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Chem 203 > Final > Flashcards

Final Flashcards

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1
Q

What is a Bronsted-Lowry Base?

A

a proton acceptor

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2
Q

What is a Bronsted-Lowry Acid?

A

proton donor

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3
Q

What does it mean to be amphiprotic?

A

a species that can either donate or accept an electron in a bronsted-lowry reaction

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4
Q

what does it mean to be amphoteric?

A

a species that can act as either an acid or a base

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5
Q

what is autoionization?

A

for water, the transfer of protons to yield hydronium and hydroxide ions

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6
Q

What is a buffer?

A

a mixture of appreciable amounts of a weak acid-base pair

it spH resists change when small amounts of acid or base are added

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7
Q

what is buffer capacity?

A

the amount of an acid or base that can be added to a volume of a buffer solution before its pH changes significantly

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8
Q

what is a conjugate acid?

A

a substance formed when a base gains a proton

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9
Q

what is a conjugate base?

A

a substance formed when an acid loses a proton

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10
Q

what is a diprotic acid/base?

A

an acid containing two ionizable hydrogen atoms per molecule
or
a base capable of accepting two protons

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11
Q

what is the levelling effect?

A

the strength of acid-base solutes in a given solvent is limited to the solvent’s characteristic acid and base species

in water, hydronium and hydroxide

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12
Q

what does a titration curve display?

A

pH vs volume of an added titrant

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13
Q

why does the neutralization reaction of a weak acid with a strong base give a weakly basic solution?

A

the salt ionizes the solution, but the anion slightly reacts with water to formulate a weak acid. The reaction also forms OH-, which then causes the solution to be basic.

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14
Q

what two assumptions can simplify calculations of equilibrium concentrations in a weak acid or base?

A
  1. Assume that the initial concentration of the acid is neglected, so this concentration can be assumed constant and equal to the initial value of the total acid concentration.
  2. Assume we can neglect the contribution of water to the equilibrium concentration of H3O+.
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15
Q

Explain why the pH does not change significantly when a small amount of an acid or a base is added to a solution that contains equal amounts of the acid H3PO4 and a salt of its conjugate base NaH2PO4.

A

Excess H3O+ is removed primarily by the reaction:
H3O+(𝑎𝑞) + H2PO4 (𝑎𝑞) ⟶ H3PO4(𝑎𝑞) + H2O(𝑙)

Excess base is removed by the reaction: OH−(𝑎𝑞) + H3PO4(𝑎𝑞) ⟶ H2PO4−(𝑎𝑞) + H2O(𝑙)

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16
Q

Explain how to choose the appropriate acid-base indicator for the titration of a weak base with a strong acid.

A

At the equivalence point in the titration of a weak base with a strong acid, the resulting solution is slightly acidic due to the presence of the conjugate acid. Thus, pick an indicator that changes colour in the acidic range and brackets the pH at the equivalence point. Methyl orange is a good example.

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17
Q

what is a salt?

A

an ionic solid that dissociates completely in water

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18
Q

define system

A

the part of the universe being studied

19
Q

define surroundings

A

a part of the universe not being studied
anything that is not a part of the system

20
Q

define universe

A

everything
system + surroundings = universe

21
Q

define the enthalpy of formation

A

the enthalpy change of a chemical reaction in which 1 mole of a pure substance is formed from its elements in their most stable states under standard state conditions

22
Q

what is specific heat capacity?

A

intensive property of a substance that represents the quantity of heat required to raise the temperature of 1 gram of the substance by 1 degree Celsius (or 1 kelvin)

23
Q

what is pressure-volume work?

A

expansion work (or pressure-volume work) occurs when a system pushes back the surroundings against a restraining pressure, or when the surroundings compress the system.

24
Q

what is internal energy?

A

the total energy of a system
U = Ek + Ep

25
Q

what is entropy?

A

state function that is a measure of the matter and/or energy dispersal within a system, determined by the number of system microstates; often described as a measure of the disorder of the system

26
Q

what is free energy? how does it relate to spontaneity, enthalpy and entropy?

A
27
Q

what is spontaneity? how does it relate to free energy, enthalpy and entropy?

A
28
Q

how can you alter spontaneity?

A
29
Q

what is the first law of conservation of energy?

A

energy can be converted from one form to another, but cannot be created nor destroyed

30
Q

What is energy?

A

the ability to do work (J)

31
Q

what is kinetic energy?

A

energy due to motion (thermal energy )

32
Q

what is potential energy?

A

energy due to position (stored energy)

33
Q

what is temperature?

A

the measure of the average kinetic energy of atoms or molecules

the quantity that determines the direction of heat flow

measure of thermal energy in a system

34
Q

what is thermal equilibrium?

A
35
Q

what is heat?

A
36
Q

what is an intensive property?

A

property of a substance that is independent of the amount of the substance

ie. density

37
Q

what is an extensive property?

A

property of a substance that depends on the amount of the substance

38
Q

what is a microstate (W)

A

A microstate is a specific configuration of all the locations and energies of the atoms or molecules that make up a system.

39
Q

what is a state funtion

A

property depending only on the state of a system, and not the path that is taken to reach that state

ex. enthalpy

40
Q

what is bomb calorimetry?

A
41
Q

what is isobaric calorimetry?

A
42
Q

is specific heat capacity intensive or extensive?

A

it is intensive

43
Q

is heat capacity extensive or intensive?

A

it is extensuve

Chem 203 (2 decks)

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