unit 4 Flashcards

(45 cards)

1
Q

when the conditions on a system at equilibrium are changed, the system will react to reach a new equilibrium that partially reduces or counteracts the change

A

le chatelier’s principle

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2
Q

describe the development of a chemical equilibrium

A

The faster reaction will gradually become slower
The slower reaction will become faster
Finally, the reaction rates become equal, and the equilibrium is established

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3
Q

what is the effect of temperature on vapor pressure of a substance

A

as temperature increases, pressure increases

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4
Q

according to le chatelier’s principle, what does a system do when conditions on a system at equilibrium are changed

A

the system will react to reach a new equilibrium that partially reduces or counteracts the change

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5
Q

chemical equilibrium can only be reached in a ?

A

closed system

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6
Q

at when is a pH level neutral?

A

7

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7
Q

describe meaning of the pH scale. Higher pH means more ?, lower pH means more ?.

A

higher pH means more basic, lower pH means more acidic

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8
Q

How to calculate the pH from [H+] and vice versa

A

10 raised to the -ph

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9
Q

how to calculate pOH from [OH-] and vice versa

A

kw/h+ or 10^-14/h+ or 10^-pOH

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10
Q

how to calculate [H+] from [OH-] and vice versa

A

[H+] x [OH-] = 1 x 10^-14

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11
Q

how to calculate pH from pOH and vice versa

A

pH + pOH = 14

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12
Q

Definition of an acid and a base according to Bronsted-Lowry

A

Acids: Substances that donates a proton
Base: substances that accept a proton

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13
Q

what are the conditions that affect the rate of a chemical reaction

A

temperature, concentration, catalyst, and inhibitors

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14
Q

describe how temperature affects the rate of a chemical reaction

A

Chemical reactions are faster at higher temperatures and slower at lower temperatures

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15
Q

describe how concentration affects the rate of a chemical reaction

A

The more particles there are in a given volume, the more frequently collisions will occur and the more rapidly the reaction will take place

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16
Q

A third-party substance that speeds up the rate of the reaction by lowering the activation energy of the reaction, thus enabling more reactant molecules to overcome the energy barrier

A

catalyst

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17
Q

Substances interfere with a normal reaction path from reactants to products, forcing the reaction to a higher activation energy route that is slower

A

inhibitor

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18
Q

what are the 3 energy changes during a molecular collision

A

transition state, potential energy barrier, and activation energy

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19
Q

when two molecules are colliding, they form a ? that has a high potential energy at the top of the hump of the curve

A

transition state

20
Q

the hump is a ? that must be surpassed before a collision can be effective

A

potential energy barrier

21
Q

the minimum kinetic energy a particle must have to enter into a reaction-producing collision

A

activation energy

22
Q

For an individual collision to result in a reaction, the particles must have:

A

enough kinetic energy and proper orientation

23
Q

whatdoes the pH scale represent

A

hydrogen ion concentration

24
Q

acidic solutions have more ?, meaning they have a ? pH

A

more H+, lower pH

25
basic solutions have less ?, meaning they have a ? pH
less H+, higher pH
26
a solution is neutral if pH = ....
7
27
If [H+] = [OH-] = 10^-7 M, the solution is
neutral
28
If [H+] > [OH-]
acidic
29
If [H+] < [OH-]
basic
30
what is the water constant (Kw) equation
Kw = [H+][OH-] = 1.0 x 10^-14
31
the more h+, the more ____ a solution is
acidic
32
the more oh-, the more _____ a solution is
basic
33
a bronsted lowry base role in proton transfer
accepts proton
34
bronsted lowry acid role in proton transfer
donates proton
35
a substance that can behave as an acid in one case and base in another
amphoteric substance
36
reversible reaction read from right to left
reverse reaction
37
reversible reaction read from left to right
forward reaction
38
has a sour taste, changes litmus strip to red
acid
39
slippery feeling, changes litmus strip to blue
base
40
number of equivalents per liter of solution
normality
41
normality equation
of equivalents/volume (in liters)
42
dilution/solution equation
Vc x Mc = Vd x Md
43
amount in moles of solute per volume in liters of solution
molarity
44
molarity equation
moles solute/liters solution
45
Definition of a base according to Arrhenius.
a compound that increases the concentration of hydroxide ion (OH −) in aqueous solution.