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gen chem 2 > acids and bases > Flashcards

acids and bases Flashcards

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1
Q

State the arrhenius definition

A

Acids produce hydrogen ions in aq solutions and bases produce hydroxide ions in aq solutions

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2
Q

State the bronsted-lowry definition

A

An acid is a proton donor and a base is a proton acceptor

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3
Q

According to the bronsted-lowry definition what are acidic protons often attached to

A

Oxygen
Halogens
Nitrogen atoms

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4
Q

According to the bronsted-lowry definition what do bases need

A

Lone pair electrons to act as a proton acceptor

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5
Q

Acids and bases occur as what

A

Acid-base pairs
Base –> conjugate acid
Acid –> conjugate base

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6
Q

What is ka

A

Acidity constant

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

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7
Q

Describe strong acids

A 
Most of acid is dissociated (ionized, strong electrolyte) 
Ka = large 
Equilibrium lies far right 
[H+]=[HA]initial 
A- much weaker base than H20
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8
Q

State strong acids

A 
HCl 
HI
HBR 
HNO3 
H2SO4 
HClO4
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9
Q

Describe weak acids

A

Ka = small
Equilibrium lies far left
[H+] < [HA]initial
A- much stronger base than a H2O

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10
Q

State weak acids

A

HF
CH3COOH (acetic acid)
HCOOH (formic acid)
HOOCCH2CCH2COOHCOOHOH (citric acid)

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11
Q

Describe relationship between acid and base conjugate pairs

A

Inverse relationship
Strong acid –> doesn’t react as base (spectator)
Weak acid –> weak base
Doesn’t react as acid –> strong base

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12
Q

What is water

A

Amphoteric

Acts as an acid or base

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13
Q

What is Kw

A

Ion product constant of water

Kw=[H3O+][HO-] = 1.0x10^-14 @ 25degrees c

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14
Q

What is Kw in neutral

A

[H30+]=[HO-] = x

Kw=x^2 –> x=1.0x10^-7

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15
Q

What is Kw in acidic

A

[H30+]>[OH-]

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16
Q

What is Kw in basic

A

[H30+] IS LESS THAN [OH-]

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17
Q

State relationship between H+ and pH

A

As [H+] increases pH decreases

As [H+] decreases or [HO-] increases pH increases

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18
Q

State formulas for the pH scale

A 
Kw=[H3O+][HO-] = 1.0x10^-14 
pH = -log [H+]
pOH = -log [HO-]
-logKw = -log [H+]-log[HO-] = 1.0x10^-14 
Pkw = pH + pOH / pH+pOH = 14.00
[H+]= 10^-pH
[pOH] = 10^-pOH
*2 decimal places, 2 sig figs*
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19
Q

State what percent dissociation is and the formula

A

Extent of ionization for a weak acid

%diss= (molarity of H+ at equil / initial concentration) x 100

20
Q

How is percent dissociation affected as weak acid becomes more dilute

A

Increases

21
Q

Formulas for pka, ka, kb and pkb

A
  • logpka=pka pka goes down ka goes up

- logpkb=pkb pkb goes down kb goes up

22
Q

State formula for Kb

A

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

23
Q

State strong bases

A 
LiOH 
KOH 
NaOH 
RbOH 
CsOH 
Mg(OH)2
Ca(OH)2
Ba(OH)2
Sr(OH)2
24
Q

State weak bases

A

Amines = ammonia, methylamine, ethylamine, aniline and pyridine
Hydroxylamines

25
Q

What are polyprotic acids

A

Molecules that have more than one acidic proton

26
Q

What is special about polyprotic acids

A

Product of 1st reaction = reactant of 2nd reaction

Each dissociation step has a Ka associated with it

27
Q

How to solve weak polyprotic acids

A

Must do 2 ice tables and carry down [H+] from first table

28
Q

How do we deal with something - x in acid base chemistry

A

Use 5% rule, approximation

If doesn’t work then use quadratic formula

29
Q

State the generalizations about WEAK polyprotic acids

A

All of [H+] comes from first dissociation step
Very little of HA- dissociates, assume [H+]=[HA-]
Concentration of [A2-]=ka2

30
Q

How to solve strong polyprotic acids

A

Don’t need ka1 –> first dissociation (first ice table) goes to completion
Concentration of H+ carries down to the second ice table

31
Q

What are salts

A

Ionic compounds that are products of acid-base neutralizations

32
Q

Which salts do not affect pH

A

Salts of the cations of strong bases

Salts of the anions of strong acids

33
Q

Which salt produces basic solutions

A

Salts containing cation (with neutral properties) and an anion that is the conjugate base of a weak acid

34
Q

Which salt produces acidic solutions

A

Salts containing anion (with neutral properties) and a cation that is the conjugate acid of a weak base

35
Q

State the relationship for any conjugate acid base pair

A

Inverse relationship between ka of acid and kb of base
Ka x Kb = Kw
PKa + PKb = 14.00

36
Q

What do highly charged metal ions form

A

Complex ions and produce acidic solutions

37
Q

What happens when both ions in a salt have acid-base properties

A

Competition between K’s
Ka>Kb pH < 7 acidic
Ka=Kb pH = 7 neutral
Ka is less than Kb ph is less than 7 = basic

38
Q

What are covalent oxides

A

They produce acidic solutions

SO3, SO2, CO2, NO2, etc

39
Q

What are ionic oxides

A

They produce basic solutions

CaO, K2O, etc

40
Q

What is the relationship between acidity and increasing electronegativity

A

Proportional

Acidity increases when going down a column in periodic table

41
Q

Describe hydrogen halides

A

Weak acid = strong bond

Strong acid = weak bond

42
Q

Describe oxyacids

A

Electron withdrawing effect (inductive) of electronegative atoms makes the O-H bond more acidic

43
Q

State lewis model definition

A

Lewis acid is an electron pair acceptor and a lewis base is an electron pair donor (Includes bronsted lowry acids and bases)
Lewis base = e- pair donor
Lewis acid = e- pair acceptor

44
Q

Acid-base properties of salts: neutral salts

A

Cation is neutral (alkali metal or alkaline earth metal)
Anion is conjugate base of a strong acid
Ex = NaCl, KNO3

45
Q

Acid-base properties of salts: basic salts

A

Cation is neutral (alkali metal or alkaline earth metal)
Anion is conjugate base of a weak acid
Ex = CH3COOHNa, NaCN

46
Q

Acid-base properties of salts: acidic salts

A

Cation is conjugate acid of a weak base (or highly charges metal cation)
Anion is the conjugate base of a strong acid
Ex = NH4Cl, AlCl3

gen chem 2 (7 decks)

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