Chapter 6 Flashcards

1
Q

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

A

Acid

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2
Q

Equilibrium constant for the reaction of an acid with H2O

A

Acid dissociation constant, Ka

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3
Q

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

A

Acidic solution

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4
Q

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

A

Aprotic solvent

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5
Q

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

A

Autoprotolysis

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6
Q

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

A

Base

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7
Q

The equilibrium constant for the reaction of a base with H2O

A

Base hydrolysis constant, Kb

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8
Q

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

A

Basic solution

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9
Q

A proton (hydrogen ion) donor

A

Brønsted-Lowry acid

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10
Q

A proton (hydrogen ion) acceptor

A

Brønsted-Lowry base

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11
Q

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 surplus ion. An application of Le Châtelier’s principle

A

Common ion effect

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12
Q

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

A

Complex ion

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13
Q

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

A

Conjugate acid-base pair

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14
Q

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

A

Coprecipitation

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15
Q

Equilibrium constant for a reaction of the type M + mX ⇌ MXn

A

Cumulative formation constant, Bn; Overall formation constant, Bn

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16
Q

A reaction in which an element in one oxidation state gives products containing that element in both higher and lower oxidation states

A

Disproportionation

17
Q

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

A

Endothermic reaction

18
Q

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

A

Enthalpy change (ΔH)

19
Q

A measure of “disorder” of a substance

20
Q

For the reaction aA + bB ⇌ cC + dD, (Cc * Dd)/(Aa * Bb)

A

Equilibrium constant (K)

21
Q

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

A

Exothermic reaction

22
Q

The change in Gibbs free energy, ΔG, for any process at constant temperature is related to the change in enthalpy, ΔH, and entropy, ΔS, by the equation ΔG = ΔH - T ΔS, where T is temperature in kelvins. A process is spontaneous (thermodynamically favorable) if ΔG is negative

A

Gibbs free energy (G)

23
Q

H+ (aq) or H3O+

A

Hydronium ion

24
Q

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

25
If a system at equilibrium is disturbed, the direction in which it proceeds back to equilibrium is such that the disturbance is partially offset
Le Châtelier’s principle
26
One that can form a chemical bond by sharing a pair of electrons donated by another species
Lewis acid
27
One that can form a chemical bond by sharing a pair of its electrons with another species
Lewis base
28
An atom or a group attached to a central atom in a molecule; any group attached to anything else of interest
Ligand
29
Process in which a stoichiometric equivalent of acid is added of a base (or vice versa)
Neutralization
30
Defined as pH = - log[H+]
pH
31
Compound that can donate or accept more than one proton
Polyprotic acid or base
32
One with an acidic hydrogen atom
Protic solvent
33
Expression having the same form as the equilibrium constant for a reaction. However, the reaction quotient is evaluated for a particular set of existing activities (concentrations), which are generally not the equilibrium values. At equilibrium, Q = K.
Reaction quotient (Q)
34
An ionic solid
Salt
35
One that contains the maximum amount of a compound that can dissolve at equilibrium
Saturated solution
36
Equilibrium constant for the dissociation of a solid salt to give its ions in solution
Solubility product (Ksp)
37
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
Standard state
38
Equilibrium constant for a reaction of the type ML(n-1) + L ⇌ MLn
Stepwise formation constant (Kn)