Med Tech Exam Review - Clinical Chemistry:
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Terms in this set (134)
In the analytic technique of A. a half-cell, also called an electrode, is composed of a
potentiometry, a single metallic conductor surrounded by a solution of
comparison is made electrolyte. An electrochemical cell consists of two half-
between the voltage of cells. If two different kinds of half-cells are connected in
one half-cell connected to such a way as to make a complete circuit, a current will
another half-cell. It is flow because of the potential difference between the
customary that all half-cell two electrodes. The connection must be between the
potentials be compared to two electrolyte solutions, usually by means of a salt
the potential generated by bridge. The universally accepted standard half-cell with
a standard electrode. This which all other half-cells are compared is the hydrogen
standard electrode is: electrode, arbitrarily assigned a potential E of 0.000 volt
a. A hydrogen electrode
b. a calcium electrode
c. a potassium electrode
d. a copper electrode
e. an iron electrode
in an electrolytic cell, the B. oxidation involves the loss of electrons, and
half-cell where reduction reduction the gain of electrons. In an electolytic cell
takes place is known as the composed of two different half-cells - for example, zinc
a. anode in zinc sulfate and copper in copper sulfate - electrons
b. cathode will flow from the anode to the cathode. thus reduction
c. inidcating electrode takes place at the cathode
d. reference electrode
e. standard electrode
,mercury covered by a layer B. In practical applications of potentiometry, it is
of mercurous chloride in desirable to use one half-cell with a known and
contact with satruated constant potential that is not sensitive to the
potassium chloride solution composition of th ematerial to be analyzed. This is
is a description of which of called the reference electrode. One common reference
the following types of electrode is the calomel electrode, which consists of
electrodes? mercury covered by a layer of mercurous chloride in
a. antimony contact with a saturated solution of potassium chloride.
b. calomel The other half-cell, called the indicator electrode, is
c. hydrogen selected on the basis of the change in its potential with
d. quinhydrone change in the concentration of the analyte of interest
e. silver/silver chloride
C. for optimum performance, pH-sensitive glass
electrodes that are not actively in use should be kep
timmersed in an aqueous medium. Since the exact
when the pH-sensitive
composition of the pH-sensitive glass varies from one
glass electrode is not
manufacturer to another, the glass electrode should be
actively in use, it should be
maintained in the medium recommended by the
kept in
manufacturer. Usual media are water, dilute HCl, and
a. distilled or deionized
buffer with a pH near the pH of the solution to be
water
measured. The functioning of a glass electrode depends
b. physiologic saline
on the properties of the pH-sensitive glass. A typical
solution
glass electrode is made by sealing a thin piece of pH-
c. the medium
sensitive glass at the end of a piece of glass tubing and
recommended by the
filling the tube with a solution of hydrochloric acid
manufacturer
saturated with silver chloride. A silver wire is immersed
d. a buffer solution with a
in the solution in the tube with one end extending
pH near the pH of the
outside the tube for external connection. This is
internal solution in the
essentially a silver/silver chloride reference electrode
electrode
sealed within the tube with the pH-sensitive glass tip.
e. a buffer solution with a
This pH-sensitive glass functions appropriately only
pH near the pH at which
when it is saturated with water. Then eac surface of the
the electrode is to be used
glass develops a hydrated latice, where exchange of
alkaline metal ions in the lattice for hydrogen ions in the
test solution can occur
, C. colligative properties of a solution are those
properties that depend only on the number of particles
in solution, not on the nature of the particles. The
colligative properties are boiling point, freezing point,
osmotic pressure, and vapor pressure. Terms used to
describe the concentration of particles in solution are
Colligative properties of
osmole (the number of particles, 6.0224x10^23, that
solutions include all of the
lowers the freezing point 1.86C) and osmolal (the
following except:
concentration of 1 osm of solute per kilogram of water).
a. boiling point
One mole of an unionized solute dissolved in 1 kg of
b. freezing point
water lowers the freezing pont 1.86C. thus it is an
c. pH
osmolal solution. For un-ionized substances such as
d. osmotic pressure
glucose, 1 mol equals 1 osm. For substances that ionize,
e. vapor pressure
such as sodium chloride, werein each molecule in
solution becomes two ions and thus two particles, 1 mol
of sodium chloride theoretically equals 2 osm. In
practice, howerever, this is not always the case; an
osmotic activit coefficient factor is used to correct for
the deviation
, the freezing point D. the freezing point of an aqueous solution is lowered
osmometer is based on the 1.86C for every osmole of dissolved particles per
principle that kilogram of water. These particles may be ions, for
a. the freezing point example. Na+ and Cl-, or undissociated molecules such
depression is inversely as glucose. The freezing point osmometer is an
proportional to the amount instrument designed to measure the freezing point of
of solute in the solution solutions. It uses a thermistor that is capable of
b. the freezing point measuring very small changes in temperature
depression varies as the
logarithm of the
concenration of solute
c. the freezing point is
raised by an amount that is
inversely proportional to
the concentration of
dissolved particles in the
solution
d. the freezing point is
lowered by an amount that
is directly proportional to
the concentration of
dissolved particles in the
solution
e. there is no relationship
between freezing point
depression and the
concentration of dissolved
particles in the solution
the main advantages of C. Fluorescence occurs when a molecule absorbs light
fluorometric over of a particular wavelength and is thereby stimulated to
spectroscopic methods of emit light of a longer wavelength. The emitted light has
analysis are a characteristic spectrum, the emission spectrum, that is
a. decreased specificity unique for each fluorescing molecule. Hence,
and decreased sensitivity fluorometric methods are extremely sensitive and highly
b. decreased specificity specific. Becasue of this extreme sensitivity, reagents
and increased sensitivity used must be of a higher degree of purity than is
c. increased specificity and required for spectroscopy since even slight traces of
increased sensitivity impurities may fluoresce
d. increased specificity and
decreased sensitivity
e. ease of obtaining
suitable quality of reagents
Questions With Proven Solutions
Save
Terms in this set (134)
In the analytic technique of A. a half-cell, also called an electrode, is composed of a
potentiometry, a single metallic conductor surrounded by a solution of
comparison is made electrolyte. An electrochemical cell consists of two half-
between the voltage of cells. If two different kinds of half-cells are connected in
one half-cell connected to such a way as to make a complete circuit, a current will
another half-cell. It is flow because of the potential difference between the
customary that all half-cell two electrodes. The connection must be between the
potentials be compared to two electrolyte solutions, usually by means of a salt
the potential generated by bridge. The universally accepted standard half-cell with
a standard electrode. This which all other half-cells are compared is the hydrogen
standard electrode is: electrode, arbitrarily assigned a potential E of 0.000 volt
a. A hydrogen electrode
b. a calcium electrode
c. a potassium electrode
d. a copper electrode
e. an iron electrode
in an electrolytic cell, the B. oxidation involves the loss of electrons, and
half-cell where reduction reduction the gain of electrons. In an electolytic cell
takes place is known as the composed of two different half-cells - for example, zinc
a. anode in zinc sulfate and copper in copper sulfate - electrons
b. cathode will flow from the anode to the cathode. thus reduction
c. inidcating electrode takes place at the cathode
d. reference electrode
e. standard electrode
,mercury covered by a layer B. In practical applications of potentiometry, it is
of mercurous chloride in desirable to use one half-cell with a known and
contact with satruated constant potential that is not sensitive to the
potassium chloride solution composition of th ematerial to be analyzed. This is
is a description of which of called the reference electrode. One common reference
the following types of electrode is the calomel electrode, which consists of
electrodes? mercury covered by a layer of mercurous chloride in
a. antimony contact with a saturated solution of potassium chloride.
b. calomel The other half-cell, called the indicator electrode, is
c. hydrogen selected on the basis of the change in its potential with
d. quinhydrone change in the concentration of the analyte of interest
e. silver/silver chloride
C. for optimum performance, pH-sensitive glass
electrodes that are not actively in use should be kep
timmersed in an aqueous medium. Since the exact
when the pH-sensitive
composition of the pH-sensitive glass varies from one
glass electrode is not
manufacturer to another, the glass electrode should be
actively in use, it should be
maintained in the medium recommended by the
kept in
manufacturer. Usual media are water, dilute HCl, and
a. distilled or deionized
buffer with a pH near the pH of the solution to be
water
measured. The functioning of a glass electrode depends
b. physiologic saline
on the properties of the pH-sensitive glass. A typical
solution
glass electrode is made by sealing a thin piece of pH-
c. the medium
sensitive glass at the end of a piece of glass tubing and
recommended by the
filling the tube with a solution of hydrochloric acid
manufacturer
saturated with silver chloride. A silver wire is immersed
d. a buffer solution with a
in the solution in the tube with one end extending
pH near the pH of the
outside the tube for external connection. This is
internal solution in the
essentially a silver/silver chloride reference electrode
electrode
sealed within the tube with the pH-sensitive glass tip.
e. a buffer solution with a
This pH-sensitive glass functions appropriately only
pH near the pH at which
when it is saturated with water. Then eac surface of the
the electrode is to be used
glass develops a hydrated latice, where exchange of
alkaline metal ions in the lattice for hydrogen ions in the
test solution can occur
, C. colligative properties of a solution are those
properties that depend only on the number of particles
in solution, not on the nature of the particles. The
colligative properties are boiling point, freezing point,
osmotic pressure, and vapor pressure. Terms used to
describe the concentration of particles in solution are
Colligative properties of
osmole (the number of particles, 6.0224x10^23, that
solutions include all of the
lowers the freezing point 1.86C) and osmolal (the
following except:
concentration of 1 osm of solute per kilogram of water).
a. boiling point
One mole of an unionized solute dissolved in 1 kg of
b. freezing point
water lowers the freezing pont 1.86C. thus it is an
c. pH
osmolal solution. For un-ionized substances such as
d. osmotic pressure
glucose, 1 mol equals 1 osm. For substances that ionize,
e. vapor pressure
such as sodium chloride, werein each molecule in
solution becomes two ions and thus two particles, 1 mol
of sodium chloride theoretically equals 2 osm. In
practice, howerever, this is not always the case; an
osmotic activit coefficient factor is used to correct for
the deviation
, the freezing point D. the freezing point of an aqueous solution is lowered
osmometer is based on the 1.86C for every osmole of dissolved particles per
principle that kilogram of water. These particles may be ions, for
a. the freezing point example. Na+ and Cl-, or undissociated molecules such
depression is inversely as glucose. The freezing point osmometer is an
proportional to the amount instrument designed to measure the freezing point of
of solute in the solution solutions. It uses a thermistor that is capable of
b. the freezing point measuring very small changes in temperature
depression varies as the
logarithm of the
concenration of solute
c. the freezing point is
raised by an amount that is
inversely proportional to
the concentration of
dissolved particles in the
solution
d. the freezing point is
lowered by an amount that
is directly proportional to
the concentration of
dissolved particles in the
solution
e. there is no relationship
between freezing point
depression and the
concentration of dissolved
particles in the solution
the main advantages of C. Fluorescence occurs when a molecule absorbs light
fluorometric over of a particular wavelength and is thereby stimulated to
spectroscopic methods of emit light of a longer wavelength. The emitted light has
analysis are a characteristic spectrum, the emission spectrum, that is
a. decreased specificity unique for each fluorescing molecule. Hence,
and decreased sensitivity fluorometric methods are extremely sensitive and highly
b. decreased specificity specific. Becasue of this extreme sensitivity, reagents
and increased sensitivity used must be of a higher degree of purity than is
c. increased specificity and required for spectroscopy since even slight traces of
increased sensitivity impurities may fluoresce
d. increased specificity and
decreased sensitivity
e. ease of obtaining
suitable quality of reagents
