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Chemistry 143 > Chapter 17 (Exam 2) > Flashcards

Chapter 17 (Exam 2) Flashcards

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1
Q

Acids (General Characteristics)

A

Sour taste, ability to dissolve many metals; ability to turn blue litmus paper red; neutralize bases

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2
Q

Common Acids

A
  • Hydrochloric (HCl) - Sulfuric (H2SO4) - Nitric (HNO3O) - Acetic (HC2H3O2) - Citric (H3C6H5O7) - Carbonic (H2CO3) - Hydrofluoric (HF) - Phosphoric (H3PO4)
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3
Q

Carboxylic Acid

A

Contains: ((O)) H - O - C - R

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4
Q

Bases (General Characteristics)

A

Bitter taste, slippery feel (react to oils to form soap-like substance); turn red litmus paper blue; ability to neutralize acids

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5
Q

Alkaloids

A

Organic bases found in plants (often poisonous)

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6
Q

Common Bases

A
  • Sodium Hydroxide (NaOH) - Potassium hydroxide (KOH) - Sodium bicarbonate (NaHCO3) - Sodium carbonate (Na2CO3) - Ammonia (NH3)
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7
Q

Arrhenius Definition: - Acid - Base - Acid + Base = ?

A
  • Acid: Substance that produces H+ ions in aqueous solution –> H+ ions ALWAYS associate with H2O molecules to form hydronium ions (H3O+) –> Strong Acid: Completely ionizes in solution (weak: partially) - Bases: Substance that produces OH- ions in aqueous solution –> Strong Base: Completely dissociates in solution (weak: produces OH- by accepting proton from water/ionizing) - Acid + Base = Water
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8
Q

Bronsted-Lowry Definition: - Acid - Base

A
  • Acid: Proton (H+) donor - Base: Proton (H+) acceptor - Acids + Bases always occur together
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9
Q

Amphoteric

A

Substances that can act as acids or bases

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10
Q

Conjugate Acid/Conjugate Base

A
  • Any base to which a proton has been added - Any acid from which a proton has been removed NH3 (base) + H2O (acid) –> NH4+ (conj. acid) + OH- (conj. base) - Base accepts proton and becomes conjugate acid - Acid donates proton and becomes conjugate base
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11
Q

Binary Acids: Factors that Affect Ease of H+ Donated

A
  • Factors influencing ease of H+ donated are polarity and strength - Increasing Electronegativity: Increasing Acidity Decreasing Strength: Increasing Acidity
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12
Q

Oxyacids

A
  • Contain H bonded to O atom H - O - H - Y (branch off in diff. directions) - Influence acidity: Electron of Y (increasing electronegativity = weakening polarizing H-O bond–more acidic) - Number of O atoms bonded to Y: Draw electron density away from element Y (more = stronger acid)
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13
Q

Monoprotic Acid

A

Only one ionizable proton

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14
Q

Diprotic Acid

A
  • Two ionizable protons
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15
Q

Strong Acids

A
  • Hydrochloric (HCl) - Hydrobromic (HBr) - Hydroiodic (HI) - Nitric (HNO3) - Perchloric (HClO4) - Sulfuric (H2SO4) – Diprotic acid
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16
Q

Weak Acids

A
  • Hydrofluoric (HF) - Acetic (HC2H3O2) - Formic (HCHO2) - Sulfurous (H2SO3) - Carbonic (H2CO3) - Phosphoric (H3PO4)
17
Q

Generic Equilibrium Constant for Acid

A

HA (aq) + H2O –>/<– H3O+ + A-

HA (aq.) –>/<– H+ (aq) + A- (aq)

Ka = [H3O+][A-]/[HA]

Ka = [H+][A-]/[HA]

18
Q

Water: Basicity and Acidity

A
  • Water is amphoteric; when pure acts as an acid and a base itself

H2O + H2O –>/<–H3O+ + OH-

  • Kw = [H+][OH-]
  • Acidic: [H3O+] > [OH-]
  • Basic: [OH-] < [H3O+]
  • Kw = 1.0 x 10-14 at 25˚C
19
Q

Calculating pH

A
  • log[H3O+]
  • [H3O+][OH-] = 1.0 x 10-14

(then use negative log of hydronium ions)

20
Q

Finding [H3O+] and pH of Strong Acids

A
  • Completely ionize, therefore concentration of H3O+ = concentration of the stron gacid
  • Then -log(H3O+)
21
Q

Finding [H3O+] and pH of Weak Acids

A
  • Solve equilibrium problem
  • Write out entirety of equation; solve ICE equilibrium problem
  • Remember: HA (aq) + H2O (aq) –>/<– H3O+ (aq) + A- (aq)
  • Use x is small approximation; check and make sure that percentage is []
22
Q

Quadratic Equation

A

[- b +/- (b2 - 4ac)-2]/2a

from: ax2 + bx + c

23
Q

Percent Ionization (Acids)

A
  • Find concetration of hydronium ions
  • Divide molarity of hydronium ions by initial molarity and multiply by 100%
24
Q

Trends in Acids

A
  • Equilibrium H3O+ concentration of weak acid increases with initial increasing concentration of acid
  • Percent ionization of weak acid decreases with increasing concentration of acid
25
Q

Mixtures of Acids: Strong and Weak

Finding pH and [H3O+]

A
  • Relative strength of acids allows us to neglect weaker acid and focus on strong one
  • Solve equilibrium for strong acid and the products of the reaction
26
Q

Mixtures of Acids: Weak + Weak

Finding pH and [H3O+]

A
  • 3 potential sources of hydronium (two weak acids and water)
  • If Ka differs by factor of several 100s in magnitude, assume that weaker acid does not make contribution
  • Solve equilibrium equation with largest Ka initial and the products
27
Q

Common Strong Bases

A
  • Lithium hydroxide (LiOH)
  • Sodium hydroxide (NaOH)
  • Potassium hydroxide (KOH)
  • Strontium hydroxide [Sr(OH)2]
  • Barium hydroxide [Ba(OH)2]

–> Mostly group 1A or 2A metal hydroxides

—> 1A: Highly soluble and can form concentrated base solutions

–> 2A: Slightly soluble (dissocate in one step)

28
Q

Weak Bases/Common Weak Bases

A
  • Produce OH- by accepting proton from H2O; ionize H2O to form OH-
  • Carbonate ion (CO32-)
  • Methylamine (CH3NH2)
  • Ethylamine (C2H5NH2)
  • Bicarbonate ion (HCO3-)
  • Pyridine (C5H5N)
  • Aniline (C6H5NH2)

–> All are either ammonia or amines

29
Q

Weak Base Ionization Constant

A
  • Kb: Extent of ionization of weak base; smaller the constant, weaker the base
30
Q

Finding OH- of Strong Base Solutions

A
  • Concentration of OH- equals concentration of initial reactant; take -log(H3O+) to find pH (again, Kw = 1.0 x 10-14)
31
Q

Finding OH- and pH for Weak Base Solution

A
  • Write out equation, solve for ICE equilibrium problem
  • Use OH- x H3O+ = 1.0 x 10^-14 to find H3O+; then -log of hydronium!
32
Q

Anions as Weak Bases

A
  • View as conjugate base of an acid
  • General: A- = conjugate base of HA
  • Anion that is a conjugate base of weak acid is itself a weak base
  • Anion that is conjugate base of strong acid is pH-neutral
  • Cl- = HCl
  • F- = HF
  • NO3- = HNO3
  • C2H3O2 = HC2H3O2
33
Q

Kw = ?

A

Kw = Ka x Kb

pKa + pKb = 14

34
Q

Cations as Weak Acids

A
  • In some cases, act as weak acids
  • Cations and counterions of strong bases typically pH neutral
  • NH4+ (cation) = NH3 (base)
  • C2H5NH3+ = C2H5NH2
35
Q

Small, Highly Charged Cations

A
  • Smaller, more highly chared cation is, the more acidic its behavior
36
Q

Classifying Salt Solutions (4 Points)

A

1) Salts in which neither cation nor anion acts as and acid or base form pH-neutral solutions.
2) Salts in which cation does not act as an acid and anion acts as a base to form basic solutions.
3) Salts in which cation acts as an acid/anion does not act as a base forms acidic solutions.
4) Salts in which cation acts as an acid and anion acts as a base form solutions in which pH depends on relative strengths of acid/base

37
Q

Polyprotic Acids

A
  • Require more than one step to ionize
  • Ka2 is always smaller for polyprotic acids (second proton must separate from an anion)
38
Q

Concentrations of Anions for Weak Diprotic Acid Solution

(Concentration of X2-?)

A
  • General polyprotic (H2X)
    (1) H2X (aq) + H2O (l) –>/<– H3O+ (aq) + HX- (Ka1)
    (2) HX- (aq) + H2O (l) –>/<– H3O+ (aq) + X2- (aq) (Ka2)

Concentration X2-: Use equlibrium constant and solve for X2-

39
Q

Lewis Acids and Bases

  • Lewis Acid
  • Lewis Base
A
  • Electron pair acceptor
  • Electron pair donor

SUBSTANCE DOESN’T NEED TO CONTAIN H+ TO BE AN ACID

  • Molecules with incomplete octets act as acids
  • Some may reconfigure to act as Lewis Acids
  • Cations may act as Lewis acids as well….ugh.

Chemistry 143 (9 decks)

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