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Inorganic and Organic Chemistry > Acid Base Equilibria > Flashcards

Acid Base Equilibria Flashcards

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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

𝐻𝐶𝑙 (𝑎𝑞)→ 𝐻+(𝑎𝑞)+𝐶𝑙− (𝑎𝑞)

what kind of acid is this

A

Arrhenius Acid

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6
Q

𝑁𝑎𝑂𝐻 (𝑎𝑞)→ 𝑁𝑎+(𝑎𝑞) 𝑂𝐻− (𝑎𝑞)

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

➢Acid – H2C2O4
➢ Base – HCO3-
➢ Conjugate base – HC2O4-
➢ 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

➢ Acid – HNO3
➢ Base – S-2
➢ Conjugate acid – HS-
➢ 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

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

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17
Q

write the conjugate acid for the following:

HS-
HSO4

A

➢HS- : H2S
➢ HSO4 : H2SO4

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18
Q

Write the conjugate base for the following

➢ CH3COOH –
➢ HPO4-2 –

A

➢ CH3COOH – CH3COO-
➢ 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

A

⇔

25
Q

the degree of dissociation of weak acid/base can be described through these

A

dissociation constant

26
Q

acid dissociation constant

A

Ka

27
Q

base dissociation constant

A

Kb

28
Q

The ___ the value of Ka and Kb, the greater the dissociation

A

higher

29
Q

determines the acidity or basicity of solutions

A

pH or pOH

30
Q

formula to determine the pH

A
  • log [H+]
31
Q

formula to determine the pOH

A
  • log [OH-]
32
Q

pKw value

A

14

33
Q

formula for Pkw

A

Pkw = pH + pOH

34
Q

describe a reaction wherein water reacts with itself

A

H2O + H2O ⇔ H3O+ +OH-

35
Q

Kw value

A

1.0x10^-14

36
Q

how is pKw computed using Kw

A

-logKw

37
Q

formula for hydronium ion given pH

A

10^-pH

38
Q

formula of pH given the hydronium ion

A

-log [H3O+]

39
Q

formula of pOH given concentration of OH

A

-log [OH-]

40
Q

formula of OH given POH

A

10^-pOH

41
Q

Kw (and pKw) will have ____ values at temperature other than 25oC

A

different

42
Q

For strong acid since the acid is completely ionized, the concentration of the acid will also be the concentration of the

A

H+

43
Q

and for the strong base the concentration of the based is considered the concentration of the -.

A

-OH.

44
Q

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

A

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
Q

Determine the H+ and -OH of the following solution with the given pH values.
a. Lemon pH = 2.3
b. Bleach = 12.0

A

a. [𝐻+]=5𝑥10−3 𝑀
[𝑂𝐻]=2𝑥10−12𝑀

b. [H+] 1𝑥10−12𝑀
[𝑂𝐻]=0.01 𝑀

46
Q

What is the pH of 6.5x10-5 M KOH (aq) at 25oC?

A

9.812

47
Q

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).

A

𝐻2𝑃𝑂4− (𝑎𝑞) ⇌𝐻𝑃𝑂4−2(𝑎𝑞)+ 𝐻+ (𝑎𝑞)

48
Q

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

A

OH = 0.004452 M
pH = 11.65

49
Q

The H+ concentration in a carbonated beverage is 4.7x10-5 M, what is the OH- concentration? (Kw = 1.0x10-14)

A

2.13 x 10^-10 M

50
Q

Consider the following weak acid and base:
CH3COOH ⇌ CH3COO- (aq) + H+ (aq) Ka =1.8x10-5

input the values into the formula of Ka

A

1.8𝑥10^−5 =[𝐻+][𝐶𝐻3𝐶𝑂𝑂𝐻]/[𝐶𝐻3𝐶𝑂𝑂−]

51
Q

HCOO- (aq) + H2O (l) ⇌ HCOOH (aq) + -OH (aq) Kb = 5.9x10-11

input the formula in Kb

A

5.9𝑥10−11=[𝐻𝐶𝑂𝑂𝐻][𝑂𝐻]/[𝐻𝐶𝑂𝑂]

52
Q

systems in which the rate of forward reaction equals the rate of the backward reaction.

A

equilibrium

53
Q

Likewise only reactants and products in what sates are included in the expression of Ka and Kb

A

aqueous and gaseous

54
Q

what states are not included in the expression of Ka and Kb

A

liquid and solid states

55
Q

The disassociation of HClO is
HClO (aq) ⇌ 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.

A

𝐾𝑎=2.8𝑥10−8

56
Q

The disassociation of HNO2 is
HNO2 (aq) ⇌ 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)

A

𝑝𝐻=1.959

57
Q

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.

A

1.33𝑥10−3=𝐻+

58
Q

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.

A

OH = (2.3x10-3 M)(2) = 4.6x10-3 M
pH = 11.7

Inorganic and Organic Chemistry (19 decks)

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