Equilibrium

dynamic equilibrium

In a chemical system, when the forward reaction and the reverse reaction are balanced and the reactions are occurring at the same rate.

It is changing at a molecular level while its macroscopic properties (an observable or measurable property such as concentration, colour, temperature, pressure, and pH) remain constant.

• System must be closed.

• Three main types that can occur.

reversible reaction

A chemical reaction that proceeds in both the forward and reverse directions.

phase equilibrium

A physical change of state.

* Evaporating, etc.

solubility equilibrium

The dissolving process (solutions).

chemical equilibrium

For any reversible reaction (the forward reaction and the reverse reaction are occurring at the same rate).

The Law of Equilibrium

In a chemical system at equilibrium, there is a __constant ratio__ between the __concentrations of the products__ and the __concentrations of the reactants__.

Equilibrium Constant Expression

**K***eq*

The ratio of equilibrium concentrations for a particular chemical system at a particular temperature.

homogeneous equilibrium

A chemical system in equilibrium in which all of the components are in the same physical state.

heterogeneous equilibrium

A chemical system in equilibrium in which the components are in different physical states (the components do not have to be the same substance).

Le Chatelier’s Principle

When a system at equilibrium is put under stress, the system will shift to relieve the stress and re-establish equilibrium.

inert gas

• Do not react with other gases

• Increasing pressure affects reactants and products equally

• There is no effect on the position of equilibrium

catalyst

• Decreasing the activation energy speeds up both the forward and reverse reaction rates equally

• The system reaches equilibrium faster

• There is no effect on the position of equilibrium

changing concentration

Shift occurs to use up added species __or__ produce more of removed species.

* Keq = no change

changing temperature

Depends on if the reaction is endothermic __or__ exothermic.

* Keq = changes (will increase or decrease)

changing pressure by changing volume

Shift occurs to reduce the number of gas molecules __or__ increase the number of gas molecules.

***NOTE****: only for gas systems!!!*

* Keq = no change

1000 Rule

If the concentration to which “*x*“ is added or subtracted from is **1000x or more greater** than the value of K (when K is small!), then we can **cancel out** ***x*** and assume that \[initial\] = \[equilibrium\].

\
**[initial] >> 1000 x K then [initial] = [equilibrium]**

Solubility-product Constant

For slightly soluble ionic compounds; determined __experimentally__.

* The magnitude of Ksp is a measure of how much solid dissolves to form a saturated solution (unitless).

solubility

The maximum amount of **solute** that can dissolve in a given quantity of **solvent** at a particular temperature.

molar solubility

The amount (in moles) of solute in 1L of a saturated solution (molarity/concentration of the solution).

unsaturated solution

A solution that contains less than the maximum amount of solute that is capable of being dissolved.

• Qsp < Ksp

• More solute dissolves

saturated solution

A solution with solute that dissolves until it is unable to dissolve anymore, leaving the undissolved substances at the bottom.

• Qsp = Ksp

• No more solute dissolves

supersaturated solution

A solution that contains more than the maximum amount of solute that is capable of being dissolved at a given temperature.

soluble ionic compounds

When **soluble** ionic compounds (salts with high solubility) dissolve in water, they dissociate **completely** into ions (i.e. NaCl).

slightly soluble ionic compounds

For **slightly soluble** ionic compounds (salts with low solubility), only a **small amount** dissolves in water (i.e. AgCl). When the solution becomes **saturated**, the __solid__ reaches **equilibrium** with the dissociated ions.

Common Ion Effect

The equilibrium of a system containing ions can be **shifted** by dissolving it into a **common ion** or a **compound that reacts** with one of the ions already in solution. This follows from **Le Chatelier’s Principle**. T__his will affect how we construct our ICE Tables__ (ion molarity is __**NOT ZERO initially**__).

* When the solubility of an ionic compound is lowered as a result of the addition of a common ion; reaction will shift towards the solid.

precipitate

An insoluble product formed in a reaction between two soluble ionic compounds.

For solutions of slightly soluble ionic compounds, we can compare Qsp and Ksp values to determine if this forms.

Solubility Quotient

Used to describe the current state of an aqueous solution and to **predict** whether a **precipitate forms or not**. If it is less than Ksp, then more solid can be dissolved. But if it is larger than Ksp, the solid will precipitate at the bottom of the solution.