Equilibrium in Chemistry
More Lessons for High School Chemistry
A series of free High School Chemistry
In this lesson, we will learn
- Equilibrium Changes
- Calculating Equilibrium Concentrations
- Solubility Equilibrium
Equilibrium changes are caused by Le Chatlier's Principle and depend upon the stress applied. Le Chatelier's Principle predicts the direction of change. For changes in volume, it is important to note that volume and pressure are inversely related. The effect of a change in concentration would increase or decrease in molecular collisions and increase or decrease the rate of forward and reverse reactions accordingly. The result from the effect of a change in temperature can either be exothermic, in which energy is released or endothermic, in which energy is consumed.
How Le Chatlier changes affect chemical equilibrium
Quick demonstration of Le Chatelier's principle using CoCl2
equilibrium. 4 stresses applied: HCl, AgNO3
, heat, and cold
Calculating Equilibrium Concentrations
The general steps of calculating equilibrium concentrations are to first write out the expression of equilibrium constant, then impute the known concentration value of each element given, and finally solve for the unknown value. When dealing with equilibrium, it is important to remember that solids and liquids are not affected.
Given initial concentrations or pressures, and the EQ constant, K, calculate equilibrium concentrations (or pressures). solving for x when x is the change in concentrations
Solubility equilibrium is the equilibrium associated with dissolving solids in water to form aqueous solutions. At the point where no more solid can dissolve, the solution is saturated. The solubility product constant is an equilibrium constant used in solubility equilibrium.
Understanding solubility equilibrium.
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