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Titration
A procedure for determining the concentration of a solution by allowing a measured volume to react with another solution of known concentration.
Equivalence Point
The point in a titration at which the number of moles of titrant added equals the number of moles of analyte in the sample.
pKa
The negative logarithm of the acid dissociation constant (Ka), which indicates the strength of an acid.
Buffer Solutions
A solution that resists changes in pH upon the addition of small amounts of acid or base.
Common-Ion Effect
The shift in the position of an equilibrium caused by the addition of an ion that is a part of the equilibrium.
Henderson-Hasselbalch Equation
An equation used to estimate the pH of a buffer solution: pH = pKa + log([A-]/[HA]).
Weak Acid
An acid that partially dissociates in solution.
Strong Acid
An acid that completely dissociates in solution.
Net Ionic Equation
An equation that shows only the species that participate in a reaction, excluding spectator ions.
Buffer Capacity
A measure of the ability of a buffer to resist changes in pH upon the addition of an acid or base.
Acid-Base Reaction
A chemical reaction that occurs between an acid and a base.
Titrand
The solution of unknown concentration being analyzed in a titration.
Titrant
The solution of known concentration that is added in a titration.
Conjugate Base
The species that remains after an acid has donated a proton.
Conjugate Acid
The species formed when a base accepts a proton from an acid.
Saturated Solution
A solution containing the maximum amount of solute that can dissolve at a given temperature.
Solubility-Product Constant (Ksp)
The equilibrium constant for a solid compound dissolving in water.
Le ChĆ¢telierās Principle
A principle stating that if a system at equilibrium is disturbed, the system shifts in a direction that counteracts the disturbance.
pH
A measure of the acidity or basicity of a solution.
pOH
A measure of the hydroxide ion concentration in a solution, calculated as pOH = -log[OH-].
Diprotic Acid
An acid capable of donating two protons (H+) per molecule.
What is titration?
A procedure for determining the concentration of a solution by allowing a measured volume to react with another solution of known concentration.
What is the equivalence point in titration?
The point at which the number of moles of titrant added equals the number of moles of analyte in the sample.
What is pKa?
The negative logarithm of the acid dissociation constant (Ka), which indicates the strength of an acid.
Define buffer solutions.
A solution that resists changes in pH upon the addition of small amounts of acid or base.
What is the common-ion effect?
The shift in the position of an equilibrium caused by the addition of an ion that is a part of the equilibrium.
What does the Henderson-Hasselbalch equation calculate?
It estimates the pH of a buffer solution: pH = pKa + log([A-]/[HA]).
What is a weak acid?
An acid that partially dissociates in solution.
What is a strong acid?
An acid that completely dissociates in solution.
What is a net ionic equation?
An equation that shows only the species that participate in a reaction, excluding spectator ions.
What is buffer capacity?
A measure of the ability of a buffer to resist changes in pH upon the addition of an acid or base.
What happens in an acid-base reaction?
A chemical reaction that occurs between an acid and a base.
What is a titrand?
The solution of unknown concentration being analyzed in a titration.
What is a titrant?
The solution of known concentration that is added in a titration.
What is a conjugate base?
The species that remains after an acid has donated a proton.
What is a conjugate acid?
The species formed when a base accepts a proton from an acid.
What is a saturated solution?
A solution containing the maximum amount of solute that can dissolve at a given temperature.
What is the solubility-product constant (Ksp)?
The equilibrium constant for a solid compound dissolving in water.
What is Le ChĆ¢telierās Principle?
A principle stating that if a system at equilibrium is disturbed, the system shifts in a direction that counteracts the disturbance.
What does pH measure?
A measure of the acidity or basicity of a solution.
What does pOH measure?
A measure of the hydroxide ion concentration in a solution, calculated as pOH = -log[OH-].
What is a diprotic acid?
An acid capable of donating two protons (H+) per molecule.
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