Exam 3 Flashcards
Effect on equilibrium when a substance with an ion in common with the dissolved species is added to the solution; causes a decrease in the solubility of an ionic species, or a decrease in the ionization of a weak acid or base
Common Ion Effect
Sign of delta H= -
Sign of delta S= +
Spontaneity?
Spontaneous at all temperature
More solid can dissolve until Q=K
Q
For any species of oxyacids, acidity increases with the ?
number of oxygen bonded to the central atom
Delta S univ>0; entropy will increase over time
Second Law of Thermodynamics
The total energy of the universe is constant
-Energy cannot be created nor destroyed, but can be converted from one form to another
First Law of Thermodynamics
A measure of the disorder in a system
Entropy (S)
Large negative delta G values means…
large K
Spontaneity? delta H and S: +
Spontaneous at only high temperatures
Provides a quantitative basis and molecular perspective to entropy using probability
Systematic Mechanics/Thermodynamics
Delta H: +
Delta S: -
Spontaneity?
Never spontaneous
What are the 4 distinct regions of a titration curve?
Buffer region, Equivalence Point, Beyond Equivalence Point, Weak Base Ionization
Large positive delta G means…
small K
Q ? K
The system is at equilibrium and the solution is saturated
=
Lewis ? are electron deficient
acids
Contains as much solute as it can hold, in equilibrium with excess (undissolved) solute
Saturated Solution
Contains a metal ion surrounded by a number of ligands
Complex Ion
A molecule or ion with a lone pair of electrons
Ligand
What sorts of changes (4) increase the randomness of a system?
Adding heat
Melting
Vaporization
Sublimation
The entropy of a pure crystalline substance at absolute zero (0 K) is 0.
Third Law of Thermodynamics
Weak organic bases that exhibit a color change at the end point of the titration
Indicators
Delta H and Delta S: -
Spontaneity?
Spontaneous only at low temperatures
Of a substance is the entropy of 1 mole of the substance in its standard state at 298 K and 1 atm
Standard Molar Entropy
The way in which a collection of particles attains a particular energy
Microstate
The salt will precipitate out until Q=K
Q>K
Have H directly bonded to a non-metal, X
HX
Binary Acid
? metal oxides and hydroxides are soluble in strong acids or bases because they can act as either acids or bases in reactions
Amphoteric
When the stoichiometric amount of acid equals that of base
Equivalence Point
Gain electrons and cause other substances to be oxidized
Oxidizing Agent
Defined as electron pair donors
Lewis Bases
H is bonded to O, which is in turn bonded to a non-metal, Y; HYO
Oxyacids
Overall trend in increasing acidity of binary acids?
Increasing electronegativity, increasing size
The concentration of a solute in a saturated solution (no more added solute will dissolve)
Solubility
A solution capable of resisting significant pH changes when a strong acid or base is added
Buffers
Lose electrons and cause other substances to be reduced
Reducing Agent
Defined as electron-pair acceptors
Lewis Acids
