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Chem 202 Final Exam Study Guide With Complete Solutions Latest Update
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Chem 202 Final Exam Study Guide With Complete Solutions Latest Update
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Solution 2024/2025Pepper
Chem 202 Final Exam Study Guide With
Complete Solutions Latest Update
Solubility (g/L) ANS✔✔ The maximum amount of solute that will dissolve in a
given quantity of solvent at a specific temperature
Molar Solubility (mol/L) (s) ANS✔✔ The number of moles dissolved in 1 L of a
saturated solution (in mol/L)
Solubility Product (Ksp) ANS✔✔ Equilibrium constant representing the
"product of solubility"
Precipitation Reactions ANS✔✔ 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 ANS✔✔ A solution already containing a solute with an ion in
common with the reversible reaction
Common Ion Effect ANS✔✔ A common ion decreases the solubility of a
"mostly insoluble" compound
, Solution 2024/2025
Pepper
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 ANS✔✔ Charged species consisting of metal ion surrounded by
ligands
Common Ion Effect (Acids and Bases) ANS✔✔ 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 ANS✔✔ 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 ANS✔✔ 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 ANS✔✔ 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] )
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