Chapter 6 Flashcards

1
Q

acid

A

A substance that increases the concentration of H+ when added to water.

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2
Q

acidic solution

A

One in which the activity of H+ is greater than the activity of OH-

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3
Q

amine

A

A compound with the general formula RNH2, R2NH, or R3N, where R is any group of atoms.

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4
Q

ammonium ion

A

The ammonium ion is NH4+. An ammonium ion is any ion of the type RNH3+, R2NH2+, R3NH+, or R4N+, where R is an organic substituent.

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5
Q

aprotic solvent

A

One that cannot donate protons (hydrogen ions) in an acid-base reaction.

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6
Q

autoprotolysis

A

The reaction in which two molecules of the same species transfer a proton from one to the other.

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7
Q

base

A

A substance that decreases the concentration of H+ when added to water.

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8
Q

basic solution

A

One in which the activity of OH- is greater than the activity of H+.

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9
Q

Bronsted-Lowry acid

A

A proton donor.

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10
Q

Bronsted-Lowry base

A

A proton acceptor.

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11
Q

carboxylate anion

A

Conjugate base (RCO2-) of a carboxylic acid.

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12
Q

common ion effect

A

Occurs when a salt is dissolved in a solution already containing one of the ions of the salt. The salt is less soluble than it would be in a solution without that extra ion. An application of Le Chatelier’s principle.

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13
Q

complex ion

A

Historical name for any ion containing two or more ions or molecules that are each stable by themselves.

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14
Q

conjugate acid-base pair

A

An acid and a base that differ only through the gain or loss of a single proton.

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15
Q

coprecipitation

A

Occurs when a substance whose solubility is not exceeded precipitates along with one whose solubility is exceeded.

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16
Q

disproportionation

A

A reaction in which an element in one oxidation state gives products containing that element in both high and low oxidation states.

17
Q

endothermic reaction

A

One for which deltaH is positive; heat must be supplied to reactants for them to react.

18
Q

enthalpy change

A

The heat absorbed or released when a reaction occurs at constant pressure.

19
Q

entropy

A

A measure of the disorder of a substance.

20
Q

exothermic reaction

A

One for which deltaH is negative; heat is liberated when products are formed.

21
Q

hydronium ion

A

H3O+; What we really mean when we write H+.

22
Q

ion pair

A

A closely associated anion and cation, held together by electrostatic attraction. In solvents less polar than water, ions are usually found as ion pairs.

23
Q

Le Chatelier’s principle

A

If a system at equilibrium is disturbed, the direction in which it proceeds back to equilibrium is such that the disturbance is partly offset.

24
Q

Lewis acid

A

One that can form a chemical bond by sharing a pair of electrons donated by another species.

25
Q

Lewis base

A

One that can form a chemical bond by sharing a pair of its electrons with another species.

26
Q

ligand

A

An atom or a group attached to a central atom in a molecule. The term is often used to mean any group attached to anything else of interest.

27
Q

neutralization

A

Process in which a stoichiometric equivalent of acid is added to a base (or vice versa).

28
Q

polyprotic acid or base

A

Compound that can donate or accept more than one proton.

29
Q

protic solvent

A

One with an acidic hydrogen atom.

30
Q

salt

A

An ionic solid.

31
Q

saturated solution

A

One that contains the maximum amount of a compound that can dissolve at equilibrium.

32
Q

standard state

A

The standard state of a solute is 1 M and the standard state of a gas is 1 bar. Pure solids and liquids are considered to be in their standard states. In equilibrium constants, dimensionless concentrations are expressed as a ratio of the concentration of each species to its concentration in its standard state.