Chem 202 Final Exam Study Guide with
Questions and Answers
Solubility (g/L) ANSWER The maximum amount of solute that will dissolve in a given
quantity of solvent at a specific temperature
Molar Solubility (mol/L) (s) ANSWER The number of moles dissolved in 1 L of a saturated
solution (in mol/L)
Solubility Product (Ksp) ANSWER Equilibrium constant representing the "product of
solubility"
Precipitation Reactions ANSWER Use Q vs. Ksp to predict whether a precipitate will form:
Q<K products too small- no precipitate forms because not enough ions
Q>K products too big (too much in solution) - precipitate forms because too many ions
Common Ion ANSWER A solution already containing a solute with an ion in common with
the reversible reaction
Common Ion Effect ANSWER A common ion decreases the solubility of a "mostly
insoluble" compound
If a solution initially contains a solute of an ion in common with a given reversible reaction,
that ions is known as a common ion
, If a product is already present in the environment, there will be a shift in equilibrium balance
back towards reactant
Complex Ion ANSWER Charged species consisting of metal ion surrounded by ligands
Common Ion Effect (Acids and Bases) ANSWER If an acid or base is already present in
solution, it will effect the overall pH of the entire solution if an acid or base (in common) is
added
Buffer ANSWER A solution that contains a weak acid or base and its conjugate, which is
resistant to pH change due to the common ion effect.
A solution is considered a buffer if: 10 ≥ [A-]/[HA] ≥ 0.1
Buffer Capacity ANSWER The greater the concentrations of the weak acid and conjugate
base (or weak base and conjugate acid), the more resistant the solution will be to pH changes.
Henderson-Hasselbalch Equation ANSWER Used to calculate the pH of a buffer solution in
which the equilibrium concentrations of acid and conjugate base are known:
pH = pKa + log( [A-]/[HA] )
Titration ANSWER A form of chemical analysis used to determine unknown concentrations
of acids or bases.
A neutralization reaction is performed until the equivalence point of the reaction is reached
Questions and Answers
Solubility (g/L) ANSWER The maximum amount of solute that will dissolve in a given
quantity of solvent at a specific temperature
Molar Solubility (mol/L) (s) ANSWER The number of moles dissolved in 1 L of a saturated
solution (in mol/L)
Solubility Product (Ksp) ANSWER Equilibrium constant representing the "product of
solubility"
Precipitation Reactions ANSWER Use Q vs. Ksp to predict whether a precipitate will form:
Q<K products too small- no precipitate forms because not enough ions
Q>K products too big (too much in solution) - precipitate forms because too many ions
Common Ion ANSWER A solution already containing a solute with an ion in common with
the reversible reaction
Common Ion Effect ANSWER A common ion decreases the solubility of a "mostly
insoluble" compound
If a solution initially contains a solute of an ion in common with a given reversible reaction,
that ions is known as a common ion
, If a product is already present in the environment, there will be a shift in equilibrium balance
back towards reactant
Complex Ion ANSWER Charged species consisting of metal ion surrounded by ligands
Common Ion Effect (Acids and Bases) ANSWER If an acid or base is already present in
solution, it will effect the overall pH of the entire solution if an acid or base (in common) is
added
Buffer ANSWER A solution that contains a weak acid or base and its conjugate, which is
resistant to pH change due to the common ion effect.
A solution is considered a buffer if: 10 ≥ [A-]/[HA] ≥ 0.1
Buffer Capacity ANSWER The greater the concentrations of the weak acid and conjugate
base (or weak base and conjugate acid), the more resistant the solution will be to pH changes.
Henderson-Hasselbalch Equation ANSWER Used to calculate the pH of a buffer solution in
which the equilibrium concentrations of acid and conjugate base are known:
pH = pKa + log( [A-]/[HA] )
Titration ANSWER A form of chemical analysis used to determine unknown concentrations
of acids or bases.
A neutralization reaction is performed until the equivalence point of the reaction is reached
