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ANACHEM MIDTERMS > ELECTROCHEMISTRY > Flashcards

ELECTROCHEMISTRY Flashcards

1
Q

It is a weak oxidizing agent used primarily for the determination of strong reductants.

A

Iodine

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2
Q

It is a reagent decomposes on standing, and has been applied to the determination of water in numerous types of samples.

A

Karl Fischer reagent

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3
Q

T OR F: Cathode is the electrode at which an oxidation takes place

A

False

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4
Q

Is capable of making electrical energy through using the chemical energy that came from chemical reactions and chemical energy by using electrical energy as its power source.

A

Electrochemical cell

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5
Q

This is an external source of electrical energy for operation

A

Electrolytic cell

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6
Q

What is called a change from the color of the oxidized form of the indicator to the color of the reduced form requires a change of about 100 in the ratio of a reactant concentrations?

A

General Redox Indicator

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7
Q

Italian physicist, was the inventor of the first battery, the so-called voltaic pile.

A

Alessandro Volta

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8
Q

Consist of two conductors called electrodes immersed in an electrolyte solution?

A

Electrochemical Cell

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9
Q

Electrode at which an oxidation takes place

A

Anode

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10
Q

What is the best known specific indicator which forms a dark blue complex with triiodide ion?

A

Starch

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11
Q

Is the electrode potential when the activities of the
reactants and products are all unity

A

Standard Electrode Potential

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12
Q

It occurs when the red color of the iron(III)/thiocyanate complex disappears as a result of the significant decrease in the iron(III) concentration at the equivalence point.

A

END POINT

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13
Q

What are the two common reductants?

A

Iron (II)
Thiosulfate ion

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14
Q

It is substance that change color on being oxidized or reduced.

A

General Redox Indicators

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15
Q

An alternative to filtration is the use of _______. Wherein, the finely divided metal is held in a vertical glass tube through which the solution is drawn under a mild vacuum.

A

REDUCTOR

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16
Q

When _____ donates a proton, it became conjugate base capable of accepting a proton.

A

Acid

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17
Q

Electrochemical cell is composed of two conductors called?

A

electrodes

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18
Q

Electrons are transferred From one reactant to another

A

Oxidation/Reduction Reaction - AKA Redox Reaction

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19
Q

Has strong affinity to electrons (electrons acceptor)

A

Oxidizing Agent(Oxidant)

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20
Q

Donates Electron to other species

A

Reducing Agent(Reductant)

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21
Q

Oxidation/reduction reaction is analogous to ______ of acid/base reaction

A

Bronsted – Lowry Concept

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22
Q

When acid donates a proton, it became conjugate base capable of ______

A

accepting a proton.

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23
Q

When a reducing agent donates an electron, it becomes an oxidizing agent that can ______

A

accept an electron

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24
Q

Two Ways in Carrying Out an Oxidation/ Reduction Reaction

A
  1. direct contact in suitable container
  2. electrochemical cell
25
Q

piece of copper is immersed in a silver nitrate solution

A

Silver Tree Experiment

26
Q

widely used in electrochemistry to prevent mixing of the contents of the two electrolyte solutions making up electrochemical cells

A

Salt Bridge

27
Q

is the electrode at which reduction occurs Cathodic Reactions.

A

Cathode

28
Q

is the electrode at which an oxidation takes place Anodic Reactions

A

Anode

29
Q

Store electrical Energy

A

Galvanic (Voltaic) cells

30
Q

are usually made from several such cells connected in series to produce higher voltages than a single cell can produce.

A

Batteries

31
Q

Italian physicist, was the inventor of the first battery, the so-called voltaic pile.

A

Alessandro Volta

32
Q

Reactions at the two electrodes in such cells tend to proceed spontaneously and produce a flow of electrons from the anode to the cathode via an ____

A

external conductor

33
Q

one of the earliest galvanic cells to find widespread practical application
used in the mid-1800s to power telegraphic communication systems

A

The Daniell Gravity Cell

34
Q

Is the phase boundary between an electrode and its solution

A

Interface

35
Q

Is a reference state that allows us to obtain relative values of such thermodynamic quantities as free energy, activity, enthalpy, and entropy.

A

Standard State

36
Q

the standard state has the properties of an ideal gas but at one atmosphere pressure

A

For Gases

37
Q

the standard states are real states and are the pure substances at a specified temperature and pressure

A

For Pure Liquid and Solvents

38
Q

the standard state is a hypothetical state that has the properties of an infinitely dilute solute but at unit concentration (molar or molal concentration, or mole fraction)

A

For Solutes in Dilute Solution

39
Q

the standard state is a real state and is the pure solid in its most stable crystalline form

A

For Solid

40
Q

Used as the universal reference electrode
It is easy to conduct, reversible and highly reproducible
Typically a Gas Electrode

A

SHE(Standard Hydrogen Electrode) AKA Normal Hydrogen Electrode(NHE)

41
Q

Is the potential of a cell in which the electrode in question is the right-hand electrode and the standard hydrogen electrode is the left-hand electrode

A

Electrode Potential

42
Q

is an important physical constant that provides quantitative information regarding the driving force for a half-cell reaction.

A

standard electrode potential

43
Q

LIMITATIONS TO THE USE OF SEP

A

Use of Concentration Instead of Activities
Effects of Other Equilibria
Formal Potentials

44
Q

reacts rapidly and reversibly, its color change is pronounced, and its solutions are stable and easily prepared

A

Ferroin

45
Q

the color changes of true redox indicators are largely independent of the chemical nature of the analyte and titrant and depend instead on the changes in the electrode potential of the system that occur as the titration progresses

A

Specific Indicators

46
Q

is another specific indicator which may be used in the titration of iron(III) with solutions of titanium(III) sulfate.

A

Potassium Thiocyanate

47
Q

7 Auxiliary Reducing Reagents (ZACaLiN C Silver)

A

Zinc
Aluminum
Cadmium
Lead
Nickel
Copper
Silver (in the presence of Chloride ion)

48
Q

An alternative to filtration is the use of a _____

A

reductor

49
Q

has a diameter of about 2 cm and holds a 40- to 50-cm column of amalgamated zinc. Amalgamation is accomplished by allowing zinc granules to stand briefly in a solution of mercury(II) chloride

A

Jones reductor

50
Q

Auxiliary Oxidizing Reagents

A

Sodium Bismuthate (NaBiO3 )
Ammonium Peroxydisulfate (NH4 )2S2O8
Sodium Peroxide and Hydrogen Peroxide

51
Q

powerful oxidizing agent capable of converting manganese(II) quantitatively to permanganate ion

A

Sodium Bismuthate (NaBiO3 )

52
Q

is a sparingly soluble solid with a formula that is usually written as oxidations are performed by suspending the bismuthate in the analyte solution and boiling for a brief period

A

bismuth salt

53
Q

In acidic solution, it converts chromium(III) to dichromate, cerium(III) to cerium(IV), and manganese(II) to permanganate.

A

Ammonium Peroxydisulfate

54
Q

is a convenient oxidizing agent either as the solid sodium salt or as a dilute solution of the acid

A

Sodium Peroxide and Hydrogen Peroxide

55
Q

easily prepared from iron(II) ammonium sulfate (Mohr’s salt), or from the closely related iron(II) ethylenediamine sulfate (Oesper’s salt).

A

Iron(II) Solutions

56
Q

is a moderately strong reducing agent that has been widely used to determine oxidizing agents by an indirect procedure in which iodine is an intermediate.

A

Sodium Thiosulfate Ions

57
Q

are indefinitely stable, can be boiled without decomposition, and do not react with hydrochloric acid.
Dichromate ion is reduced to green chromium(III) ion.

A

Potassium dichromate

58
Q

This ion cannot be used with hydrochloric acid solutions unless special precautions are taken to prevent the slow oxidation of chloride ion that leads to overconsumption of the standard reagent?

A

Permanganate ion

ANACHEM MIDTERMS (5 decks)

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