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AH Chemistry > 2.1 Equilibrium > Flashcards

2.1 Equilibrium Flashcards

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1
Q

Equilibrium

A

When the rate of the forward reaction equals the rate of the backwards reaction

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2
Q

When the rate of the forward reaction equals the rate of the backwards reaction

A

Equilibrium

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3
Q

In equilibrium, the composition of products and reactants remain ______

A

constant

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4
Q

__________, the composition of products and reactants remain ______

A

In equilibrium

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5
Q

In equilibrium, the ______________ remain constant

A

composition of products and reactants

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6
Q

For an equilibrium to be established, what must happen

A

The reaction must take place in a closed environment

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7
Q

Equilibrium equation (higher)

A

A + B → C + D

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8
Q

Increasing the concentration of A or B shifts equilibrium to the _____

A

Right

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9
Q

Increasing the concentration of C or D shifts equilibrium to the ____

A

Left

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10
Q

Increasing the concentration of _____ shifts equilibrium to the left

A

C + D

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11
Q

Increasing the concentration of ______ shifts equilibrium to the right

A

A + B

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12
Q

________ the concentration of C or D shifts equilibrium to the left

A

Increasing

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13
Q

_______ the concentration of A or B shifts equilibrium to the right

A

Increasing

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14
Q

______ the pressure shifts equilibrium to where the higher number of moles

A

Decreasing

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15
Q

Decreasing the _________ shifts equilibrium to where the higher number of moles

A

Pressure

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16
Q

Decreasing the pressure shifts equilibrium to ______________________

A

where the higher number of moles

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17
Q

_____________ the pressure shifts equilibrium to where the lower number of moles is

A

Increasing

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18
Q

Increasing the _________ shifts equilibrium to where the lower number of moles is

A

Pressure

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19
Q

Increasing the pressure shifts equilibrium to _________________________

A

where the lower number of moles is

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20
Q

Exothermic reaction energy change

A

Negative, energy is released

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21
Q

Negative, energy is released

A

Exothermic

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22
Q

Exothermic reaction:

_________ the temperature shifts equilibrium to the left

A

Increasing

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23
Q

Exothermic reaction:

Increasing the _____________ shifts equilibrium to the left

A

Temperature

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24
Q

Exothermic reaction:

Increasing the temperature shifts equilibrium to the _____

A

Left

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25
Q

Exothermic reaction:

_____________ the temperature shifts equilibrium to the right

A

Decreasing

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26
Q

Exothermic reaction:

Decreasing the _________ shifts equilibrium to the right

A

Temperature

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27
Q

Exothermic reaction:

Decreasing the temperature shifts equilibrium to the ________

A

Right

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28
Q

______________ reaction:

Decreasing the temperature shifts equilibrium to the right

A

Exothermic

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29
Q

Endothermic reaction energy change

A

Positive

Energy is absorbed

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30
Q

__________ reaction:

Increasing the temperature shifts equilibrium to the right

A

Endothermic

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31
Q

Positive, energy is absorbed

A

Endothermic

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32
Q

__________ reaction:

Increasing the temperature shifts equilibrium to the right

A

Endothermic

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33
Q

Endothermic reaction:

_________ the temperature shifts equilibrium to the right

A

Increasing

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34
Q

Endothermic reaction:

Increasing the _________ shifts equilibrium to the right

A

Temperature

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35
Q

Endothermic reaction:

Increasing the temperature shifts equilibrium to the ________

A

Right

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36
Q

_________ reaction:

Decreasing the temperature shifts equilibrium to the left

A

Endothermic

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37
Q

Endothermic reaction:

_________________ the temperature shifts equilibrium to the left

A

Decreasing

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38
Q

Endothermic reaction:

Decreasing the __________ shifts equilibrium to the left

A

Temperature

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39
Q

Endothermic reaction:

Decreasing the temperature shifts equilibrium to the ____

A

Left

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40
Q

Catalyst

A

speed up the rate of reaction by providing an alternative route through lowering the activation energy

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41
Q

speed up the rate of reaction by providing an alternative route through lowering the activation energy

A

Catalyst

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42
Q

Equilibrium and catalyst

A

Catalyst does not change position of equilibrium

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43
Q

Equilibrium equation AH

A

aA + bB → cC dD

Small letters are number of moles

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44
Q

Equilibrium constant, K

A

The ratio of concentration of products:reactants

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45
Q

The ratio of concentration of products:reactants

A

Equilibrium constant

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46
Q

When calculating equilibrium constants, what is value of pure solids (s) and liquids (l)

A

1 mol/l

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47
Q

When calculating equilibrium constants, what is the value of aqueous solutions

A

What is stated in question

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48
Q

Equilibrium if Kc is less than 1

A

More reactants

Equilibrium lies to the left

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49
Q

Value of K when there are more reactants

Equilibrium lies to the left

A

less than 1

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50
Q

Equilibrium when K=1

A

Equilibrium

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51
Q

Value of K when equilibrium is reached

A

1

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52
Q

Equilibrium when K is less than 1

A

More reactanthan products

Equilibrium lies to the left

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53
Q

Value of K when there is more products than reactants

Equilibrium lies to the right

A

K is more than 1

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54
Q

Extent of reaction when Kc < 10^-3

A

Effectively no reaction

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55
Q

Value of Kc when there is effectively no reaction

A

Kc < 10^-3

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56
Q

Extent of reaction when Kc is 10^-3 to 10^3

A

Significant quantities of products and reactants at equilibrium

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57
Q

Value of Kc when there is significant quantities of reactants and products at equilibrium

A

10^-3 to 10^3

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58
Q

Extent of reaction value of Kc is > 10^3

A

Reaction is effectively complete

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59
Q

Value of Kc when the reaction is effectively complete

A

Kc is > 10^3

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60
Q

What is Kc for

A

Solutions

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61
Q

K for solutions

A

Kc

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62
Q

What is Kp for

A

Gases

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63
Q

K for gases

A

Kp

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64
Q

Homogeneous equilibrium

A

All the species are in the same gaseous phase

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65
Q

All the species are in the same gaseous phase

A

Homogenous equilibrium

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66
Q

Heterogeneous equilibrium

A

All the species are in more than one phase

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67
Q

All the species are in more than one phase

A

Heterogeneous equilibrium

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68
Q

Effect of pressure on equilibrium constant

A

No effect

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69
Q

Effect of concentration on equilibrium constant

A

No effect

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70
Q

Effect of temperature on K

A

Has an affect

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71
Q

Catalyst effect on equilibrium

A

No affect

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72
Q

What can affect K

A

Temperature

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73
Q

What doesn’t affect K

A

Pressure
Concentration
Catalysts

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74
Q

___________ reaction:

At higher temperatures, products are favoured so K will increase

A

Endothermic

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75
Q

Endothermic reaction:

At _______ temperatures, products are favoured so K will increase

A

Higher

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76
Q

Endothermic reaction:

At higher temperatures, ________ are favoured so K will increase

A

Products

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77
Q

Endothermic reaction:

At higher temperatures, products are favoured so K will _______

A

Increase

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78
Q

________ reaction:

At lower temperatures, reactants are favoured so K will decrease

A

Endothermic

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79
Q

Endothermic reaction:

At _______ temperatures, reactants are favoured so K will decrease

A

Lower

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80
Q

Endothermic reaction:

At lower ________, reactants are favoured so K will decrease

A

Temperature

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81
Q

Endothermic reaction:

At lower temperatures, ______ are favoured, so K will decrease

A

Reactants

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82
Q

Endothermic reaction:

At lower temperatures, products are _________ so K will decrease

A

Favoured

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83
Q

Endothermic reaction:

At lower temperatures, products are favoured so K will ________

A

Decrease

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84
Q

_______ reaction:

Reactants are favoured, so a decrease in K

A

Exothermic

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85
Q

Exothermic reaction:

A _______ in temperature causes a decrease in K

A

Rise

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86
Q

Exothermic reaction:

A rise in __________ causes a decrease in K

A

Temperature

87
Q

Exothermic reaction:

A rise in temperature causes a ________ in K

A

Decreases

88
Q

__________ reaction:

A fall in temperature causes an increase in K

A

Exothermic

89
Q

Exothermic reaction:

A ______ in temperature causes an increase in K

A

Fall

90
Q

Exothermic reaction:

A fall in ________ causes an increase in K

A

Temperature

91
Q

Exothermic reaction:

A fall in temperature causes an _______ in K

A

Increase

92
Q

Units for K

A

No units

93
Q

Equilibrium of water and aqueous solutions

A

There is an equilibrium between the water molecules and hydronium (hydrogen) and hydroxide ions

94
Q

Equilibrium of water and aqueous solutions

A

There is an equilibrium between the water molecules and hydronium (hydrogen) and hydroxide ions

95
Q

Ionisation of water equation

A

H20 (l) + H2O (l) → H3O+ (aq) + OH- (aq)

96
Q

H20 (l) + H2O (l) → H3O+ (aq) + OH- (aq)

A

Ionisation of water equation

97
Q

H3O+

A

Hydronium ion, a hydrated proton, H+

98
Q

Hydronium ion, a hydrated proton, H+

A

H3O+

99
Q

Water in reactions relating to pH

A

It is amphoteric

100
Q

Amphoteric

A

Can react as an acid and a base

101
Q

Can react as an acid and a base

A

Amphoteric

102
Q

The dissociation constant for the ionisation of water aka

A

The iconic product of water, Kw

103
Q

The ionic product of water, Kw

A

The dissociation constant for the ionisation of water aka

104
Q

What does the value of ionic product vary with

A

Temperature

105
Q

Ionic product of water at 25

A

1 x 10^-14

105
Q

Two relationships between pH and hydrogen ion concentration

A

pH = -log10 [H+]

[H+] = 10^-pH

106
Q

in water and aqueous solutions with a pH of 7, what is the concentration of H+ and OH-

A

Both are 10^-7 mol l-1 at 25 degrees

107
Q

Brønsted Lowry definition of acid

A

A proton donor

108
Q

A proton donor

A

Acid

109
Q

Bronsted Lowry definition of base

A

Proton acceptor

110
Q

Proton acceptor

A

Base

111
Q

For every acid, there is a …

A

Conjugate base

Which is formed by the loss of a proton

112
Q

For every conjugate base, what is there

A

A acid

113
Q

For every base, what is there

A

A conjugate acid

Which is formed by the gain of a proton

114
Q

For every conjugate acid, what is there

A

A base

115
Q

What happens to strong acids and strong bases in aqueous solutions

A

They are completely dissociated into ions

116
Q

What are completely dissociated into ions in aqueous solutions

A

Strong acids and bases

117
Q

In what are strong acids and bases completely dissociated completely dissociated into ions

A

Aqueous solutions

118
Q

In what are weak acids and bases only partially dissociated into ions

A

In aqueous solutions

119
Q

What are partially dissociated into ions in aqueous solutions

A

Weak acids and bases

120
Q

What happens to weak acids and weak bases in aqueous solutions

A

Only partially dissociated into ions

121
Q

Strong acids

A

Hydrochloric acid

Sulphuric acid

Nitric acid

122
Q

Hydrochloric acid

Sulphuric acid

Nitric acid

A

Strong acids

123
Q

Weak acids

A

Ethanoic acid

Carbonic acid

Sulfurous acid

124
Q

Ethanoic acid

Carbonic acid

Sulfurous acid

A

Weak acids

125
Q

Strong base examples

A

Solutions of metal hydroxides

126
Q

Solutions of metal hydroxides

A

Strong base examples

127
Q

Examples of weak bases

A

Ammonia and amines

128
Q

Ammonia and amines

A

Examples of weak bases

129
Q

The weakly acidic nature of solutions of carboxylic acids, sulphur dioxide and carbon dioxide can be explained by _____

A

referencing equations to show the equilibria

130
Q

The weakly acidic nature of solutions of carboxylic acids, sulphur dioxide and carbon dioxide can be explained by _____

A

referencing equations to show the equilibria

131
Q

The ___________ of solutions of carboxylic acids, sulphur dioxide and carbon dioxide can be explained by referencing equations to show the equilibria

A

Weakly acidic nature

132
Q

The weakly acidic nature of ___________ can be explained by referencing equations to show the equilibria

A

solutions of carboxylic acids, sulphur dioxide and carbon dioxide

133
Q

The _________ of a solution of ammonia or amines can be explained by referencing an equation showing the equilibrium

A

Weakly basic nature

134
Q

The weakly alkaline nature of a ___________ can be explained by referencing an equation showing the equilibrium

A

Solution of ammonia or amines

135
Q

The weakly alkaline nature of a solution of ammonia or amines can be explained by _______

A

referencing an equation showing the equilibrium

136
Q

What differs between weak acids and strong acids

A

pH values

Conductivity

Reaction rates

137
Q

What stays the same between weak acids and strong acids

A

The stoichiometry of the reactions

138
Q

What differs between weak bases and strong bases

A

pH values

Conductivity

Reaction rates

139
Q

What stays the same between weak bases and strong bases

A

The stoichiometry

140
Q

Acid dissociation constant symbol

A

Ka

141
Q

Acid dissociation equations

A

Ka = [H+] [A-] / [HA]

pKa = -log10 Ka

142
Q

Ka = [H+] [A-] / [HA]

pKa = -log10 Ka

A

Acid dissociation equation

143
Q

pH of a weak acid equation

A

pH = 1/2pKa - 1/2log10c

144
Q

pH = 1/2pKa - 1/2log10c

A

pH of a weak acid

145
Q

A soluable salt of a strong acid and a strong base dissolves in water to produce a ______

A

Neutral solution

146
Q

________ dissolves in water to produce a neutral solution

A

A soluable salt of a strong acid and a strong base

147
Q

A soluble salt of a weak acid and a strong base dissolves in water to produce an ______

A

Alkaline solution

148
Q

A ______ dissolves in water to produce an alkaline solution

A

soluble salt of a weak acid and a strong base

149
Q

A soluble salt of a strong acid and a weak base dissolves in water to produce an _______ solution

A

Acidic

150
Q

A soluble salt of a strong acid and a weak base dissolves in water to produce an __________

A

Acidic solution

151
Q

____________ dissolves in water to produce an acidic solution

A

A soluble salt of a strong acid and a weak base

152
Q

What does the name of a salt depend on

A

The acid and base used

153
Q

A buffer solution

A

One which the pH remains approximately constant when small amounts of acid, base or water are added

154
Q

A solution which the pH remains approximately constant when small amounts of acid, base or water are added

A

Buffer solution

155
Q

Acid buffer

A

A solution of a weak acid and one of its salts made from a strong base

156
Q

A solution of a weak acid and one of its salts made from a strong base

A

Acid buffer

157
Q

Action of acid buffer to keep pH constant

A

The weak acid provides H+ ions, these are removed by the addition of a small amount of base

The salt of the weak acid provides the conjugate base, which can absorb excess hydrogen ions produced by the addition of a small amount of acid

158
Q

Action of a basic buffer to keep pH constant

A

The weak base removes excess hydrogen ions,

and the conjugate acid provided by the salt supplies hydrogen ions when these are removed

158
Q

The weak acid provides H+ ions, these are removed by the addition of a small amount of base

The salt of the weak acid provides the conjugate base, which can absorb excess hydrogen ions produced by the addition of a small amount of acid

A

Action of acid buffer to keep pH constant

159
Q

The weak base removes excess hydrogen ions,

and the conjugate acid provided by the salt supplies hydrogen ions when these are removed

A

Action of basic buffer to keep pH constant

160
Q

Basic buffer

A

A solution of a weak base and one of its salts

161
Q

A solution of a weak base and one of its salts

A

Basic buffer

162
Q

In a ____________, the weak base removes excess hydrogen ions, and the conjugate acid provided by the salt supplies hydrogen ions when these are removed.

A

Basic buffer solution

163
Q

In a basic buffer solution, _______________, and the conjugate acid provided by the salt supplies hydrogen ions when these are removed.

A

The weak base removes excess hydrogen ions

164
Q

In a basic buffer solution, the weak base removes excess hydrogen ions, and _________________ when these are removed.

A

The conjugate acid provided by the salt supplies hydrogen ions

165
Q

Acid dissociation constant

A

pH = pKa - log10 [acid] / [salt]

166
Q

pH = pKa - log10 [acid] / [salt]

A

Acid dissociation contant

167
Q

Dissociation of indicators as weak acids

A

HIn (aq) + H2O (l) -> H+ (aq) + In- (aq)

168
Q

The acid indicator dissociation constant equation

A

Kin = [H+] [In-] / [HIn]

169
Q

In aqueous solution, what is the colour of an acid indicator

A

It is distinctly different from that of its conjugate base

170
Q

What is the colour of a indicator determined by

A

The ratio of [Hin] to [In-]

171
Q

The pH range over which a colour change occurs can be estimated by what expression

A

pH = pKin +- 1

172
Q

pH less than 7

A

Acidic, more H+ than OH-

173
Q

Conjugate acid

A

Substance left when the acid donates

174
Q

Substance left when the acid donates

A

Conjugate acid

175
Q

Conjugate base

A

Substances formed when a base accepted protons

176
Q

Substances formed when a base accepted protons

A

Conjugate base

177
Q

What does gene pH scale give a measurement of

A

Concentration of hydrogen ions in aqueous solutions

178
Q

Concentration of hydrogen ions in aqueous solutions

A

pH scale

179
Q

Acidic, more H+ than OH-

A

pH less than 7

180
Q

pH = 7

A

Neutral

Equal OH- to H+

181
Q

Neutral

Equal OH- to H+

A

pH = 7

182
Q

pH greater than 7

A

Less H+ than OH-

Alkaline

183
Q

Less H+ than OH-

Alkaline

A

pH greater than 7

184
Q

pH equation

A

pH = -logv10 [H]

185
Q

pH = -logv10 [H]

A

pH equation

186
Q

Degree of ionisation of acids

A

The ability of non ionised molecules to produce hydrogen ions

187
Q

The ability of non ionised molecules to produce hydrogen ions

A

Degree of ionisation

188
Q

The strength of an acid is related to its concentration

True or false

A

False

189
Q

Soluble base

A

Alkali

190
Q

Why is a soluble base called an alkali

A

It will produce hydroxide ions when in an aqueous solution

191
Q

Weak acids and bases dissociating

A

Do not fully dissociate

192
Q

Acid dissociation constant

A

Ka

193
Q

Ka

A

Acid dissociation constant

194
Q

What does Ka measure

A

The strength of an acid

195
Q

The higher the value of Ka,

A

The stronger the acid

196
Q

Ka equation

A
197
Q

pH for weak acids equation

A
198
Q
A

pH weak acids

199
Q

Strength of a salt solution depends on enzymes

A

The strength of the parent acid and base

200
Q

Equivalence point

A

The point in a titration where the amount of titrant added is enough to neutralise the solution completely

201
Q

The point in a titration where the amount of titrant added is enough to neutralise the solution completely

A

Equivalence point

202
Q

What does the shape of the rotation curve indicate

A

The type of titration

203
Q

What indicates the type of titration

A

The shape of the titration curve

204
Q

What does the vertical region of a titration curve show

A

Where there is a rapid change in pH

And

Equivalence point

205
Q

What happens at the equivalence point

A

Indicator changes colour

206
Q

Good indicator

A

When HIn (acid) is a distinctly different colour from In (conjugate base)

207
Q

When HIn (acid) is a distinctly different colour from In (conjugate base)

A

Good indicator

208
Q

What does the ratio of HIn : In determine

A

It’s colour

209
Q

When does a complete change occur

A

When the concentration of acid and conjugate base are equal

210
Q

When is a colour distinguished

A

When HIn and In differ by a factor of 10

211
Q

When HIn and In differ by a factor of 10

A

Colour is distinguished

AH Chemistry (8 decks)

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