PRAKTIKUM PENENTUAN PERUBAHAN ENTALPI REAKSI PENETRALAN

Summary

In this educational video, viewers learn how to determine the heat change (ΔH) in a neutralization reaction between hydrochloric acid (HCl) and sodium hydroxide (NaOH) using a simple calorimeter. The experiment involves measuring the initial temperatures of both solutions, mixing them, and observing the resulting temperature change. By using basic lab equipment like a thermometer and calorimeter, the video guides viewers through the process of calculating the heat of the reaction. The goal is to understand how calorimetry can be used to measure enthalpy changes in chemical reactions.

Takeaways

• 😀 The experiment aims to determine the enthalpy change (delta H) of the neutralization reaction between HCl and NaOH using a simple calorimeter.
• 😀 A calorimeter is a tool designed to measure heat changes without heat exchange between the system and the environment.
• 😀 The experiment uses a simple calorimeter along with tools such as thermometers, glass beakers, and pipettes.
• 😀 The key materials for the experiment include 1 M HCl and 1 M NaOH solutions.
• 😀 The first step is to measure 50 mL of NaOH solution using a graduated cylinder, ensuring accurate measurement by aligning the meniscus.
• 😀 After measuring NaOH, its initial temperature is recorded with a thermometer. The initial temperature of NaOH is 28°C.
• 😀 Similarly, 50 mL of HCl solution is measured using a pipette, ensuring precise measurement by checking the meniscus.
• 😀 The initial temperature of HCl is also 28°C before the solutions are mixed.
• 😀 The two solutions, NaOH and HCl, are then mixed in the calorimeter, and the temperature change is monitored using a thermometer.
• 😀 After mixing, the temperature increases rapidly and stabilizes at 39°C, indicating an exothermic reaction between NaOH and HCl, allowing for the calculation of the reaction’s heat change using the provided formula.

Q & A

What is the purpose of the experiment described in the transcript?

The purpose of the experiment is to determine the heat of reaction (ΔH) during the neutralization of hydrochloric acid (HCl) and sodium hydroxide (NaOH) using a simple calorimeter.

What materials are used in this experiment?

The materials used include 1 M NaOH solution, 1 M HCl solution, a simple calorimeter, a thermometer, beakers, measuring cylinders, and pipettes.

What is a calorimeter, and why is it used in this experiment?

A calorimeter is an instrument designed to measure the heat of chemical reactions. It is used in this experiment to ensure that no heat is lost to the surroundings, allowing for an accurate measurement of the temperature change during the reaction.

How is the NaOH solution prepared for the experiment?

50 mL of 1 M NaOH solution is measured using a pipette, ensuring accuracy by aligning the meniscus with the marked level on the measuring cylinder, and then poured into a beaker.

What is the initial temperature of the NaOH and HCl solutions?

The initial temperature of both the NaOH and HCl solutions is 28°C.

What happens after the NaOH and HCl solutions are mixed in the calorimeter?

Once the NaOH and HCl solutions are mixed in the calorimeter, the temperature increases rapidly and continues to rise until it reaches 39°C.

Why is it important to prevent heat loss to the environment during the experiment?

Preventing heat loss to the environment is crucial because it ensures that all the heat produced during the reaction is measured accurately, allowing for precise calculations of the heat of the reaction (ΔH).

What can be calculated from the temperature change observed during the experiment?

From the observed temperature change, the heat of the neutralization reaction (ΔH) can be calculated using the appropriate formula.

What is the final temperature reached during the reaction?

The final temperature reached during the reaction is 39°C.

How can you ensure that the volume of solutions measured is accurate during the experiment?

Accurate measurement of solutions is ensured by using a pipette to measure exact volumes, aligning the meniscus with the mark on the measuring cylinder, and being careful when transferring the liquids into the beaker or calorimeter.