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CHEM 305 > Exam 2 Bold Words > Flashcards

Exam 2 Bold Words Flashcards

(63 cards)

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0
Q

Base

A

Substance that decreases the concentration of H3O+

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1
Q

Acid

A

Substance that increases the concentration of H3O+

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2
Q

Salt

A

Any ionic solid

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3
Q

Neutralize

A

Reaction between an acid and a base

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4
Q

Conjugate acid-base pair

A

Relation between acid and a base due to the gaining or loss of one H+

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5
Q

Autoprotolysis

A

One substance acts as both an acid and a base

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6
Q

Acidic

A

H+ concentration > OH- concentration

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7
Q

Basic

A

H+ concentration < OH- concentration

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8
Q

Strong acid/base

A

Completely dissociates in aqueous solution

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9
Q

Weak Acids

A

React with water by donating a proton to H2O

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10
Q

Acid Dissociation Constant

A

Ka

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11
Q

Weak Bases

A

React with water by abstracting (grabbing) a proton from H2O

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12
Q

Base hydrolysis constant

A

Kb

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13
Q

Carboxylic Acids

A

Weak acids

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14
Q

Carboxylate anions

A

Weak bases

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15
Q

Amine

A

Nitrogen-containing compound

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16
Q

pK

A

Negative log of an equilibrium constant

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17
Q

Buffer

A

Consists of a mixture of a weak acid and the conjugate base

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18
Q

Henderson-Hasselbalch equation

A

Tells the pH of a solution

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19
Q

How many H+ concentrations can be measured in a solution?

A

1

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20
Q

Why does a buffer resist changes in pH?

A

It does so because the strong acid or base is consumed by B or BH+

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21
Q

Indicator Error

A

Difference between the observed end point (color change) and the true equivalence point

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22
Q

Kjeldahl nitrogen analysis

A

Method for determining nitrogen in organic substances such as porteins

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23
Q

Polyprotic Acids

A

Those having more than one acidic proton

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24
Amino Acids
Building blocks of proteins containing an acidic carboxylic acid group, a basic amino group, and a variable substituent designated R group
25
Zwitterion
Structure remaining after an amino acid is formed with positive and negative sides
26
Hydrolyze
React with water
27
Amphiprotic
A molecule that can both donate and accept a proton
28
Ionic Atmosphere
The region of net positive charge around any particular anion
29
Activities
Concentration multiplied by the activity coefficient
30
Activity coefficient
Depends on ionic strength
31
Extended Debye-Huckel Equation
Used to calculate the activity coefficient of a given species
32
Charge Balance
Algebraic statement of electroneutrality --> The sum of positive charges in solution equals the um of the negative charges in solution
33
Redox Reaction
Electrons are transferred from one species to another
34
Oxidized
Loses electrons
35
Reduced
Gaining electrons
36
Oxidizing agent
Takes electrons from another substance and becomes reduced
37
Reducing agent
Gives electrons to another substance and becomes oxidized
38
Coulombs
Measure of electric charge (C)
39
Faraday Constant
9.649 X 10^4 C/mol
40
Electrode
Device to conduct electrons into or out of the chemicals involved in the redox reaction
41
Electroactive species
Molecule that can donate or accept electrons at an electrode
42
Electric potential
Measures the work that can be done when electrons move from one point to another
43
Volts
Measure of potential difference
44
Electrolysis
Chemical reaction in which we apply a voltage to drive a redox reaction that is not spontaneous and would not otherwise occur
45
Salt bridge
Place where ions migrate to maintain electroneutrality in each vessel
46
Cathode
Electrode at which reduction occurs
47
Anode
Electrode where oxidation occurs
48
Standard Reduction Potential
Each half-cell is measured by an experiment shown in idealized form
49
Standard Hydrogen Electrode
Standard electrode to compare all other standards to
50
Nernst Equation
Expresses the net driving force of a reaction
51
Indicator Electrode
Electrode that responds directly to the analyte
52
Reference Electrode
The half cell with a constant potential
53
Silver-silver chloride Electrode
Standard reference electrode used instead of hydrogen reference electrode
54
Saturated Calomel Electrode
Cell is saturated with KCl
55
Potentiometry
Use of voltage measurements to extract chemical information
56
Junction Potential
The voltage difference when two dissimilar electrolyte solutions are placed in contact
57
Ion-Selective Electrode
Responds preferentially to one species in a solution
58
Combination Electrode
Incorporating both the glass and reference electrodes in one body
59
Solid-state ion-selective electrode
Crystals of one substance doped with an impurity
60
Liquid-based ion-selective electrode
Ion-exchange equilibrium of analyte between the liquid ion exchanger and the aqueous solution gives rise to the electrode potential
61
Selectivity Coefficient
Response to X/Response to A | Measures interference of another ion when measuring response to ion A
62
Compound Electrode
Conventional electrode surrounded by a membrane that isolates the analyte to which the electrode responds

CHEM 305 (1 decks)

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