Ass

Front 1

What are the two general goals ofchemical analysis?

Back 1

identification, qualitification

Front 2

Major/minor component of a solution?

Back 2

Solvent/solute

Front 3

What type of errors can be minimized by makingrepeated measurements (a) while errors of this type cannot (b)?

Back 3

a) random errors

b) systematic errors

Front 4

(1) Are all salts electrolytes (a)? Are allelectrolytes salts (b)?

Back 4

Yes, no.

Front 5

Gravimetric and titrimetric methods are examplesof (a) and spectroscopy and chromatography examplesof (b) in chemical analysis

Back 5

a) classical or wet chemistry

b) instrumental

Front 6

The ionic strength of a solution dependson (a) and (b) for each ion present in the solution

Back 6

a) concentration

b) charge

Front 7

A polyprotic acid has more than one ____

Back 7

exchangable hydrogen atom

Front 8

A buffer solution contains a weak acid and

Back 8

the salt of the weak acid

Front 9

The buffer capacity is

Back 9

the measure of how well a solution resists a change in pH when a strong acid or base is added

Front 10

An amino acid in solution can exist inone of two forms as

Back 10

neutral or zwitterionic

Front 11

A reaction to be suitable for an analysis bytitration must

Back 11

be fast and have a large equilibrium constant (go to completetion)

Front 12

The transition range of an indicator correspondsto

Back 12

a 1:10 parts change in color as a minimal observation limit or pH=pka+-1

Front 13

At the equivalence point of anacid-base titration an indicator should have a pKa equal to

Back 13

the pH of the solution

Front 14

A multidentate ligand binds to a metal ionthrough

Back 14

multiple atoms or attachment sites

Front 15

A formation constant (stability constant) is the

Back 15

the equilibrium constant for reaction of a metal with a ligand

Front 16

In terms of the free energy for formation of ametal-chelate complex the main contribution arises from

Back 16

the increase in entropy

Front 17

The conditional formation constant is the

Back 17

equilibrium constant for metal complex formation at a given pH

Front 18

The equivalence point of a metal-EDTA titrationcorresponds to

Back 18

the metal concentration from dissociation of the metal complex in pM

Front 19

A redox reaction occurs by

Back 19

transfer of electrons

Front 20

A species is said to be oxidized when

Back 20

it loses electrons

Front 21

The electrode at which oxidation occurs in an electrochemical cell is the

Back 21

anode

Front 22

A species with a large positive standardreduction potential is

Back 22

an oxidizing reagent

Front 23

The reference electrode for the measurement ofstandard reduction potentials is the

Back 23

standard hydrogen electrode

Front 24

A salt bridge is required in a workingelectrochemical cell to

Back 24

offset the flow of electrons through a circuit by a counter flow of ions between the two parts of the galvanic cell

Front 25

A redox reaction has reached equilibrium whenthe potential of an electrochemical cell is

Back 25

0 volts

Front 26

In potentiometry an electrochemical cellcontains two electrodes identified by their function

Back 26

an indicator electrode and a reference electrode

Front 27

A glass electrode used to determine pH is anexample of

Back 27

an ion selective electrode

Front 28

A silver|silverchloride electrode is often used in potentiometric measurements as a

Back 28

reference electrode

Front 29

The selectivity coefficient of an electrodedescribes

Back 29

the relative response of the electrode to different species of the same charge

Front 30

Secondary electrodes (also called compoundelectrodes) work by

Back 30

surrounding a conventional electrode with a membrane to isolate or generate the analyte to which the electrode responds

Front 31

Prior to a redox titration the species to bedetermined must be

Back 31

in the same oxidation state

Front 32

An increase in entropy has what effect on areaction?

Back 32

favors the formation of products

Front 33

The free energy for a reaction is large andnegative. Does this mean the reaction is spontaneous(fast)?

Back 33

No, it indicates the reaction is favorable but says nothing about the rate of the reaction.

Front 34

A solubility product constant can describe thesolubility of what type of substance?

Back 34

A sparingly soluble electrolyte.

Front 35

Precipitation is the process by which ---- ?

Back 35

a solid is displaced from a solution from a chemical reaction or change in volume

Front 36

A protonic acid is described as -----?

Back 36

donates a proton to a base

Front 37

Bronsted-Lowry base is

Back 37

a proton acceptor (electron lone pair donor)

Front 38

A conjugate acid is ----?

Back 38

complementary form of a base in an equilibrium reaction

Front 39

What is an activity coefficient ?

Back 39

adjust an ideal solution to the behavior of a real solution

Front 40

In an ideal solution what is the standard form for the amount of electrolyte used in an equlibrium reaction?

Back 40

molarity