Topics 7.11 - 7.12

Dynamic Equilibrium

A state where the rate of dissolution of a solute is equal to the rate of precipitation.

Solubility Rules

Guidelines used to predict the solubility of ionic compounds in water.

Precipitation Reaction

A reaction in which ions in solution form an insoluble ionic compound.

Common Ion Effect

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

Molar Solubility

The concentration of a saturated solution expressed in moles per liter.

Aqueous Solution

A solution in which the solvent is water.

Saturated Solution

A solution that contains the maximum amount of solute that can dissolve at a given temperature.

Dissolution

The process of dissolving a solute in a solvent to form a solution.

Spectator Ions

Ions that do not participate in the chemical reaction and remain unchanged during the reaction.

Concentration

The amount of a substance per defined space, typically expressed in moles per liter.

Equilibrium Constant (K)

The numerical value obtained from the equilibrium expression at a given temperature.

Dilution

The process of reducing the concentration of a solute in solution, usually by adding more solvent.

Charge Balance

The principle that the total positive charge must equal the total negative charge in a compound.

Undissolved Solid

The solid state of a solute that remains in the beaker, indicating a saturated solution.

Net Ionic Equation

An equation that shows only the particles that participate in the reaction, excluding spectator ions.

Le Chatelier's Principle

The principle stating that if a system at equilibrium is disturbed, the system will shift in a direction to reduce the disturbance.

What does Ksp represent?

Ksp represents the solubility equilibrium constant for ionic compounds, indicating the maximum concentration of ions in a saturated solution.

How do solubility rules assist in predicting solubility?

Solubility rules categorize salts to determine which are soluble, such as those containing alkali metals or ammonium ions.

What are Precipitate Formation criteria?

Precipitate formation can be determined by comparing Qsp to Ksp; if Qsp > Ksp, a precipitate forms.

How does the Common Ion Effect relate to Le Chatelier's Principle?

The Common Ion Effect demonstrates Le Chatelier's Principle by showing that adding a common ion reduces the solubility of a salt.

What happens during Evaporation of a Saturated Solution?

During evaporation, the concentration of dissolved ions largely remains unchanged, affecting solubility predictions.

What indicates a high solubility in Ksp values?

Generally, a Ksp greater than 1 indicates high solubility of an ionic compound.

How can Qsp be used to predict precipitation reactions?

By evaluating if Qsp is less than or greater than Ksp, one can predict whether a precipitate will form.