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Arrhenius acid
- substance that dissociates in water to produce hydrogen ions, H+
- HA<--> H+ + A-
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Arrhenius Base
- a substance that dissociates in water to produce hydroxide ions, OH-
- MOH<--> M+ + OH-
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Bronsted-Lowry Acid
sustance that can transfer H+; proton donor
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Bronsted-Lowry Base
sustance that can accept H+; proton acceptor
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Conjugate acid-base pairs
chemical species whose formulas differ only by one hydrogen ion, H+
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Due to __ of the H ion, it is actually __ by one or more __.
For our purpose, H+ is equivalent to __.
- high reactivity
- hydrated
- water molecules
- H30+
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True or False: H+ does not exist alone as H+
true: as H30+
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What is Bronsted Lowry Theory Acid reaction with water?
HA+H2O <--> H3O+ + A-
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What is Bronsted Lowry Theory Base reaction with water?
NH3 + H2O <--> OH- + NH4+
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Water is what?
aphoteric (amphoprotic): it can act as an acid or as a base and thus can react with itself
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How does water react with itself.
This is called the __ of water.
- 2 H2O <--> H3O+ + OH-
- autoionization
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How many water molecules dissociate when reaction with itself?
1 in 10 milllion
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With equal concentrations of reactants and products, what will be the direction of reaction?
from stronger to weaker, whether base or acid
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Weak acid
an acid that is only partially dissociated in water and is thus a weak electrolyte
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Lewis Acid
electron-pair acceptor; these are generally cations and neutral molecuels with vacant valence orbitals, such as Al3+, Cu2+, H+. BF3
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Lewis Base
electron-pair donor; these are generally anions and nuetral molecules with available pairs of electrons, such as H2O NH3, O2-
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The bond formed between a lewis acid and a lewis base is called a __.
coordinate bond
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Explain in depth the coordinate bond
when the bond is formed between one species that donates both pairs of electrons and the other donates none
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What is the ion-product constant for water
Kw= [H+][OH-]= 1.0 x 10^-14
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What is the relation between H+ and OH- in the constant for water
[H3O+]= [OH-]=1.0 x 10-7
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What happens if hte concentration of H3O+ goes up or OH- goes up?
the other one will go down to maintain equilibrium
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Acidic would be ?
H3O+ > OH-
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Neutral would be
H3O+ = OH-
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Basic would be
H3O+ < OH-
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What is the scale of pH?
logarithmic
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What happens when a solution gets more acidic?
pH gets smaller, while the concentration gets bigger
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pH values
- Basic >7
- Neutral =7
- Acidic < 7
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The pH of a solution is the __ of hte __.
- negative logarithm
- hydrogen ion concentration
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acid base indicator
a substance that changes color in a specifc pH range
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What do indicators exhibit?
pH dependent color changes because they are weak acids ahd have different colors in their acid and conjugate base forms
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Strong acids and bases
strong electrolytes that are assumed to ionize completely in water
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weak acids and bases
are weak electrolytes that ionize only to a limited extent in water
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Solutions of weak acids and bases contain __ and __.
- ionized
- nonionized species
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If an acid is strong, what
its conjugate base has no measurable strength
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__ is the strongest acid that can exist in aqueous solution
H3O+
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__ is the strongest base that can exist in aqueous solution
OH-
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Acid ionization constant
the equilibrium onstant for the ionization of an acid
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percent dissociation
- a measur eof the strength of an acid
- % dissociation= [H+]/[HA0] x 100
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Strong acids have __
Percent dissociation of a weak acid does what as it conncentration increases?
- higher percent dissociation
- decreases as its concentration increases
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base ionization constant
the equilibrium constant for the ionization of a base
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the ionization of weak bases is treated how?
the same way as the ionization of weak acids
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Base dissociation constant
kb= [BH+][OH-]/ [B]
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product of Ka and Kb
multiplying out the expressions for Ka and Kb equals Kw
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Salts that produce neutral solutions are
those formed from strong acids and strong bases
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salts that produce basic solutiosn are those formed from
weak acids and strong bases
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salts that produce acidic solutions are those formed from
strong acids and weak bases
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Ka > kb
the solution will contain more H30+ ions
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Ka < kb
the solution will contain an exces of OH- ions
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Ka = Kb
the solution will contain approx. equal concentrations
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What is the trend for acid strenghth for HnX?
increases with increasing polarity of HX bond and increasing size of X
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Explain the trend of acid strength for HnYO3.
it increases with incrasing electronegativity
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