ANALYTICAL CHEMISTRY Flashcards
A ____ only partially ionizes when dissolved in
water. H2CO3 is an example
weak electrolyte
The _____ of a Brønsted-Lowry base is the potential proton donator formed
when a Brønsted-Lowry base accepts a proton.
conjugate acid
An _____ solvent can act either as an acid or a base. Water is an example.
amphiprotic
_______ is self-ionization of a solvent to produce both
a conjugate acid and a conjugate base.
Autoprotolysis
The ________ states that the position of an
equilibrium always shifts in such a direction to relieve
an applied stress.
Le Châtelier principle
A ________ solvent is one in which a series of acids (or bases)
all dissociate completely. Water is an example since HCl
and HClO4 dissociate completely.
leveling
______ of a solution is defined as the number of moles
of a strong acid (or a strong base) that causes 1.00 L of a buffer
to undergo a 1.00-unit change in pH.
Buffer capacity
_______ is the process by which a solid phase forms and is carried out of
solution when the solubility product of a chemical species is exceeded.
Precipitation
_____________
is a process in which normally soluble compounds are carried out of solution during
precipitate formation.
Coprecipitation
_____ is a type of coprecipitation in which a compound is trapped within a
pocket formed during rapid crystal formation
Occlusion
_______ is also a type of
coprecipitation in which a contaminant ion replaces an ion in the crystal lattice
Mixed-crystal formation
________ is a process in which a precipitate is heated in the presence of the solution
from which it was formed (the mother liquor). It improves the purity and
filterability of the precipitate.
Digestion
In _____, the filtered solid precipitate is redissolved and reprecipitated.
Because the concentration of the impurity in the new solution is lower, the second
precipitate contains less coprecipitated impurity.
reprecipitation
The _______ describes a layer of solution containing sufficient excess
negative ions that surrounds a charged particle. This balances the
surface charge on the particle.
counter-ion layer
____ describes an unstable state in which a solution contains higher solute
concentration than a saturated solution. It is relieved by precipitation of
excess solute
Supersaturation
A ____ is an organic compound that contains two or more electron-donor
groups located in such a configuration that five- or six-membered rings are formed when
the donor groups complex a cation.
chelating agent
What variables can cause the pH range of an indicator
to shift?
Temperature, ionic strength, the presence of organic solvents,
and colloidal particles
_______are titrations based on the formation of precipitates with
standard solutions of silver nitrate. An example is the titration of a halide ion with silver
nitrate to form the isoluble silver halide
Argentometric titrations
A solution is basic if:
a. [OH-] > 0
b. [OH-] = 1x10-7M
c. [OH-] > [H+]
d. [OH-] > 1x10-7M
c. [OH-] > [H+]
Water at room temperature usually has a slightly acidic pH. This is largely attributed to what compound(s)?
a. Sulfuric acid
b. Dissolved metals
c. Carbonic acid
d. Nitric acid
c. Carbonic acid
When benzoic acid dissolves in water, it partially reacts with water and ionizes to form benzoate and hydronium ions. In this reaction, what is the conjugate acid?
a. Benzoate ions
b. Hydronium ions
c. Water
d. Benzoic acid
b. Hydronium ions
Define a salt in terms of acid and base.
a. A salt is a compound that follows Le Chatelier’s Principle in reactions with
other compounds.
b. All of these
c. A salt is a compound formed when the nucleus of a hydrogen tom enters a quantity of water.
d. A salt is a compound (other than water) produced by the reaction of an acid and a base.
d. A salt is a compound (other than water) produced by the reaction of an acid and a base.
When a can of soda is opened and CO2 is released to the atmosphere, what is the resultant pH of the soda?
a. Decreases
b. Increases
c. The same
d. Allthese
b. Increases
