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30 Cards in this Set

  • Front
  • Back
What will anions of strong acids do to the pH?
No change
What will cations of strong bases do to the pH?
No change
What will anions of weak acids do to the pH?
Higher the pH
What will cations of weak acids do to the pH?
Lower the pH
What will polyatomic cations with >1+ protons do to the pH? (NH_4^+ and H_3O^+)
Lower the pH
What will metal ions do to the pH?
Lower the pH

Hydration-positive charge interact with the oxygen electrons
Increasing metal charge=more acidic
What are binary acids?
Binary acids are compounds containing H and one other element
What are the acidity trends of binary acids?
1. Bond strength increases with decreasing size=less acidic
2. Larger differences of electronegativity=more acidic
3. Acidity increases down a particular group
What is the Oxy-acids rule #1?
For two acids with equal number of OH and O: the acid with the most electronegative central atom is more acidic
What is the Oxy-acids rule #2?
The OH bond becomes more polar as electron density is pulled away. Larger size conjugate bases can "spread out" the extra charge more easily
What is the common-ion effect?
Weak electrolyte ionization is decreased by adding a strong electrolyte that has an ion in common with the weak electrolyte
What is the characteristic of buffered solutions?
Because buffer solutions contain both acidic and basic species they are resistive to pH changes
-assuming the amounts of HX and X- in the buffer are large in comparison to the amount of OH- and H+ added.
-And the weak acid/base was not used up
What do you use to find the initial pH of a titration?
Normal ICE table
What do you use to find the pH before the equivalence point?
BCA table, the used henderson-hasselbalch equation
What do you use to find the pH at the equivalence point?
BCA table, the ICE table with the conjugate reacting with water
What do you use to find the pH after the equivalence point?
BCA table, the find the pH based on just the strong acid or base
Solubility?
how much solid will dissolve before a solution becomes saturated....g/L
Molar solubility?
how many moles dissolve to make the saturated solution....mol/L
Solubility-The Common-ion effect?
In general, the solubility of a slightly soluble salt is decreased by the presence of a second solute that furnishes a common ion
Complex ions?
Metal complexes are formed as Lewis bases share non-bonding electrons with vacant orbitals on the metal
Amphoteric substances?
Amphoteric substances are soluble in strong acid or strong base, but insoluble at neutral pH

Examples: Al^3+, Cr^3+, Zn^2+, Sn^2+
K_sp < Q
Then precipitation until Q=K_sp
K_sp=Q
Saturated solution
K_sp>Q
Then all of solid dissolves
What are the three factors that affect solubility?
1. The presence of common ions
2. The pH of a solution will affect the solubility of any substance where the anion is basic
3. Formation of complex ions
What is the first law of thermodynamics?
Energy is conserved(not created or destroyed)
What is the second law of thermodynamics?
In any irreversible(spontaneous) process the entropy of the universe increases
What is the third law of thermodynamics?
Entropy of a pure crystalline substance at absolute zero is zero
Entropy increases with???
1. increased temperature of atoms/molecules
2. increased volume for atoms/molecules to move in
3. increased number of independently moving objects
What are the factors that effect spontaneity?
1. Enthalpy
2. Temperature
3. Entropy