate the body, balance blood acidity and pressure, and help rebuild damaged tissue.

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

What is the Arrhenius definition of an acid?

A

An Arrhenius acid is a substance that increases the concentration of hydrogen ions (H+) in aqueous solution.

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

What is the Brønsted-Lowry definition of a base?

A

A Brønsted-Lowry base is a substance that accepts protons (H+).

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

Fill in the blank: According to the Lewis theory, an acid is a substance that _____ an electron pair.

A

accepts

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

What is a key difference between Arrhenius and Brønsted-Lowry theories?

A

Arrhenius theory focuses on H+ and OH- ions in water, while Brønsted-Lowry theory involves proton transfer.

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

What are colligative properties?

A

Colligative properties are properties of solutions that depend on the number of solute particles in a given amount of solvent, not the identity of the solute.

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

List four colligative properties.

A
  1. Vapor pressure lowering 2. Boiling point elevation 3. Freezing point depression 4. Osmotic pressure
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

What is the formula for boiling point elevation?

A

ΔT_b = i * K_b * m

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

What does ‘i’ represent in the boiling point elevation formula?

A

‘i’ represents the van ‘t Hoff factor, which indicates the number of particles the solute dissociates into.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

True or False: Colligative properties are affected by the nature of the solute.

A

False

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

What is the formula for freezing point depression?

A

ΔT_f = i * K_f * m

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
In the context of colligative properties, what does 'm' stand for?
'm' stands for the molality of the solution.
26
What is osmotic pressure?
Osmotic pressure is the pressure required to stop the flow of solvent into a solution through a semipermeable membrane.
27
What is the formula for calculating osmotic pressure?
π = i * C * R * T
28
In the osmotic pressure formula, what does 'C' represent?
'C' represents the molar concentration of the solution.
29
What is the van 't Hoff factor for a non-electrolyte?
The van 't Hoff factor for a non-electrolyte is 1.
30
Fill in the blank: The stronger the acid, the _____ its conjugate base.
weaker
31
What is the significance of the pH scale?
The pH scale measures the acidity or basicity of a solution, where lower values are more acidic and higher values are more basic.
32
What is the pH of a neutral solution at 25 degrees Celsius?
7
33
Which property describes the lowering of vapor pressure in a solution?
Raoult's Law
34
True or False: Colligative properties are independent of the number of solute particles.
False
35
buffers
solutions with an ability to resist pH change in additions pf small amount of either strong acid or base
36
what does an acid and base in buffer react with
acid- OH- and base- H+
37
acidic buffer
contains weak acid and its salt( conjugate base)
38
basic buffer
contains weak base and its salt( conjugate acid)
39
common effect(Le Chatelier principle)
if a change is made to a system at equilibrium, the system will shift in a direction that opposes the change to restore equilibrium
40
What are the two main components of a buffer?
A weak acid and its conjugate base, or a weak base and its conjugate acid.
41
How does a buffer work?
It neutralizes added H⁺ or OH⁻ ions through reversible acid-base reactions, keeping the pH relatively constant.
42
What is the pH range in which a buffer is most effective?
Around ±1 pH unit from the pKa of the weak acid or base.
43
What is the Henderson-Hasselbalch equation?
pH = pKa + log([A⁻]/[HA]), where A⁻ is the conjugate base and HA is the weak acid.
44
What happens when [A⁻] = [HA] in a buffer? a- conjugate base ha-weak acid
pH = pKa, and the buffer has maximum efficiency.
45
What factors affect buffer capacity?
Concentration of buffer components (higher = greater capacity). Ratio of acid/base components (closer to 1:1 = more effective).
46
Give an example of a biological buffer system.
The bicarbonate buffer system in blood: H₂CO₃ ⇌ H⁺ + HCO₃⁻
47
What is an acidic buffer?
A buffer with a pH less than 7, made from a weak acid and its conjugate base (e.g., CH₃COOH + CH₃COONa).
48
What is a basic buffer?
A buffer with a pH greater than 7, made from a weak base and its conjugate acid (e.g., NH₃ + NH₄Cl).
49
how does dilution affect buffer capacity and pH?
Dilution lowers buffer capacity, but pH remains relatively unchanged unless diluted significantly.
50
Can strong acids or strong bases form buffers?
No, because they fully dissociate and do not establish an equilibrium needed for buffering.
51
electrolysis
using electricity to cause a reaction in a solution or ionic compound
52
electrolyte
liquid solution consisting of partially dissociated ions
53
oxidation number
hypothetical charge the atom would have if all bond to atoms of different elements were treated as ionic
54
What is the function of a salt bridge in a galvanic cell?
t maintains electrical neutrality by allowing ion flow between half-cells.
55
What is the standard electrode potential (E°) of a hydrogen electrode?
0.00 V (by definition).
56
How is cell potential (E°cell) calculated for a galvanic cell?
E°cell = E°cathode − E°anode
57
Which electrode is the site of oxidation in an electrochemical cell?
anode
58
Why must both half-cells be connected in an electrochemical cell?
To allow the flow of electrons through the external circuit and ions through the salt bridge.
59
What is the relationship between Gibbs free energy and cell potential?
ΔG° = −nFE°cell
60
What do the signs of ΔG and E°cell indicate about spontaneity?
If ΔG < 0 and E°cell > 0, the reaction is spontaneous.
61
What do the variables in ΔG° = −nFE°cell represent?
→ n = moles of electrons F = Faraday constant (96,485 C/mol e⁻) E°cell = standard cell potential
62
What does "Q" represent in the Nernst equation?
The reaction quotient = [products] / [reactants] for the redox reaction.
63
How does increasing the concentration of reactants affect cell potential?
It increases E (makes it more positive).
64
What happens to the cell potential if product concentration increases?
E decreases (reaction becomes less favorable).
65
What does Faraday's first law state?
The mass of substance produced at an electrode is proportional to the quantity of electricity passed.
66
What does Faraday's second law state?
For the same quantity of electricity, different substances are produced in amounts proportional to their molar masses / number of electrons exchanged.
67
Nernst equation
elates the electrode potential of a half-cell to its standard potential, temperature, and the concentrations of reactants and products.

chem org (2 decks)

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