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Chem II > Ch 16 Acids And Bases > Flashcards

Ch 16 Acids And Bases Flashcards

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1
Q

What are the properties of Acids?

A

1) Sour taste (like vinegar)
2) Ability to dissolve many metals
3) Ability to neutralize based
4) Change blue litmus paper red

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2
Q

What is a binary acid?

A

An acid with a proton (H+) attached to a nonmetal atom (i.e. H).

For example: HCl, HF

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3
Q

What are oxyacids?

A

Acids that have the proton (H+) attaches to an oxygen atom.

Fro example: H2SO4 or HNO3

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4
Q

What are the 2 main components of acid rain?

A

1) H2SO4 - Sulfuric acid

2) HNO3 - Nitric acid

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5
Q

What are monoprotic, diprotic, and triprotic acid?

A

1) Monoprotic - Acid with only 1 proton (H+). i.e. HCl
2) Diprotic - Acid with 2 protons (H+). i.e. H2SO4
3) Triprotic - Acid with 3 protons. i.e. H3PO4

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6
Q

What are the 6 Strong Acids?

A

1) HCl - Hydrochloric Acid
2) HBr - Hydrobromic Acid
3) HI - Hydroiidic Acid
4) HNO3 - Nitric Acid
5) HClO4 - Perchloric Acid
6) H2SO4 - Sulfuric Acid

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7
Q

What are Carboxylic Acids?

A

Organic acids with the group COOH attached to it. i.e.

1) H3C6H5O7 (Citric Acid) - Found In limes, lemons and oranges.
2) C4H6O5 (Malic Acid) - Found In grapes and apples.

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8
Q

What’s the acidic name for Vitamin-C?

A

Ascorbic Acid

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9
Q

What are the occurrences/uses for the following 3 Strong Acids?

1) Hydrochloric Acid (HCl)
2) Sulfuric Acid (H2SO4)
3) Nitric Acid (HNO3)

A

1) Hydrochloric Acid (HCl) - Stomach acid, metal cleaning, food preparation, ore refining.
2) Sulfuric Acid (H2SO4) - Fertilizer, explosives, dye, glue, car batteries, electroplating of copper.
3) Nitric Acid (HNO3) - Fertilizer, explosives, dyes, glues.

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10
Q

What are the occurrences/uses of the following 5 Weak Acids?

A

1) Acetic Acid (HC2H3O2) - plastic and rubber manufacturing, food preservation, active component of vinegar.
2) Citric Acid (H3C6H5O7) - Citrus fruits, used to adjust pH in foods and beverages.
3) Carbonic Acid (H2CO3) - Carbonated beverage
4) Hydrofluoric Acid (HF) - Metal cleaning, glass frosting and glass etching.
5) Phosphoric Acid (H3PO4) - Fertilizer, biological buffering, beverage preservation.

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11
Q

What are the 8 Strong Bases?

A

1) LiOH - Lithium Hydroxide
2) NaOH - Sodium Hydroxide
3) KOH - Potassium Hydroxide
4) RbOH - Rubidium Hydroxide
5) CsOH - Cesium Hydroxide
6) Ca(OH)2 - Calcium Hydroxide
7) Sr(OH)2 - Strontium Hydroxide
8) Ba(OH)2 - Barium Hydroxide

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12
Q

Which is the most corrosive acid learned in class?

A

HF - Hydrofluoric Acid

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13
Q

What are the properties of Bases?

A

1) Taste bitter
2) Feels slippery
3) Turns red litmus paper blue
4) Ability to neutralize acids

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14
Q

What’s the most common property of alkaloid plants?

A

Plant product that is alkaline is often poisonous.

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15
Q

What are the occurrences/uses of the following common bases?

1) Sodium Hydroxide (NaOH)
2) Potassium Hydroxide (KOH)
3) Sodium Bicarbonate (NaHCO3)
4) Sodium Carbonate (Na2CO3)
5) Ammonia (NH3)

A

1) Sodium Hydroxide (NaOH) - Petroleum processing, soap and plastic manufacturing.
2) Potassium Hydroxide (KOH) - Cotton processing, electroplating, soap production and batteries.
3) Sodium Bicarbonate (NaHCO3) - Baking Soda, antacid, source of CO2.
4) Sodium Carbonate (Na2CO3) - Glass and soap manufacturing, general cleanser, water softener.
5) Ammonia (NH3) - Detergent, fertilizer and explosives manufacturing, synthetic fiber production.

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16
Q

What is Arrhenius’ definition of an acid and a base?

A

1) Acid - Produces H+ in a solution

2) Base - Produces OH- in a solution

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17
Q

What is the Bronsted-Lowry definition of an acid and base?

A

1) Acid - H+ donor

2) Base - H+ Accepter

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18
Q

Give an example of a base according to the Bronsted-Lowry Definition that is not a base according to the Arrhenius definition.

A

NH3 (Ammonia) - It doesn’t produce OH-, but it accepts H+ to become NH4, which makes it a base according to Bronsted-Lowry.

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19
Q

Explain the Arrhenius Acid-Base Reactions

A

1) The H+ from the acid combines with the OH- from the base to make a molecule of H2O
2) The cation from the base combines with the anion from the acid to make a salt.

HCl(aq) + NaOH(aq) —> NaCl(aq)+ H2O(l)

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20
Q

Explain the Bronsted-Lowry Acid-Base Theory.

A
  • All Arrhenius Acid-Base are Bronsted-Lowry Acid/Base.
    1) Any reaction involving H+ transfer is an acid-base reaction.
    2) The Acid is the H+ donor, the base is an H+ acceptor.
    3) The Acid molecule donates an H+ to the base molecule.

HCl(aq) + H20(l) –> Cl-(aq) + H3O+ (aq)
NH3 + H2O NH4 + OH-

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21
Q

Define Amphoteric Substances. Give some examples.

A

Substances that can act either as an acid or a base because they have both a transferable H and an atom with lone-pair electrons.
i.e. H2O, HCO3-, HPO4^2-

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22
Q

Give an example of a reaction when water acts as a base an another where it acts as an acid.

A

1) HCl + H20 –> CL- + H3O+ (water as a base)

2) NH3 + H2O NH4 + OH- (water as an acid)

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23
Q

What are Conjugate Pairs?

A

When a base accepts a proton and becomes a conjugate acid or when an acid donates a proton and becomes a conjugate base they are considered conjugate pairs.

24
Q

How do conjugated pairs relate to each other as far as their strengths are considered?

A

1) The stronger the acid, the weaker the conjugated base.
2) The weaker the acid, the stronger the conjugated base.
3) The stronger the base, the weaker the conjugated acid.
4) The weaker the base, the stronger the conjugated acid.

25
Q

How does an acid’s/base’s strength relate to to its strength as an electrolyte?

A

1) A strong acid, is a strong electrolyte (all the acid molecules ionize).
2) A strong base is a strong electrolyte (All the base molecules form OH- ions, either through dissociation or reaction with water).
3) A weak acid is a weak electrolyte (only a small percent of the molecules ionize).
4) A weak base is a weak electrolyte (only a small percent of the base molecules form OH- ions).

26
Q

What are the names of the following acids?

1) HI
2) HCHO2
3) H2SO3
4) HClO2
5) HNO2
6) HC7H5O2
7) HClO
8) HCN
9) HCH5O

A

1) HI - Hydriodic acid
2) HCHO2 (HCOOH) - Formic acid
3) H2SO3 - Sulfurous acid
4) HClO2 - Chlorous acid
5) HNO2 - Nitrous acid
6) HC7H5O2 - Benzoic acid
7) HClO - Hypochlorous acid (bleach)
8) HCN - Hydrocyanic acid
9) HCH5O - Phenol

27
Q

How is an acid’s strength measured?

A

An acid’s strength is measured by the size of the equilibrium constant when it reacts with H2O (aka the acid ionization constant, Ka).
HA + H2O –> H3O + A

28
Q

How does an acid’s strength or a base’s strength relate to the ionization constant?

A

1) A small pKa/large Ka or small pKb/large Kb equals a strong acid or base (Ka&raquo_space;1).
2) A large pKa/small Ka or large pKb/small Kb equals a weak acid or base.

29
Q

What is the formula to calculate Ka of an Acid or Base?

A

Ka = {[H3O+][A-]}/[HA] or {[H+][A-]}/[HA]

Kb = {[BH+][OH-]}/[B]

30
Q

How are pKa and pKb calculated?

A

1) pKa = -log(Ka) , Ka = 10^-pKa

2) pKb = -log(Kb) , Kb = 10^-pKb

31
Q

What are the Ka and Pka for the following monoprotic weak acids at 25 degrees Celsius:

1) HClO2 - Chlorous acid
2) HNO2 - Nitrous acid
3) HF - Hydrofluoric acid
4) HCHO2 - Formic acid
5) HC7H502 - Benzoic acid
6) HC2H3O2 - Acetic acid
7) HClO - Hypochlorous acid
8) HCN - Hydrocyanic acid
9) HCH5O - Phenol

A

1) HClO2 - Chlorous acid: 1.1 X 10^-2; 1.96
2) HNO2 - Nitrous acid: 4.6 X 10^-4; 3.34
3) HF - Hydrofluoric acid: 6.8 X 10^-4; 3.17
4) HCHO2 - Formic acid: 1.8 X 10^- . 4; 3.74
5) HC7H502 - Benzoic acid: 6.5 X 10^-5; 4.19
6) HC2H3O2 - Acetic acid: 1.8 X 10^-5; 4.74
7) HClO - Hypochlorous acid: 2.9 X 10^-8; 7.54
8) HCN - Hydrocyanic acid: 4.9 X 10^-10; 9.31
9) HCH5O - Phenol: 1.3 X 10^-0; 9.89

32
Q

What is the Kb for the following weak bases at 25 degrees Celsius:

1) CO3^2 - Carbonate ion
2) CH3NH2 - Methylamine
3) C2H5NH2 - Ethylamine
4) NH3 - Ammonia
5) HCO3 - Bicarbonate ion (aka Hydrogen Carbonate)
6) C5H5N - Pyridine
7) C6H5NH2 - Aniline

A

1) CO3^2 - Carbonate ion: 1.8 X 10^-4
2) CH3NH2 - Methylamine: 4.4 X 10^-4
3) C2H5NH2 - Ethylamine: 5.6 X 10^-4
4) NH3 - Ammonia: 1.76 X 10^-5
5) HCO3 - Bicarbonate ion (aka Hydrogen Carbonate): 2.3 X 10^-8
6) C5H5N - Pyridine: 1.7 X 10^-9
7) C6H5NH2 - Aniline: 3.9 X 10^-10

33
Q

What is Autoionization?

A

Autoionization is when water acts with itself as an acid and a base to form ions.
H20 + H2O H3O + OH- (this can also be written as:)
H2O H + OH-

34
Q

What is the Ion Product Constant of Water?

A

It is the equilibrium constant for the auto ionization of water. It is represented by Kh and says that H3O and OH concentrations will always be the same number.
[H3O+] x [OH-] = Kw = 1 x 10^-14 at 25 deg celcius.

35
Q

Since all aqueous solutions contain both H3O+ and OH_ ions, describe the concentration amounts of H3O relative to the concentration amounts in the following types of solutions:

1) Neutral Solutions
2) Acidic Solutions
3) Basic Solutions

A

1) Neutral Solutions - Have equal [H30-] and [OH-];
[H30-] = [OH-] = 1 X 10^-7.
2) Acidic Solutions - Have a larger [H30-] than [OH-]; [H30-] > 1 x 10^-7 and [OH-] < 1 x 10^-7.
3) Basic Solutions - Have a larger [OH-] than [H3O+];
[H30-] < 1 x 0^-7 and [OH-] > 1 x 10^-7.

36
Q

How is pH and pOH calculated if given [H3O] and [OH]?

A 
pH = -log[H3O]
pOH = -log[OH-]
37
Q

Given pH or pOH, how is [H3O] or [OH-] calculated?

A 
[H3O+] = 10^-pH
[OH-] = 10^-pOH
38
Q

What is the value of pH + pOH?

A

14

39
Q

What happens when you add H30 to a strong acid as well as to H2O?

A

1) There will be two sources of H3O+: the acid and the water.
2) However, the contribution of H+ to H3O is negligible because the contribution of H30+ from the strong acid is so significant, it makes the contribution of H3O from water insignificant. Therefore,
[H3O]acid [HA]

40
Q

What are the steps in determining the pH of weak base?

A

1) Write the equation for the reaction, and use it as a guid to prepare the ICE Table: HA + H2O A + H3O+
2) Complete the ICE Table with the given info, keep in mind the stoichiometry for equilibrium concentrations.
3) Determine [H3O+] from the calculated value of x, and calculate pH as necessary.
4) Check answer.

41
Q

Define percent Ionization

A

It’s another way to determine/measure the strength of an acid; it represents the percentage of acid molecules that ionize when dissolved in water.
The higher the percent ionization, the stronger the acid.
Concentration of ionized acid = [H3O+]
%Ionization = ([Ionized Acid]/[Initial Concentration of Acid]) x 100

42
Q

How do you find the pH for a strong base?

A 
First find the [OH-], then calculate pOH or the pH. i.e.
Find the pH 0f 0.243M NaOH solution?
[NaOH] = 0.243 = [OH-]
pOH = -log 0.243 = 0.61
pH = 14 - 0.61 = 3.39
43
Q

How do you find the pH for a weak base such as NH3?

A

Follow the similar strategy of a weak acid by using the ICE Table.

44
Q

How can you easily tell if a Salt Solution will be an acidic, basic or neutral solution?

A

1) If the cation is a counter ion of a strong base and the anion is a conjugate base of a strong acid, it will form a neutral solution. i.e. NaCl, Ca(NO3)2, KBr.
2) If the cation is a countering of a strong base and the anion is a conjugate base of a weak acid, it will form a basic solution. i.e. NaF, Ca(C2H3o2)2, KNO2
3) If the cation is a countering of a weak base and the anion is the conjugate base of a strong acid it will form an acidic solution. i.e. Al(NO3)3, (NH4)2SO4

45
Q

What is a Binary Acid?

Describe the characteristics of the strengths of Binary Acids.

A

A binary Acid is an acid with only 2 elements i.e. HCl

1) Binary Acid strength increases to the right across a row. HF > HO > HN > HC
2) Binary Acid strength increases down the column i.e. HI > HBr > HCl > HF
3) The more polarized the bond, the more acidic the acid is.
4) The stronger the bond between the binary acid, the weaker the acid (bond strength increases as you go up and to the right of the periodic table).

46
Q

How do you calculate Polarity using electronegativity and how does polarity change when moving across the periodic table?

A

Polarity of a molecule equals the difference of their electronegativity. The more the electronegativity, the more polarized the molecule. i.e. O = 3.5 and H = 2.1; the electronegativity of H20 = 3.5 -2.1 = 1.4.
Electronegativity increases as you go up and to the right of the periodic table.

47
Q

What is an Oxyacid?

A

Oxyacids contain a hydrogen atom bonded to an oxygen atom. The oxygen atom is in turn bonded to another atom (which we call Y): H – O – Y

48
Q

What are the characteristics of Oxyacids?

A

1) Acidity of oxyacids increases up and to right across a periodic table.
2) The more electronegative the Y atom, the stronger the oxyacid: HClO > HBrO > HIO
3) The larger the oxidation number of the central atom, the stronger the acid. i.e. H2CO3 > H3BO3
4) The more oxygens attached to Y, the stronger the oxyacid: HClO4 > HClO3 > HClO2 > HClO

49
Q

What are the characteristics of the Lewis acid-Base Theory?

A

1) It focuses on transferring an electron pair
2) A Lewis acid is a lone pair (of electron) acceptor. H+, B in BF3; small, highly charged metal cations; atoms that are attached to highly electronegative atoms and have multiple bonds.
3) A Lewis base is a lone pair (of electron) donor. Anions are better Lewis Bases than neutral atoms or molecules. N- is better than N and S is better than O.
4) Arrhenius and Bronsted-Lowry acid-base reactions are also Lewis acid-base reactions.
5) Generally results in the formation of a covalent bond.

50
Q

What is an Adduct?

A

The product that forms in a Lewis acid-Base Reaction.

i.e. BF3 (lewis acid) + :NH3 (lewis base) –> F3B:NH3 (adduct)

51
Q

What percent of the fuels used in the US comes from the combustion of fossil fuels?

A

82%

52
Q

What are the three main components of Acid Rain?

A

1) H2CO3 - Carbonic Acid
2) 2H2SO4 - Sulfuric Acid
3) 4HNO3 - Nitric Acid

53
Q

How are the three main components of Acid Rain formed?

A

1) Combustion of fossil fuels produces CO2, which combines with water to produce Carbonic Acid.
CH4 + 2O2 –> CO2 + 2H2O&raquo_space;>
CO2 + H20 H2CO3
2) Natural fossil fuels contain Sulfur that burn to produce SO2 gas, which reacts with O2 to form SO3.
2SO2 + O2 –> 2SO3&raquo_space;>
2SO2 + O2 2H2SO4
3) The high temps of combustion allow N2, in the air to combine with O2 to form oxides of nitrogen.
N2 +2O2 –> 2NO2»>
4NO2 + O2 4HNO3

54
Q

Describe the Acid Rain Legislation we discussed in Class.

A

The 1990 Clean Air act - attacks acid rain by forcing utilities to reduce SO2.

55
Q

Which acid is inside vinegar?

A

CH3COOH (Acetic Acid) - can also be written as HC2H3O2.

56
Q

How does the initial concentration of a weak acid relate to the % ionization and the pH?

A

The smaller the concentration, the higher the % ionization and the higher the pH will be.

57
Q

What are the basic reactions when you mix an acid with water and a base with water?
HA + H2O = ?
HB + H2O = ?

A

HA + H2O H3O + A

HB + H2O = B + OH

Chem II (7 decks)

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