Your Safer Source for Science

Since 1977

Address P.O. Box 219 Batavia, IL 60510
Phone 800-452-1261
Fax 866-452-1436

Exploring Equilibrium: It Works Both Ways—Student Laboratory Kit

By: The Flinn Staff

Item #: AP1757

Price: $62.65

In Stock.

In the Exploring Equilibrium Laboratory Kit, students explore the nature and consequences of equilibrium in three reversible chemical reactions. Students observe reactions to predict if a reaction is exothermic or endothermic.

See more product details

This item can only be shipped to schools, museums and science centers

Product Details

Our physical sense of equilibrium suggests a condition of equal balance—in the motion of a seesaw, the swing of a pendulum, the stretch of a spring. How does physical equilibrium translate to the properties of chemical equilibrium? In this comprehensive student laboratory kit, students explore the nature and consequences of equilibrium in three reversible chemical reactions—the acid–base equilibrium of bromcresol green indicator, the solubility equilibrium of magnesium hydroxide and the complex-ion equilibrium of iron(III) thiocyanate. For each reaction, students:

• Observe what it means to say that a reversible chemical reaction can go both ways.
• Examine the effects of changing the concentrations of reactants and products on the position of equilibrium.
• Use LeChâtelier’s Principle to explain how balance can be restored when the equilibrium is disturbed.

Students practice critical-thinking skills as they build on their observations and apply their knowledge to predict whether a reaction is exothermic or endothermic, based on the effect of temperature on the position of equilibrium. Applications of chemical equilibrium in biological and environmental science are highlighted through discussion. Includes reproducible student handouts, detailed background information, Teacher Notes with sample data and answers to questions and all necessary chemicals and consumable supplies.

Complete for 30 students working in pairs.


Materials Included in Kit: 
Bromcresol green solution, 0.04%, 35 mL
EDTA solution, 0.1 M, 40 mL
Hydrochloric acid solution, 0.1 M, 75 mL
Iron(III) nitrate solution, 0.1 M, 75 mL
Magnesium chloride solution, 1 M, 60 mL
Potassium thiocyanate solution, 0.1 M, 75 ml
Sodium hydroxide solution, 0.5 M, 75 mL
Sodium phosphate (monobasic) solution, 0.1 M, 40 mL
Universal indicator solution, 35 mL
Pipet, Beral-type, graduated, 150
Tubes, culture, disposable, 13 x 100 mm, 90

Correlation to Next Generation Science Standards (NGSS)

Science & Engineering Practices

Planning and carrying out investigations
Analyzing and interpreting data
Obtaining, evaluation, and communicating information

Disciplinary Core Ideas

HS-PS1.A: Structure and Properties of Matter
HS-PS1.B: Chemical Reactions

Crosscutting Concepts

Cause and effect
Energy and matter

Performance Expectations

HS-PS1-4. Develop a model to illustrate that the release or absorption of energy from a chemical reaction system depends upon the changes in total bond energy.
HS-PS1-5. Apply scientific principles and evidence to provide an explanation about the effects of changing the temperature or concentration of the reacting particles on the rate at which a reaction occurs.
HS-PS1-6. Refine the design of a chemical system by specifying a change in conditions that would produce increased amounts of products at equilibrium.