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Quantitative Analysis > Chapter 6 > Flashcards

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

A

Entropy

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

A

Ion pair

25
Q

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

A

Le Châtelier’s principle

26
Q

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

A

Lewis acid

27
Q

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

A

Lewis base

28
Q

An atom or a group attached to a central atom in a molecule; any group attached to anything else of interest

A

Ligand

29
Q

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

A

Neutralization

30
Q

Defined as pH = - log[H+]

A

pH

31
Q

Compound that can donate or accept more than one proton

A

Polyprotic acid or base

32
Q

One with an acidic hydrogen atom

A

Protic solvent

33
Q

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.

A

Reaction quotient (Q)

34
Q

An ionic solid

A

Salt

35
Q

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

A

Saturated solution

36
Q

Equilibrium constant for the dissociation of a solid salt to give its ions in solution

A

Solubility product (Ksp)

37
Q

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

A

Standard state

38
Q

Equilibrium constant for a reaction of the type ML(n-1) + L ⇌ MLn

A

Stepwise formation constant (Kn)

Quantitative Analysis (12 decks)

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