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Inorganic and Organic Chemistry > Acid Base Equilibria > Flashcards

Acid Base Equilibria Flashcards

1
Q

the degree of dissociation of weak acid and base is described by

A

Ka/Kb

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2
Q

General expression for Ka

A

= [P] / [R]

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3
Q

Whose definition is this

Acid – any substance that increase the H+ concentration of the solution or produces H+ in aqueous medium

A

Arrhenius

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4
Q

Whose definition is this

Base – substance that increases the OH- concentration or produces OH in aqueous medium

A

Arrhenius

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5
Q

𝐻𝐢𝑙 (π‘Žπ‘ž)β†’ 𝐻+(π‘Žπ‘ž)+πΆπ‘™βˆ’ (π‘Žπ‘ž)

what kind of acid is this

A

Arrhenius Acid

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6
Q

π‘π‘Žπ‘‚π» (π‘Žπ‘ž)β†’ π‘π‘Ž+(π‘Žπ‘ž) π‘‚π»βˆ’ (π‘Žπ‘ž)

what kind of base is this

A

Arrhenius base

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7
Q

Acid – proton (H+) donor

Whose definition of base is this

A

Bronsted-Lowry Acid

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8
Q

Base - proton (H-) acceptor

A

Bronsted-Lowry Base

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9
Q

contains one more H atom and one more + charge than the base that formed it; becomes more positive

A

Conjugate Acid

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10
Q

formed when proton is removed from an acid;

A

conjugate base

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11
Q

example of an amphoteric compound, can be an acid and base

A

water

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12
Q

Acid - electron pair acceptor

whose definition is this

A

Lewis

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13
Q

Base - electron pair donor

whose definition is this

A

Lewis

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14
Q

Identify the acid, base, conjugate acid (ca) and conjugate base (cb) in the following reaction:

H2C2O4 + HCO3- -> HC2O4- + H2CO3

A

➒Acid – H2C2O4
➒ Base – HCO3-
➒ Conjugate base – HC2O4-
➒ Conjugate acid– H2CO3

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15
Q

Identify the acid, base, conjugate acid (ca) and conjugate base (cb) in the following reaction:

S-2 + HNO3 -> HS- + NO3+

A

➒ Acid – HNO3
➒ Base – S-2
➒ Conjugate acid – HS-
➒ Conjugate base – NO3

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16
Q

Identify the acid, base, conjugate acid (ca) and conjugate base (cb) in the following reaction:

H2PO4- + HCrO4- -> H3PO4 +CrO4-

A

➒ acid – HCrO4-
➒ base – H2PO4-
➒ conjugate acid – H3PO4 +
➒ conjugate base - CrO4-

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17
Q

write the conjugate acid for the following:

HS-
HSO4

A

➒HS- : H2S
➒ HSO4 : H2SO4

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18
Q

Write the conjugate base for the following

➒ CH3COOH –
➒ HPO4-2 –

A

➒ CH3COOH – CH3COO-
➒ HPO4-2 – PO4-3

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19
Q

may be categorized into strong and weak depending on their degree of dissociation

A

acid and base

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20
Q

are completely ionized in solution

A

strong base/acid

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21
Q

only partially disassociated

A

weak base/acid

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22
Q

Example of Strong Acids

A

HClO4 - Perchloric Acid
HCL - Hydrochloric Acid
HBr - Hydrobromic Acid
HI - Hydroiodic Acid
HNO3 - Nitric Acid
H2SO4 - Sulfuric Acid

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23
Q

Give examples of strong bases

A

LiOH - Lithium Hydroxide
NaOH - Sodium Hydroxide
KOH - Potassium Hydroxide
Ca(OH)2 Calcium Hydroxide
Sr(OH)2 Strontium Hydroxide
Ba(OH)2 Barium Hydroxide

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24
Q

symbol for partial disassociation

25
the degree of dissociation of weak acid/base can be described through these
dissociation constant
26
acid dissociation constant
Ka
27
base dissociation constant
Kb
28
The ___ the value of Ka and Kb, the greater the dissociation
higher
29
determines the acidity or basicity of solutions
pH or pOH
30
formula to determine the pH
- log [H+]
31
formula to determine the pOH
- log [OH-]
32
pKw value
14
33
formula for Pkw
Pkw = pH + pOH
34
describe a reaction wherein water reacts with itself
H2O + H2O ⇔ H3O+ +OH-
35
Kw value
1.0x10^-14
36
how is pKw computed using Kw
-logKw
37
formula for hydronium ion given pH
10^-pH
38
formula of pH given the hydronium ion
-log [H3O+]
39
formula of pOH given concentration of OH
-log [OH-]
40
formula of OH given POH
10^-pOH
41
Kw (and pKw) will have ____ values at temperature other than 25oC
different
42
For strong acid since the acid is completely ionized, the concentration of the acid will also be the concentration of the
H+
43
and for the strong base the concentration of the based is considered the concentration of the -.
-OH.
44
Calculate the pH and pOH of the following strong acid and strong base: 0.150 M HCl 2. 0.298 M NaOH 3. 0. 415 M Mg(OH)2
0.150 M HCl - 𝑝𝐻=0.824,pOH = 13.18 2. 0.298 M NaOH = 𝑝𝑂𝐻=0.526, 𝑝𝐻=13.47 3. 0. 415 M Mg(OH)2 = 𝑝𝑂𝐻= 0.08, 𝑝𝐻=13.92
45
Determine the H+ and -OH of the following solution with the given pH values. a. Lemon pH = 2.3 b. Bleach = 12.0
a. [𝐻+]=5π‘₯10βˆ’3 𝑀 [𝑂𝐻]=2π‘₯10βˆ’12𝑀 b. [H+] 1π‘₯10βˆ’12𝑀 [𝑂𝐻]=0.01 𝑀
46
What is the pH of 6.5x10-5 M KOH (aq) at 25oC?
9.812
47
Write a balanced equation showing the H2PO4- ion can be either a Bronsted-Lowry acid or a Bronsted-Lowry base (you may use water to react with it).
𝐻2𝑃𝑂4βˆ’ (π‘Žπ‘ž) β‡Œπ»π‘ƒπ‘‚4βˆ’2(π‘Žπ‘ž)+ 𝐻+ (π‘Žπ‘ž)
48
Find the [OH-] and pH of the following solutions 0.25g of Ba(OH)2 dissolved in enough water to make 0.655 L of solution. Ba(OH) = 171.34 g/mol
OH = 0.004452 M pH = 11.65
49
The H+ concentration in a carbonated beverage is 4.7x10-5 M, what is the OH- concentration? (Kw = 1.0x10-14)
2.13 x 10^-10 M
50
Consider the following weak acid and base: CH3COOH β‡Œ CH3COO- (aq) + H+ (aq) Ka =1.8x10-5 input the values into the formula of Ka
1.8π‘₯10^βˆ’5 =[𝐻+][𝐢𝐻3𝐢𝑂𝑂𝐻]/[𝐢𝐻3πΆπ‘‚π‘‚βˆ’]
51
HCOO- (aq) + H2O (l) β‡Œ HCOOH (aq) + -OH (aq) Kb = 5.9x10-11 input the formula in Kb
5.9π‘₯10βˆ’11=[𝐻𝐢𝑂𝑂𝐻][𝑂𝐻]/[𝐻𝐢𝑂𝑂]
52
systems in which the rate of forward reaction equals the rate of the backward reaction.
equilibrium
53
Likewise only reactants and products in what sates are included in the expression of Ka and Kb
aqueous and gaseous
54
what states are not included in the expression of Ka and Kb
liquid and solid states
55
The disassociation of HClO is HClO (aq) β‡Œ ClO- (aq) + H+ (aq) Calculate the Ka of HClO using the following equilibrium concentrations: HCl = 0.100M, ClO = 5.3x10-5 M, H+ = 5.3x10-5 M.
πΎπ‘Ž=2.8π‘₯10βˆ’8
56
The disassociation of HNO2 is HNO2 (aq) β‡Œ NO2 (aq) + H+ (aq) Calculate the pH of HNO2 when 0.200M HNO2is allowed to come to equilibrium, Ka = 6.0x10-4 (hint: use ICE)
𝑝𝐻=1.959
57
Butyric acid HC4H7O2 , is responsible for the odor of rancid butter and cheese. Its Ka is 1.51x10-5. Calculate [H=] in solutions prepared by adding 13.5g of butyric acid in enough water to make 1.30L.
1.33π‘₯10βˆ’3=𝐻+
58
Find the [OH-] and pH of the following solutions 0.25g of Ba(OH)2 dissolved in enough water to make 0.655 L of solution.
OH = (2.3x10-3 M)(2) = 4.6x10-3 M pH = 11.7

Inorganic and Organic Chemistry (19 decks)

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