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Chemistry > Ch 18 & 19 > Flashcards

Ch 18 & 19 Flashcards

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1
Q

Strong Acids

A 
HCl
HBr
HI
HNO3
HClO4
H2SO4
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2
Q

Weak Acids

A 
HF
HCN
HNO2
H3PO4
H2CO3
CH3COOH
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3
Q

Strong Bases

A 
LiOH
NaOH
KOH
Ba(OH)2
Ca(OH)2
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4
Q

Weak Base

A

NH3

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5
Q

Arrhenius Acid

A

substance that produces H+ in solution

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6
Q

Arrhenius Base

A

substance that produces OH- in solution

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7
Q

net ionic equation for Strong Acid/base reaction

A

H+ + OH- –> H2O

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8
Q

Limitation of Arrhenius defition

A

doesn’t recognize role of solvent in ionization of solute

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9
Q

Bronsted-Lowry Acid

A

proton (H+) donor

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10
Q

Bronsted-Lowry Base

A

proton acceptor

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11
Q

conjugate acid base pair

A

differ ONLY in presence or absence of proton

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12
Q

3 main groups of acids

A

binary acids
oxoacids
carboxylic acids (organic acids)

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13
Q

binary acid

A

has H-X structure (HF, HCl, HBr, etc)

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14
Q

factors that determine relative strength of binary acids

A

bond strength
(stronger bond=weaker acid)
Polarity of bond
(more polar=stronger acid)

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15
Q

oxoacid

A

has H-O-Z structure

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16
Q

factors that determine relative strength of oxoacids

A

electronegativity of Z
(more electronegative=stronger acid)
number of O’s bonded to Z
(more O’s=stronger acid)

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17
Q

Carboxylic Acids

A

R-COOH structure

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18
Q

Factors that increase acid strength of organic acids

A 
substituent groups (R)
    (CH3COOH
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19
Q

amphoteric substance

A

can act as both an acid and a base (H2O)

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20
Q

Kw value & equation

A

1*10^-14

Kw={H+}[OH-}

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21
Q

Acid dissociation constant equation

A

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

22
Q

strong vs weak acid Ka & pKa

A

strong acid-larger Ka/smaller pKa

weak acid-smaller Ka/higher pKa

23
Q

types of strong acids

A

Hydrohalic

Oxoacids

24
Q

types of weak acids

A

hydrohalic
oxoacids
carboxylic acids

25
Q

types of strong bases

A

M2O/MOH (M=group 1 metal)

MO/M(OH)2 (M=group 2 metal)

26
Q

types of weak bases

A

Ammonia

Amines (RNH2)

27
Q

direction of equilibrium

A

towards weak acid/base side

28
Q

percent ionization equation

A

[H+]/[HA]

29
Q

Kb equation

A

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

30
Q

what salts yield neutral solutions?

A

salts of strong acid & strong base

31
Q

what salts yield acidic solutions?

A

salts of strong acid & weak base

32
Q

what salts yield basic solutions?

A

salts of strong base & weak acid

33
Q

how to determine if salt of a weak acid& weakbase will be acidic or basic

A

Ka>Kb acidic salt

Kb>Ka basic salt

34
Q

Lewis acid

A

an atom or molc that is an e- pair acceptor

35
Q

Lewis base

A

atom or molc that is an e- pair donor

36
Q

bond joining Lewis acid & Lewis base

A

coordination covalent bond

37
Q

buffer solution

A

pH changes only slightly when acid/base is added

38
Q

how buffer works

A

weak acid/base pair
weak acid neutralizes added base
weak base neutralizes added acid

39
Q

Henderson-Hasselbach Equation & use

A

pH=pKa + log [A-]/[HA] ( [base]/[acid] )

can be used for buffer solutions

40
Q

buffer capacity

A

amount of acid/base that a buffer can neutralize before its pH changes appreciably

41
Q

pH range for effective buffers

A

pKa +/- 1

42
Q

indicator

A

changes color based on pH of solution

43
Q

end point

A

point in titration when indicator changes color

44
Q

equivalence point

A

point in titration when moles of added species is stoichiometricly equal to starting moles of other species

45
Q

how acid-base indicators work

A

acid and base forms of the indicator have different colors

46
Q

acid base indicator pH equation

A

pH= pKin + log [in]/[Hin]

47
Q

best indicator for strong base/acid combo

A

bromthymol blue
(pH range of 6-8)
yellow to blue

48
Q

bromcresol green properties

A

4-6 pH range

yellow to blue

49
Q

solubility

A

maximum amount of a salt that will dissolve (g/mL or mol/L)

50
Q

Solubility product

A

Ksp

product of the molar concentrations

51
Q

how does pH affect solubility?

A

only affects basic salts

the higher the [H+], the more soluble

Chemistry (6 decks)

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