Titrations and Solubility Products (Ksp)

Flashcards covering key vocabulary and concepts related to titrations and solubility products (Ksp) as discussed in the lecture notes.

Titration

A technique to determine the concentration of a solute by reacting it with a reagent of known concentration.

Equivalence Point

The point in a titration where the amount of titrant added is exactly enough to completely react with the analyte.

End Point

The point in a titration at which an indicator changes color, signaling the endpoint of the reaction.

Ksp - Solubility Product Constant

An equilibrium constant that represents the solubility of a salt in a saturated solution.

Common-Ion Effect

The decrease in solubility of a salt when a common ion is added to the solution.

Factors Affecting Solubility

Include pH, common ions, and temperature, which can alter the solubility of salts.

Strong Acid/Strong Base Titration

A titration involving strong acids and bases that typically has a pH change at the equivalence point of 7.

Weak Acid/Strong Base Titration

A titration involving a weak acid and a strong base, where the pH at equivalence point is above 7.

Half-Equivalence Point

The point in a titration where half of the acid has been converted to its conjugate base.

Phenolphthalein

An acid-base indicator that turns pink in a basic solution and is colorless in an acidic solution.

Selective Precipitation

A process used to separate different ions in solution by selectively precipitating one ion while keeping others in solution.

Stoichiometric Ratio

The ratio of the amounts of the various reactants involved in a reaction, which determines the proportions in which they react.

pH Titration Curve

A graphical representation of the change in pH as a function of the amount of titrant added in a titration.

Indicator

A substance that changes color at a specific pH level, used to signal the end of a titration.

Solubility

The ability of a substance to dissolve in a solvent, typically expressed in molarity.

Buffer Region

The region in a titration curve where the pH changes slowly due to the presence of a weak acid and its conjugate base.

Molar Solubility

The number of moles of solute that can dissolve in one liter of solution.

pH at Equivalence Point

For strong acid-strong base titration, it is 7; for weak acid-strong base, it is above 7.

Le Châtelier's Principle

If a system at equilibrium is disturbed, the system will shift in a direction to counteract the disturbance.