Acid-bases Flashcards
any species that dissolves in aqueous solution to produce H+ ions
arrhenius acid
any species that dissolves in aqueous solution to produce OH ions
arrhenius base
any species that acts as a proton donor
bronsted-lowry acid
any species that acts as a proton acceptor
bronsted-lowry base
any species that accepts a pair of electrons
lewis acid
any species that donates a pair of electrons
lewis base
the species that is the acid with one proton lost
conjugate base
The species that is the base with one proton gained
conjugate acid
The stronger the base or acid, the ___ its conjugate is, and the weaker the base or acid, the __ its conjugate is
weaker, stronger
The definitions of acid-bases in order of most specific to general are ____, _____, and ___. Arrehenius definition is concerned with reactions that only occur in __ __. Bronsted-lowry and arrhenius definitions are concerned with __ __, and the lewis definition is concerned with ____ transfers. The ___ definition is the most common
arrhenius, bronsted-lowry, lewis, aqueous solutions, protons transfers, electron, bronsted-lowry
The higher the concentration of ___ ions the lower the pH, this is given by the equation ____
H+, pH = -log[H+]
The higher the concentration of ___ ions the lower the pOH. This is given by the equation ____
OH-, pOH = -log[OH]
The pH and pOH are the -_ concentrations of protons and hydroxide ions. The sum of pH and pOH is always __ for a solution at room temperature
log, 14
In a neutral solution, both the pOH and pH are ___. In an acidic solution, the pH is ___7, and the pOH is ___ than 7. In a basic solution the pH is ___7 and the pOH is ___ 7
7, <, >, >, <
describes the extent ot which a particular substance dissociates into its ions
dissociation constants
Ka is given by the equation:
ka = [H3O+][A-]/[HA]
kb is given by the equation
kb = [HB][OH]/[B]
The dissociation constant of water is defined as ____ and is ____ at 25°C. Because equal concentrations of __- and ___ dissociate from H2O, water has a __ pH and Kw = _______, or _______
kw, 1E-14, H+, OH-, neutral, [OH][H+], ka(kb)
The __ the pka the stronger the acid and the ___ its ability to donate protons. It is equal to ___
lower, greater, -log(Ka)
The lower the pkb, the __ the base and the greater its ability to ___ a proton. It is equal to ____
stronger, accept, -logkb
A strong acid is one where the ka is ___ 1 and is dissociates completely in water to form ___
> , H+
A strong base is one where kb ___ 1, and dissociates completely in water to form ______
> , OH-
Binary acids include __ ___ like __, ___, __ and ____. THe larger the __ __ of the halide, the more acidic the compound, and the ___ the bond between them
hydrogen halides, HI, HBr, HCl, HF, atomic radius, weaker
acids that contain oxygen are called ____. The more oxygen molecules there are, the more ____ the compound
oxoacids, acidic
The strength of an acid ___ as the stability of its conjugate base ___
increases, increases
For oxoacids that have the same number of oxygen atoms, the compound with the more ____ central atom will be a stronger acid. This is because the more electronegative atom will be more ___ when the acid loses a proton and acquires a ___ charge
electronegative, stable, negative
when a strong acid reacts with a strong base to produce water
neutralization reaction
Neutralization reactions go to ___ and the moles can be calculated using the equation ____
completion, M1V1 = M2V2
1 mole of ___+ ions neutralizes 1 mole of ___- ions
H, OH
The product of a neutralization reaction of acids and bases
salt
A strong acid and a weak base react to form a __ ___. A weak acid and a strong base form a ___ ___
acidic salt, basic salt
To determine whether a salt is acidic or basic, break the salt into its respective ___, then add ___ or ___. Whichever acid or base is stronger determines whether the salt is acidic or basic. If both are strong, the salt is __
ions, H, OH, neutral
If the basic salt includes a group ___ or group __ metal cation, the cation is neutral
I, II,
a solution that resists a change in pH when small amounts of acid or base are added to it
buffer
A buffer is made of a __ acid and __ base. The buffer works best when the acid and base and ___ are equal in ___
weak, weak, conjugates, concentration
Acidic buffers are made by combining a __ acid and a ____, in a ___ ratio. They can also be made with a weak acid and ___ base in a ___ ratio. They can also be made with a __ and a ___ acid in a __ ratio
weak, salt, 1:!, strong, 2:1, salt, strong, 2:1
Assume ___% ionization of weak acids and bases, and ____% ionization of strong acids, bases and ___
0, 100, salts
to make alkaline buffers you can combine a ___ base and a ___ in a 1:1 ratio. You can also use a ____ base and ___ acid in a 2:1 ratio. You can also use a __ and a strong base in a ___ ratio
weak, salt, weak, strong, salt, 2:1
The henderson-hasselbalch equation can be used to calculate the pH or pOH of a buffer and is given by ____.
pH = pka + log[A]/[HA]
A buffer is considered to be a buffer if it is _____ of the ___
+/-1. pka
___ is an experiment used to determine the unknown concentration of an acid or base by adding an acid or base of a __ __
titration, known concentration
the solution of unknown concentration
analyte
changes colour at the equivalence point
indicator
the solution of known concentration
titrant
The point at which the analyte has equal concentrations of OH and H; the point at which the amount of titrant added is just enough to neutralize the analyte solution
equivalence point
Indicators are ___ acids or base that are used to estimate the __ __ of an acid-base titration. You should pick one with a ___ close to the __ of the equivalence
weak, equivalence point, pka, pH
The ____ ____ point is seen when strong acids and weak bases are combined or when weak acids and strong bases are combined. It is the ___ of the __ ___, and is where ___
half equivalence point, midpoint, buffering region, pH = pKa
The volume of analyte needed to reach the equivalence point is given by the equation ____
N1V1 = N2V2
If a strong acid and base are added together, it should completely neutralize and the equivalence point should be a ___. If a strong acid and weak base are added, the equivalence point is ___ 7. If a weak acid and strong base are added the equivalence point is __7
7, <, >
____ acids and bases can donate or accept more than 1 H+ ion. These titration curves usually feature multiple __ __ and multiple __ __
polyvalent, buffering regions, equivalence points
