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Scott > Ch. 7 Acid, Bases & Equilibrium > Flashcards

Ch. 7 Acid, Bases & Equilibrium Flashcards

1
Q

Common Acids: Binary & Ternary Acids

HI = __________

HBr = _________

HCl = _________

HF = _________

A

HI = Hyroiodic acid

HBr = Hydrobromic acid

HCl = Hydrochloric acid

HF = Hydroflouric acid

fyi**: (adding H+ makes it an acid)

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2
Q

Common Acids: Binary & Ternary Acids

H2SO4 = ________

HNO3 = ________

H2CO3 = _______

H3PO4 = _______

A

H2SO4 = Sulfuric acid

HNO3 = Nitric acid

H2CO3 = Carbonic acid

H3PO4 = Phosphoric acid

  • fyi: (don’t* use hydro when naming ternary acids)
  • fyi**: (adding H+ makes it an acid)*
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3
Q

Common Bases: From Polyatomic ions

NaOH = ______

KOH = _______

Mg(OH)2 = ______

Ca(OH)2 = _______

CaCO3 = _______

Li2CO3 = _______

NaHCO3 = _______

Ca(HCO3)2 = ______

A

NaOH = Sodium Hydroxide

KOH = Potassium Hydroxide

Mg(OH)2 = Magnesium Hydroxide (milk of mag)

Ca(OH)2 = Calcium Hydroxide

CaCO3 = Calcium Carbonate

Li2CO3 = Lithium Bicarbonate

NaHCO3 = Sodium Bicarbonate

Ca(HCO3)2 = Calcium Bicarbonate

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4
Q

Acids Vs. Bases

Acids taste _______

Bases taste _______

Bases are also _______ to the touch.

A

Acids taste Sour

Bases taste Bitter

Bases are also Slippery to the touch.

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5
Q

Bronsted-Lowry Acids & Bases:

Acids _______ H+

Bases _______ H+

Acids are proton _______.

Bases are proton _______.

A

Acids release H+

Bases accept H+

Acids are proton donors.

Bases are proton acceptors.

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6
Q

Bronsted-Lowry Acids & Bases:

Define: Amphoteric

A

Amphoteric: Compounds that can act as acids or bases.

i.e: H2O

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7
Q

Bronsted-Lowry Acids & Bases:

Define: Conjugates

A

Conjugates: Compounds which differ only in the presence or absence of H+.

i.e: H2O & H3O+

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8
Q

Bronsted-Lowry Acids & Bases:

HCN + H2O ⇔ CN- + H3O+

Which are acids and which are bases?

What are the conjugate pairs?

A

HCN + H2O ⇔ CN- + H3O+

HCN: acid

H2O: base

CN-: base

H3O+= acid

Conjugate pairs: HCN/CN- & H2O/H3O+

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9
Q

Bronsted-Lowry Aids & Bases:

NH3 + H2O ⇔ NH4+ + OH-

Which are acids and which are bases?

What are the conjugate pairs?

A

NH3 + H2O ⇔ NH4+ + OH-

NH3 = base

H2O​ = acid

NH4+ = acid

OH- = base

Conjugate pairs: NH3/NH4+ & H2O​/OH-

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10
Q

Bronsted-Lowry Acids & Bases:

NH3 + H2O ⇔ NH4+ + OH-

What is the conjugate base of H2O acid?

A

NH3 + H2O ⇔ NH4+ + OH-

OH-

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11
Q

Equilibrium:

Define: Equilibrium

A

Equilibrium: The rate at which forward and reverse reactions are equal.

i.e: N2O4(g) ⇔ 2NO2(g)

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12
Q

Equilibrium:

Keq = _______

A

Keq = Equilibrium constant

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13
Q

Equilibrium:

Equilibrium constant values vary with _________.

Can a catalyst effect equilibrium or the value of Keq?

A

Temperature(25°C)

NO

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14
Q

Equilibrium Constant:

______ & _____ are NOT included in equilibrium equations.

A

Solvents(l) & Solids(s) are NOT included in equilibrium constant equations(Keq).

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15
Q

Equilibrium Constant:

aA + bB ⇔ cC + dD

Keq =

A

aA + bB ⇔ cC + dD

Keq = [C]c x [D]d / [A]a<strong> </strong>x [B]b

aA + bB ⇔ cC + dD

fyi: (lowercase = coefficiants from balanced equation)

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16
Q

Equilibrium Constant:

Balance the reaction and write the corresponding equilibrium constant expression.

CO(g) + O2(g) ⇔ CO2(g)

Keq =

A

2CO(g) + O2(g) ⇔ 2CO2(g)

Keq = [CO2]2 / [CO]2[O2]

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17
Q

Equilibrium Constant:

Balance the reaction and write the corresponding equilibrium constant expression.

C(s) + H2O(g) ⇔ CO(g) + H2(g)

Keq =

A

C(s) + H2O(g) ⇔ CO(g) + H2(g)

(balanced)

Keq = [CO][H2] / [H2O]

fyi: (solvents(l) & Solids(s) are NOT included in Keq.)

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18
Q

Equilibrium Constant:

Balance the reaction and write the corresponding equilibrium constant expression.

H2SO4(aq) + H2O(l) ⇔ HSO4-(aq) + H3O+(aq)

Keq =

A

H2SO4(aq) + H2O(l) ⇔ HSO4-(aq) + H3O+(aq)

(balanced)

Keq = [HSO4-][H3O+] / [H2SO4]

fyi: (solvents(l) & Solids(s) are NOT included in Keq.)

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19
Q

Ka values for selected acids:

Which of the following is stronger?

Ka = 2.5 x 1010

OR

Ka = 6.6 x 10-4

(Ka refers to acids, different than Keq)

A

Ka = 2.5 x 1010 is the stronger acid.

fyi: (larger values are stronger acids)

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20
Q

Ka values for selected acids:

Ka values are always at ____°C

21
Q

Ka values for selected acids:

Higher Ka value indicates a better _______ donor.

A

proton donor

22
Q

Acid(?) are ________

A

Aqueous

Acids(aq)

23
Q

Ionization of Water:

Kw = _________________

A

Kw = [OH-][H3O+] = 1.0 x 10-14

24
Q

Ionization of Water:

Kw is constant at ____°C.

25
Q

Ionization of Water:

[OH-] > [H3O+] = ______

[OH-] < [H3O+] = ______

A

[OH-] > [H3O+] = Basic

[OH-] < [H3O+] = Acidic

26
Q

Ionization of Water:

[OH-] = 8.4 x 10-3M

pH= 11.92

Calculate the [H3O+] and pH.

Acidic, basic, or neutral?

(explain steps)

A

1 x 10-14 / [OH-] = [H3O+]

[H3O+] = 1.19 x 10-12

pH = -Log([H3O+]​) = 11.92

11.92 = Basic

27
Q

Ionization of Water:

[H3O+] = 9.1 x 10-8M

pH = 7.0

Calculate the [OH-] and pH.

Acidic, basic, or neutral?

(explain steps)

A

1 x 10-14 / [H3O+] = [OH-]

[OH-] = 1.1 x 10-7

pH = -Log([H3O+]) = 7.0

7.0 = Neutral

28
Q

Ionization of Water:

How do you find the pH?

A

pH = -Log([H3O+])

29
Q

Ph Values:

pH has ____ sig figs after the decimal

30
Q

Ph Values:

Acidic / Basic / Neutral?

0 → 6.9 = _______

  1. 0 = ______
  2. 1 → 14.0 = ______
A

0 → 6.9 = Basic

  1. 0 = Neutral
  2. 1 → 14.0 = Acidic
31
Q

A ________ is a solution that resists large changed in pH when small amounts of acid or base are added.

32
Q

What makes a buffer solution?

A

A weak acid and its conjugate base

H2CO3(aq) and HCO3-(aq)

H2CO3(aq) + H2O(l) ⇔ HCO3-(aq) + H3O+(aq)

33
Q

Buffers are ______ acids.

34
Q

Le Châtelier’s Principle:

What happens when a reversible reaction is pushed out of equilibrium?

A

The reaction responds to reestablish equilibrium.

35
Q

Le Châtelier’s Principle:

What is one way to upset an equilibrium?

A

Varying the concentration of reactant or product.

36
Q

Le Châtelier’s Principle:

H2O(l) + CO2(g) ⇔ H2CO3(aq)

Increasing CO2 upsets the equilibrium and a net _______reaction takes place.

fyi: (upsets = changing concentration)

A

net forward reaction

37
Q

Le Châtelier’s Principle:

H2O(l) + CO2(g) ⇔ H2CO3(aq)

Decreasing CO2 upsets the equilibrium and a net _________ reaction takes place.

fyi: (upsets = changing concentration)

A

net reverse reaction

38
Q

Le Châtelier’s Principle:

H2O(l) + CO2(g) ⇔ H2CO3(aq)

Increasing H2CO3 upsets the equilibrium and a net ________ reaction takes place.

fyi: (upsets = changing concentration)

A

net reverse reaction

39
Q

Le Châtelier’s Principle:

For the equilibrium reaction below, predict which direction (forward or reverse) will be the faster one until equilibrium is reestablished when:

2SO2(g) + O2(g) ⇔ 2SO3(g)

a. SO2 is increased
b. SO3 is increased
c. SO2 is decreased
d. O2 is increased

A

a. Net forward reaction, SO3 increases

b. Net forward reaction

c. Net reverse reaction, SO3 decreases

d. Net forward reaction

40
Q

The pH of your blood normally ranges between _____ & _____.

How is this narrow range maintained?

A

7.35 & 7.45

With the help of buffers

41
Q

Blood pH below the normal range is called ________.

Blood pH above normal range is called _________.

A

acidosis

alkalosis

42
Q

The most important buffer system in the blood is formed from _________ and its conjugate base, HCO3- .

43
Q

Buffers in the blood: Two important equations

CO2(g) + H2O(l) ⇔ ___________

CO2(g) + H2O(l) ⇔ ___________________

A

CO2(g) + H2O(l) ⇔ H2CO3(aq)

CO2(g) + H2O(l) ⇔ HCO3-(aq) + H3O+(l)

44
Q

Acidosis & Alkalosis are potentially fatal! Why?

A

Adding OH- (base) = Loss of salt bridge due to OH- bonding w/ and forming H2O.

pH increases / H3O decreases

Adding H+ (acid) = Won’t allow NH3 and O- to bond. Forms and Carboxylic acid(no longer a protein) pH decreases / H3O increases

45
Q

The solution is alkaline = the solution is _______.

46
Q

Common Causes / Symptoms of:

Acidosis

A
  1. Lung disease, asthma
  2. Excessive alcohol consumption
  3. Ketosis / Starvation
  4. Holding your breath too long
  5. Hypoventilation (not enough CO2 is exhaled)
47
Q

Common Causes / Symptoms of:

Alkalosis

A
  1. Excessive use of antacids
  2. Anxiety, fever
  3. Hyperventilation (CO2 is blown off faster than it is produced in the cells.)
48
Q

Blood buffer (w/ help from organs):

Scott (26 decks)

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