FINALS Flashcards
ACID PROPERTIES:
When dissolved in water, acids
- Conduct electricity
- Change blue litmus to red
- Have a sour taste
- React with bases to neutralize their properties
- React with active metals to liberate hydrogen
BASE PROPERTIES:
When dissolved in water, bases
- Conduct electricitv
- Change red litmus to blue
- Have a slippery feeling
- React with acids to neutralize their properties
classification of substances in terms of their behavior in water.
acid-base
is a substance with H in its formula that
dissociates to yield H3O
acid
is a substance with OH in its formula that dissociates to yield OH-
base
When an acid reacts with a base, they undergo
neutralization
is a substance that dissociates in aqueous medium to form yield hydronium ions, H3O+
arrhenius acid
dissociates completely into ions in water
strong acid
A _____ solution of a strong acid contains no HA molecules
dilute
A ______ acid dissociates slightly to form ions in water
weak
In a dilute solution of a weak acid, most HA molecules are _________.
undissociated
T or F | THE EXTENT OF DISSOCIATION FOR STRONG ACIDS
• There are no HA molecules in solution
The HA will turn into hydronium ion and an anion
True
Gaseous form of HCI -> called as
hydrogen chloride gas
When hydrogen chloride is aqueous or added to water, it becomes
Hydrochloric acid
THE EXTENT OF DISSOCIATION FOR WEAK ACIDS: Most HA molecules are _________.
undissociated
Weak acid: Majority will not be converted into individual ions, rather, around __ to ___% will not be converted
98-99%
Weak acid: Small part will be converted into ________ ion and anion when weak acid dissociates in water
hydronium ion
Stronger acids have more
H3O
Liberates hydrogen from hydrochloric acid ( strong or weak acid?). There’s a violent formation of bubbles
strong acid
If _______, then the acid is strong
Ka > 1
If ______, then the acid is weak
Ka < 1
If ______, then the base is strong
Kb > 1
If ______, then the base is strong
Kb > 1
If _____,thenthebaseisweak.
Kb<1
HCl
Strong acid
HBr
Strong acid
HI
Strong acid
HNO3
Strong acid
H2SO4
Strong acid
HClO4
Strong acid
HF
Weak acid
HCN
Weak acid
HClO
Weak acid
HNO2
Weak acid
RCOOH
Weak acid
Carboxylic acids
Weak acid
CH3OOH
Weak acid
C6H5OOH
Weak acid
oxoacids in which the number of O atoms exceeds the number of ionizable protons by two or more
Strong acids
acids in which H is not bonded to O or to a halogen
Weak acids
oxoacids in which the number of O atoms equals or exceeds the number of ionizable protons by one
Weak acids
water-soluble compounds containing O2- or OH- ions
Strong bases
M2O or MOH (M = Group 1A(1) metal (Li, Na, K, Rb, Cs)
strong base
MO or M(OH)2 (M = group 2A(2) metal (Ca, Sr, Ba)
strong base
ammonia (NH3)
Weak base
amines
Weak base
RNH2
Weak base
R2NH
Weak base
R3N
Weak base
AUTOIONIZATION OF WATER
Also called “___________”
self ionization of water or auto-dissociation of water
an ionization reaction in pure water or in an aqueous solution, in which a water molecule, H2O, deprotonates loses the nucleus of one of its hydrogen atoms) to become a hydroxide ion, OH-
AUTOIONIZATION OF WATER
The water molecule can act as a ____ or ____ Forming the conjugate acids and base
base or an acid
WATER IS
AMPHOTERIC
“__________” means the ability of a substance to react either as an acid or as a base.
Amphoteric
Water dissociates very slightlyaqinto ions oinaqan equilibrium process known as autoionization or
self-ionization
Kw= [H3O+][OH-] =
1.0x10^-14 (at 25° C)
[H3O+] = [OH-] =
1.0x10^-7 (at 25°C)
A change in ____ causes an inverse change in [OH-], and vice versa.
[H3O+]
In an acidic solution
[H3O+] > [OH-]
In a neutral solution
[H3O+] = [OH-]
In basic solution
[H3O+]<[OH-]
pH: In an acidic solution
pH < 7.00
pH: In a neutral solution
pH = 7.00
pH: In basic solution
pH > 7.00
The higher the pH, the lower the [H3O+] and the _____ acidic the solution.
less
____ and ____ scales express the acidity and basicity of dilute aqueous solutions
pH and pOH
It is known as the power of hydrogen or the measure of hydrogen ions H+ or hydronium ions [H3O+] concentrations
pH
It is the measure of hydroxide ion [OH-] concentration
pOH
pKw =
-log Kw
pKw =-log Kw
(= 14.0 at 25°C)
T or F| If [H3O] increases, [OH] decreases (and vice versa)
True
T or F| If pH increases, pOH decreases (and vice versa)
True
• These expressions are analogous to the expression for pH.
pKa and pKb
We derived it to express the concentration in a more convenient way using whole numbers
pKa and pKb
pKa =
-log Ka
pKb =
-log Kb
The ______ the value of pKa the stronger the acid
smaller
The ______ the value of pKb, the stronger the base.
smaller
An acid is a proton donor, any species that donates an H+ ion.
• An acid must contain H in its formula.
Brønsted-Lowry Acid-Base
A base is a proton acceptor, any species that accepts
an H+ ion.
• A base must contain a lone pair of electrons to bond to H+.
Brønsted-Lowry Acid-Base
An acid-base reaction is a proton-transfer process.
Brønsted-Lowry Acid-Base
__________acid is a substance that is a proton donor.
Brønsted-Lowry
_______base is a substance that is a proton acceptor.
Brønsted-Lowry
A _________________ reaction occurs when an acid and a base react to form their conjugate base and conjugate acid, respectively.
Brønsted-Lowry acid-base
The ___ direction of an acid-base reaction depends on the relative strength of the acids and bases involved.
net
A reaction will favor the formation of the ______ acid and base.
weaker
The stronger the acid is, the _____ its conjugate base.
weaker
- is called the acid-dissociation constant or the equilibrium constant for the dissociation of weak acid.
Ka
– is a measure of acid strength.
Percent Ionization
Percent Ionization formula =
concentration of ionized HA/original concentration of HA x 100%
is any species that donates an electron pair to form a bond.
Lewis base
is any species that accepts an electron pair to form a bond.
Lewis acid
donation and acceptance of an electron pair to form a covalent bond.
Lewis acid-base
Lewis acid is a substance that is an electron pair _______.
acceptor
Lewis base is an electron pair ____.
donor
Molecules that contain a polar multiple bond often function as
Lewis acids
A ______cation acts as a Lewis acid when it dissolves in water to form a hydrated ion
metal
