PRAKTIKUM PERGESERAN KESETIMBANGAN

Summary

This chemistry experiment demonstrates how shifts in equilibrium occur when different substances, such as FeCl₃, KSCN, Na₂HPO₄, and water, are added to a reaction system. The primary goal is to observe color changes in the solutions, which indicate shifts to the right or left in the equilibrium. As various substances increase or decrease ion concentrations (Fe³⁺, SCN⁻, HPO₄²⁻), the color intensity changes, with the solutions becoming either darker or lighter. The results are explained through Le Chatelier's Principle, providing insight into how concentration changes influence chemical equilibrium and the visible outcomes of these shifts.

Takeaways

• 😀 The experiment is about studying the shift in chemical equilibrium and its response to changes in concentration.
• 😀 FeCl3 and KSCN solutions are used in the experiment to observe their effect on the color changes and equilibrium shift.
• 😀 25 mL of distilled water is prepared, and 1 drop each of FeCl3 and KSCN is added and mixed.
• 😀 The solution is divided into five test tubes, each receiving different treatments to observe the effects of various additives.
• 😀 Test tube 1 serves as the control, with no additional solutions added, to compare the effects of other treatments.
• 😀 In test tube 2, 1 drop of KSCN is added to observe a color change and compare it with the control solution.
• 😀 In test tube 3, 1 drop of FeCl3 is added to observe a color change and compare it with the control solution.
• 😀 In test tube 4, 1 drop of Na2HPO4 is added, which contains HPO4 ions that bind with Fe3+ ions, shifting the equilibrium.
• 😀 In test tube 5, 5 mL of distilled water is added to observe the impact of volume change on the equilibrium.
• 😀 The main reactions involve Fe3+ and SCN- ions interacting, with the color change indicating shifts in the chemical equilibrium.
• 😀 Adding KSCN or FeCl3 shifts the equilibrium to the right, making the color darker, while adding Na2HPO4 or distilled water shifts it to the left, making the color lighter.
• 😀 The experiment demonstrates the principle of Le Chatelier's Principle, where concentration changes affect the position of equilibrium.

Q & A

What is the purpose of the chemistry experiment described in the script?

The purpose of the experiment is to observe the shift in chemical equilibrium by altering the concentration of reactants and observing the resulting changes in the system, including the color changes of the solutions.

What chemicals are used in the experiment?

The chemicals used in the experiment include FeCl3 (iron chloride), KSCN (potassium thiocyanate), Na2HPO4 (disodium hydrogen phosphate), and aquades (distilled water).

How is the experiment set up?

The experiment is set up by preparing a solution of FeCl3 and KSCN in aquades, which is then distributed into five test tubes, each treated with different substances to observe how they influence the chemical equilibrium.

Why is one test tube left untreated?

The first test tube is left untreated to serve as a control for comparison with the other test tubes that have been altered with additional chemicals.

What is added to the second test tube and what is the expected outcome?

In the second test tube, one drop of KSCN is added. The addition of KSCN increases the concentration of SCN- ions, causing the equilibrium to shift to the right, resulting in a darker color.

What happens when FeCl3 is added to the third test tube?

When FeCl3 is added to the third test tube, it increases the concentration of Fe3+ ions, causing the equilibrium to shift to the right. This results in the solution becoming darker in color.

What is the function of Na2HPO4 in the fourth test tube?

Na2HPO4 is added to the fourth test tube to bind Fe3+ ions with HPO4 2- ions, shifting the equilibrium to the left and causing the solution to become lighter or more faded in color.

What is the role of adding aquades (distilled water) to the fifth test tube?

Adding aquades (distilled water) to the fifth test tube dilutes the solution, increasing the volume and thus shifting the equilibrium to the left. This results in the solution becoming lighter in color.

How does the addition of KSCN affect the equilibrium?

The addition of KSCN increases the concentration of SCN- ions in the system, which causes the equilibrium to shift to the right, producing a darker color in the solution.

What chemical reaction occurs in this experiment?

The chemical reaction in this experiment involves Fe3+ ions from FeCl3 reacting with SCN- ions from KSCN to form a reddish-brown complex, FeSCN2+, which is responsible for the color change observed in the experiment.