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Chemistry > Test 4 > Flashcards

Test 4 Flashcards

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1
Q

Acid-base buffer

A

A solution that resists changes in the pH when a small amount of either strong acid or strong base is added

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2
Q

common-ion effect

A

The sift in the position of an ionic equilibrium away from an ion involved in the process that is caused by the addition or presence of that ion

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3
Q

Henderson-Hasselbalch equation

A

An equation for calculating the pH of a buffer system.

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4
Q

buffer capacity

A

A measure of the ability of a buffer to resist a change in pH; related to the total concentrations and relative proportions of buffer components

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5
Q

buffer range

A

The pH range over which a buffer acts effectively

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6
Q

acid-base titration curve

A

A plot of the pH of a solution of acid versus the volume of base added to the solution

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7
Q

equivalence point

A

The point in a titration when the number of moles of the added species is stoichiometrically equivalent to the original number of moles of the other species

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8
Q

end point

A

The point in a titration at which the indicator changes color.

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9
Q

solubility-product

A

An equilibrium constant for a slightly soluble ionic compound dissolving in water.

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10
Q

complex ion

A

An ion consisting of a central metal ion bonded covalently to molecules and/or anions called ligands

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11
Q

ligand

A

A molecule or anion bonded to a central metal ion in a complex ion.

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12
Q

formation constant(Kf)

A

An equilibrium constant for the formation of a complex ion from the hydrated metal ion and ligands.

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13
Q

spontaneous change

A

A change that occurs by itself, that is , without an on going input of external energy.

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14
Q

entropy

A

A thermodynamic quantity related tot he number of ways the energy of a system can be dispersed through the motions of its particles

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15
Q

second law of thermodynamics

A

A law stating that a process occurs spontaneously in the direction that increases the entropy of the universe

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16
Q

third law of thermodynamics

A

A law stating that the entropy of a perfect crystal is zero at 0 K

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17
Q

standard molar entropy

A

The entropy of 1 mol of an ideal gas at standard temperature and pressure

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18
Q

standard entropy of reaction

A

The entropy change that occurs when all components are in their standard states

19
Q

free energy

A

A thermodynamic quantity that is the difference between the enthalpy and the product of the absolute temperature and the entropy: G= H-TS

20
Q

standard free energy of formation

A

The standard free energy change that occurs when 1 mol of a compound is made from its elements with all components in their standard states.

21
Q

coupling of reactions

A

The pairing of reactions of which one releases enough free energy for the other to occur

22
Q

adenosine triphosphate

A

A high energy molecule that serves most commonly as a store and source of energy in organisms

23
Q

electrochemistry

A

The study of the relationship between chemical change and electrical work

24
Q

electrochemical cell

A

A system that incorporates a redox reaction to produce or use electrical energy

25
Q

half-reaction method

A

A method of balancing redox reactions by treating the oxidation and reduction half-reactions separately

26
Q

voltaic cell

A

An electrochemical cell that uses a spontaneous redox reaction to generate electric energy

27
Q

electrolytic cell

A

An electrochemical system that uses electrical energy to drive a non spontaneous chemical reaction

28
Q

electrode

A

The part of an electrochemical cell that conducts the electricity between the cell and the surroundings

29
Q

electrolyte

A

A substance that conducts a current when it dissolves in water

30
Q

anode

A

The electrode at which oxidation occurs in an electrochemical cell. Electrons are given up by the reducing agent and leave the cell at the anode

31
Q

cathode

A

The elected at which reduction occurs in an electrochemical cell. Electrons enter the cell and are acquired by the oxidizing agent at the cathode.

32
Q

half-cell

A

A portion of an electrochemical cell in which a half-reaction takes place.

33
Q

salt bridge

A

An inverted U tube containing a solution of a non reacting electrolyte that connects the compartments of a voltaic cell and maintains neutrality by allowing ions to flow between compartments

34
Q

cell potential

A

The potential difference between the electrodes of an electrochemical cell when no current flows

35
Q

voltage

A

The potential difference between the electrodes of an electrochemical cell when no current flows

36
Q

electromotive force(emf)

A

The potential difference between the electrodes of an electrochemical cell when no current flows

37
Q

volt

A

The SI unit of electric potential: 1V= 1 J/C

38
Q

coulomb

A

The SI unit of electric charge. One coulomb is the charge of 6.242x1018 electrons; one electron posses a charge of 1.602x10-19C.

39
Q

standard cell potential

A

The potential of a cell measured with all components in their standard states and no current flowing

40
Q

standard electrode potential

A

The standard potential of a half-cell, with the half-reaction written as a reduction

41
Q

standard reference half-cell

A

A specially prepared platinum electrode immersed in 1M H+ through which H2 gas at 1atm is bubbled.

42
Q

Faraday constant

A

The physical constant representing the charge of 1mol of electrons: F= 96,485 C/mole e-

43
Q

Nernst equation

A

An equation stating that the voltage of an electrochemical cell under any conditions depends on the standard cell voltage and the concentrations of the cell components

44
Q

concentration cell

A

A voltaic cell in which both compartments contain the same components but at different concentrations

Chemistry (25 decks)

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