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CHM 1120 > Acids and bases > Flashcards

Acids and bases Flashcards

1
Q

What happens to the remainder on the product side of an acid gives away a proton?

A

it is a base

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2
Q

What are characteristics of strong acids and bases?

A

React 100%
Value of x is the size of initial concentration
Value of K is large
Equilibrium favours the product side so much there is effectively no reactant remaining, irreversible reaction

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3
Q

What are characteristics of weak acids and bases?

A

React less than 100%
X is relatively small
K value is smaller than 1
Equilibrium favours reactant side and there is a measurable amount of product
The larger the K value, the stronger the acid or base
Have a range of strengths based on their K values

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4
Q

Do strong acids have full, partial, or no ionization?

A

full

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5
Q

Do weak acids have full, partial, or no ionization?

A

partial because they have a measurable amount of product

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6
Q

Do very weak a ids have full, partial, or no ionization?

A

none because the lower the K value, the less HA reacts

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7
Q

The stronger the acid…

A

the weaker its conjugate base

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8
Q

The weaker the acid…

A

the stronger its conjugate base

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9
Q

The stronger the base…

A

the weaker the conjugate acid

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10
Q

The weaker the base…

A

the stronger its conjugate acid

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11
Q

What are middle strength acids and bases?

A

not super strong or super weak,
they can sometimes donate and accept electrons

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12
Q

Are very weak acids and bases spectator ions?

A

yes

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13
Q

What is the autoionization of water?

A

water can undergo a reaction with itself

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14
Q

What does it mean when water is amphoteric?

A

it can be both an acid or a base

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15
Q

What is the value of Kw?

A

Kw = [H3O][OH] = 1.0x10-14 at 25 degrees celsius

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16
Q

Are H3O and OH directly or inversely proportional?

A

inversely
If H3O concentration goes up, OH concentration goes down because they are equal to a constant number

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17
Q

Do acidic solutions have more H3O or OH?

A

H3O

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18
Q

Do basic solutions have more H3O or OH?

A

OH

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19
Q

What is the pH equation?

A

pH=-log[H3O+]

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20
Q

What is the pOH equation?

A

pOH=-log[OH-]

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21
Q

Is there any excess H3O or OH when the pH is neutral?

A

no

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22
Q

What kind of acid is it when Ka<1?

A

weak

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23
Q

What kind of acid is it when Ka>1?

A

strong

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24
Q

What kind of base is it when Kb<1?

A

weak base

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25
What kind of base is it when Kb>1?
strong
26
What happens to the base when it steal protons?
turns into its conjugate acid and forms OH
27
Are the Ka and Kb of weak acids and bases related to Kw for a conjugate acid-base pair?
yes
28
What is the Kw equation?
Ka x Kb = Kw
29
What is the value of Kw?
1.0 x 10^-14
30
What do salts contain?
either a weak acid or a weak base as the cation or anion
31
What is the pH of acidic salt?
less than 7
32
Do medium strength acids and bases have a Ka and a Kb?
yes
33
What are the strong acids?
HClO4, HI, HBr, HCl, H2SO4, HNO3, HClO3
34
What are the strong bases?
LiOH, NaOH, KOH, RbOH, CsOH, Ba(OH)2, Sr(OH)2, Ca(OH)2
35
Do conjugate bases of strong acids have base strength?
no
36
What are the conjugate bases of strong acids?
Cl, Br, NO3, HSO4, ClDo O4
37
Do conjugate bases of strong acids accept protons?
no
38
Do counterions strong bases have acid strength?
no
39
Do weak conjugate acids of strong bases donate protons?
no
40
What are the weak conjugate acids of strong bases?
Na, K, Li, Rb, Sr 2+, Ba 2+
41
What are polyprotic acids?
acids that have more than one acidic proton
42
What is diprotic?
2 acidic protons
43
What is triprotic?
3 acidic protons
44
What is polyprotic?
many acidic protons (used for anything greater than 2)
45
Are protons donated in successive stages?
yes
46
What happens to the acid strength of remaining protons after each proton is donated?
decreases
47
What is the Total [H3O] equal to?
[H3O]+[H3O]+[H3O]+...
48
What step is the majority of H3O made in?
first step
49
What is the common ion effect?
how equilibrium is affected when a conjugate product (common ion) is already present in the solution
50
What are buffer solutions?
solutions that resist pH change when strong acid or base is added
51
What are buffer solutions made from?
solutions that contain both an acid and a base
52
How do you create a solution with both an acid and a base?
you use conjugate acid/base pairs of weak acids/bases
53
What kind of concentration do typic buffer solutions have?
equal concentration of conjugate acids and bases
54
Do buffer solutions buffer at a specific pH?
yes
55
Can buffer solutions have a super strong acid or base? Why?
no because their conjugate is too weak
56
Do buffers resist pH changes?
yes
57
Is there more or less H3O when the Ka is larger?
more
58
Is there more or less H3O when the Ka is smaller?
less
59
What is the relationship in between ratio of weak acid to weak conjugate base and H3O?
direct
60
What happens to pH when the ratio of [HA]/[A] changes?
H3O changes which changes the pH
61
What is the Henderson-Hasselbalch equation?
pH = pKa + log[A]/[HA]
62
What is the pKa the starting point for?
buffer pH
63
What is the size of pH relative to pKa when [A]> [HA]
pH > pKa
64
What is the size of pH relative to pKa when [HA] > [A]?
pH < pKa
65
What are neutralization reactions?
reactions that involve strong acids and bases in which one or the other is neutralized (removed from the solution by complete reaction) irriversible reactions
66
What kind of pH do neutralization reactions have?
neutral
67
What do neutralization reactions make?
salt and water
68
What happens to the weak acid when H3O is added to a weak acid and a conjugate base?
weak acid gets bigger
69
What happens to the conjugate base when OH is added to a weak acid and a conjugate base?
conjugate base gets bigger
70
What is the buffer capacity?
amount of strong acid that can be added to a solution before the pH changes dramatically
71
What pH rand do buffers have the most buffering capacity in?
in a pH range of pKa ± 1
72
When do you do ICE charts and MICE charts?
Do ice charts when the reaction is reversible, do mice charts when reaction is irreversible Mice charts use initial moles Ice charts use initial molarity
73
How do you make a buffer solution?
1. Adding a salt of the conjugate acid or base to an existing solution of a weak acid or base -Add roughly the same amount of salt 2. Partial neutralization of a weak acid or base solution -Add less than the amount of strong acid/base solution because we want it to be partially neutralized -You get roughly equal amounts of conjugate acids and bases
74
How do you choose a pH when making a buffer solution?
Find a list of weak acid pKa values Choose a weak acid with a pKa +- 1 from your target pH
75
What is titration used to determine?
concentration of a solution by reacting it with a reagent of known concentration
76
When are reactants stoichiometrically equivalent?
at the equivalence point
77
What is the titration equation?
HX + B → BX + H2O
78
Does pH change as the volume increases?
yes
79
What is the equivalence point?
the point at which the reactants are stoichiometrically equivalent to each other -Moles of what you’re adding is the same as (or equivalent to ) what is in the beaker
80
What is the pH of a strong acid and strong base reaction?
7 because they cancel each other out
81
What is the end point?
the point at which a visual indicator changes colour -Colour change occurs when the reaction is complete
82
What are the four regions of a titration curve?
initial pH, buffer region, equivalence point, beyond the equivalence point
83
What is the initial pH?
no titrant added yet, pH is calculated by determining [H3O] at equilibrium
84
What is the buffer region?
solution that has been partially neutralized. Neutralization reaction produces the conjugate in amounts equal to that of the titrant added
85
What is the equivalence point?
solution that has been completely neutralized. Neutralization reaction has reacted all of the original substance so that none is left. All of the titrant was used during the reaction. Neutralization reaction produces a conjugate. pH is calculated from the equilibrium between a weak acid or base and water
86
What is beyond the equivalence point?
more titrant has been added than there are substances to react with. All original species have reacted, you are adding more strong base to solution that contains only the conjugate base (or stronger acid to a solution that contains only a conjugate acid). The pH is calculated based on the amount of excess titrant you have added beyond the equivalence point

CHM 1120 (5 decks)

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