Related Topics:

More Lessons for High School Chemistry

Math Worksheets

A series of free High School Chemistry Video Lessons.**Equilibrium Changes**

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 CoCl_{2} equilibrium. 4 stresses applied: HCl, AgNO_{3}, 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**

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.

You can use the free Mathway calculator and problem solver below to practice Algebra or other math topics. Try the given examples, or type in your own problem and check your answer with the step-by-step explanations.

More Lessons for High School Chemistry

Math Worksheets

A series of free High School Chemistry Video Lessons.

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

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.

Rotate to landscape screen format on a mobile phone or small tablet to use the **Mathway** widget, a free math problem solver that **answers your questions with step-by-step explanations**.

You can use the free Mathway calculator and problem solver below to practice Algebra or other math topics. Try the given examples, or type in your own problem and check your answer with the step-by-step explanations.

We welcome your feedback, comments and questions about this site or page. Please submit your feedback or enquiries via our Feedback page.

[?] Subscribe To This Site