Praktikum Titrasi Asam Kuat Basa Kuat | HCl dengan NaOH

Syifa Sa'diyyah

26 Dec 202107:04

Summary

TLDRThis video demonstrates the practical process of performing a titration between a strong acid (HCl) and a strong base (NaOH). It begins with an introduction of the equipment and materials, such as a burette, pipette, Erlenmeyer flask, and phenolphthalein indicator. The video details key steps, including rinsing apparatus, assembling the setup, and preparing solutions. The titration process is explained, highlighting careful volume measurements, color change observation at the titration's endpoint (a pale pink hue), and recording data. This step-by-step guide aids in understanding the practical execution of acid-base titration.

Takeaways

🧪 The experiment is about titration of a strong acid (HCl) with a strong base (NaOH).
🔧 The equipment used includes a clamp, stand, burette (50 ml), pipet (10 ml), funnel, Erlenmeyer flask (100 ml), and beakers (100 ml).
💧 The chemicals involved are distilled water (aquades), phenolphthalein indicator, 0.1 M hydrochloric acid (HCl), and 0.1 M sodium hydroxide (NaOH).
🧴 Before use, volumetric equipment (such as the burette and pipet) must be rinsed with the respective solutions.
⚖️ The burette is filled with 50 ml of 0.1 M NaOH, ensuring the meniscus is at the proper scale for accurate measurement.
📏 The pipet is rinsed with 0.1 M HCl before transferring 10 ml of HCl solution into the Erlenmeyer flask for the titration.
🎨 Two drops of phenolphthalein are added to the HCl in the flask to act as the indicator for the titration.
🔍 The titration process involves slowly adding NaOH from the burette to the HCl solution in the Erlenmeyer flask while stirring.
🌸 The endpoint of the titration is reached when the solution turns a faint pink color, indicating neutralization.
📝 Data collection involves recording the volume of NaOH used to reach the endpoint, repeating the experiment for accuracy.

Q & A

What is the objective of the experiment presented in the script?
-The objective of the experiment is to perform a titration between a strong acid (hydrochloric acid) and a strong base (sodium hydroxide).
What are the main materials and tools needed for the titration process?
-The materials and tools required include a clamp, a stand, a 50 mL buret, a 10 mL pipette, a short glass funnel, three 100 mL Erlenmeyer flasks, two 100 mL beakers, distilled water, phenolphthalein indicator, 0.1 M hydrochloric acid solution, 0.1 M sodium hydroxide solution, and white paper as a base.
Why is it important to rinse the buret before the titration begins?
-Rinsing the buret ensures that it is clean and that no residual substances will affect the accuracy of the titration results. In this experiment, the buret is rinsed with 0.1 M sodium hydroxide solution.
How should the buret be filled with sodium hydroxide solution?
-The buret should be filled with 0.1 M sodium hydroxide solution using a glass funnel. Ensure the buret tap is closed to prevent leakage, and fill the buret to 50 mL, adjusting the volume to the meniscus level for accuracy.
What is the purpose of the phenolphthalein indicator in this titration?
-Phenolphthalein is used as an indicator to detect the endpoint of the titration. It changes color to pink when the solution turns from acidic to slightly basic, indicating the completion of the titration.
Why is it necessary to place white paper under the Erlenmeyer flask during titration?
-White paper is placed under the Erlenmeyer flask to make it easier to observe the color change, which signals the endpoint of the titration.
How is the titration performed once the materials are set up?
-The titration is performed by gradually adding 0.1 M sodium hydroxide from the buret into the hydrochloric acid in the Erlenmeyer flask, while gently swirling the flask, until the solution turns pale pink.
What does the endpoint of the titration indicate?
-The endpoint is indicated by a slight pink color that persists in the solution, showing that the hydrochloric acid has been neutralized by the sodium hydroxide.
How is the volume of sodium hydroxide used in the titration measured?
-The volume of sodium hydroxide is measured by reading the scale on the buret before and after titration, and the difference gives the volume of sodium hydroxide used.
What is the next step after completing the titration process?
-After completing the titration, the volume of sodium hydroxide used is recorded for analysis, and the process is typically repeated for accuracy.

Outlines

00:00

🧪 Introduction to Acid-Base Titration Practical

In this section, the team introduces themselves as 'Group 2' and explains that they will be conducting a practical titration of a strong acid with a strong base. The equipment and materials required for the titration include a 50 mL burette, 10 mL pipette, Erlenmeyer flasks, beakers, distilled water, phenolphthalein indicator, 0.1 M hydrochloric acid, and 0.1 M sodium hydroxide solution. The script outlines the preparation steps, such as rinsing the burette with sodium hydroxide solution and ensuring the burette tap is closed. The correct procedure for handling and filling the burette with sodium hydroxide solution using a funnel is detailed, emphasizing proper techniques to achieve accurate measurements.

05:00

🧫 Preparing for Accurate Titration and Adding Acid

This section continues with the preparation steps. It explains the rinsing of the 10 mL pipette with 0.1 M hydrochloric acid and the process of using the pipette to transfer the acid into a 100 mL Erlenmeyer flask. The importance of ensuring the solution wets the pipette walls evenly is emphasized. Additionally, the description covers filling the pipette with the acid to the correct measurement, transferring it to the flask, and how careful attention to detail during these steps ensures precision in determining the concentration of the hydrochloric acid.

🔬 Adding the Indicator and Setting Up for Titration

After the hydrochloric acid is transferred to the Erlenmeyer flask, the next step is to add two drops of phenolphthalein indicator. This step is crucial as the indicator will signal the endpoint of the titration by changing color. The Erlenmeyer flask, now containing the acid and indicator, is placed under the burette filled with sodium hydroxide. A white paper is placed beneath the flask to help visualize the color change clearly. The titration setup is now complete, and the team is ready to begin the titration process.

🎯 Performing the Titration and Recording Results

This final section explains the actual titration process. It describes how the sodium hydroxide is gradually added from the burette to the hydrochloric acid in the Erlenmeyer flask while gently swirling the flask to ensure the solutions mix evenly. The titration is continued until a pale pink color persists in the solution, indicating the endpoint. The volume of sodium hydroxide used is recorded by reading the scale on the burette. This is a critical step in calculating the concentration of the hydrochloric acid. The section concludes with the team stating that the experiment is performed in triplicate to ensure accuracy and reliability of the results.

Mindmap

Keywords

💡Titration

Titration is a laboratory method used to determine the concentration of a solution by reacting it with a solution of known concentration. In the video, the students are performing a titration of a strong acid (hydrochloric acid) with a strong base (sodium hydroxide). The process involves slowly adding the base to the acid until a chemical reaction reaches its endpoint, indicated by a color change due to an indicator.

💡Strong Acid and Strong Base

A strong acid, such as hydrochloric acid (HCl), and a strong base, like sodium hydroxide (NaOH), completely dissociate into ions in water. This makes them highly reactive and ideal for titration experiments. In the video, these substances are used to showcase a titration reaction, where the acid's concentration is calculated by neutralizing it with the base.

💡Burette

A burette is a precise glass tube used in titration to dispense small, measured volumes of a liquid, typically the titrant. In the video, the burette is filled with 0.1 M sodium hydroxide solution and used to add the base to the acid solution in the Erlenmeyer flask. The students ensure accurate measurements by checking the meniscus and making sure the burette is properly rinsed before use.

💡Phenolphthalein

Phenolphthalein is a pH indicator commonly used in titrations involving strong acids and bases. It changes color from clear to pink as the solution shifts from acidic to basic. In the video, two drops of phenolphthalein are added to the hydrochloric acid solution in the Erlenmeyer flask. The pink color indicates the endpoint of the titration, showing that the acid has been neutralized by the base.

💡Endpoint

The endpoint in a titration is the point at which the reaction is complete, often indicated by a color change due to an indicator. In the video, the endpoint is reached when the addition of sodium hydroxide causes the solution in the Erlenmeyer flask to turn a pale pink, signifying that the hydrochloric acid has been neutralized.

💡Meniscus

The meniscus is the curve seen at the liquid's surface in a tube, due to surface tension. Accurate measurements in titration are taken at the bottom of the meniscus. The video emphasizes the importance of reading the burette at eye level and ensuring the meniscus is aligned with the calibration mark for precise volume measurements.

💡Pipette

A pipette is a laboratory tool used to transfer a measured volume of liquid. In the video, a 10 ml pipette is used to measure and transfer hydrochloric acid into the Erlenmeyer flask. The correct use of the pipette, including rinsing it with the solution to be measured, ensures accurate delivery of the desired volume for titration.

💡Neutralization

Neutralization is the chemical reaction between an acid and a base to produce water and a salt. In the video, neutralization occurs when the sodium hydroxide (base) is added to hydrochloric acid (acid) until the solution reaches the endpoint. This process is fundamental to titration experiments as it allows for the determination of the acid's concentration.

💡Erlenmeyer Flask

An Erlenmeyer flask is a type of laboratory flask with a conical base and a narrow neck, used to mix and contain reaction solutions. In the video, three Erlenmeyer flasks are used to hold the acid solution and phenolphthalein indicator during titration. Their shape makes them ideal for swirling the solution without spilling, which is necessary to mix the acid and base effectively.

💡Calibration

Calibration refers to the process of verifying and adjusting the precision of measuring instruments. In the video, the calibration of the burette is crucial for accurate titration results. Ensuring the burette is properly rinsed and the meniscus is at the correct level before starting the experiment ensures the measurements are reliable and accurate.

Highlights

Introduction of the titration experiment: strong acid with strong base.

Preparation of tools and materials for titration: including buret, pipet, Erlenmeyer flask, and more.

Explanation of washing the volumetric tools with the solutions to be used, specifically washing the buret with 0.1 M NaOH solution.

Proper method of washing buret: pouring the NaOH solution and ensuring all surfaces are rinsed.

Setting up the equipment: ensuring the buret is clamped correctly and aligned with scale in front.

Filling the buret with 0.1 M NaOH solution to 50 ml and ensuring no solution leaks by keeping the tap closed.

Filling the buret over the scale line and then adjusting the level to get an accurate quantitative volume.

Washing the 10 ml pipet with 0.1 M HCl solution to ensure accurate pipetting.

Pipetting 10 ml of 0.1 M HCl solution into the Erlenmeyer flask for the titration.

Adding 2 drops of phenolphthalein indicator into the Erlenmeyer flask containing HCl.

Placing the Erlenmeyer flask below the buret containing NaOH, with a white paper background for clear color observation.

Starting the titration by releasing NaOH solution into the HCl in the Erlenmeyer flask while gently swirling the flask.

Titration end point: identified when the solution turns pale pink.

Recording the volume of NaOH used during the titration by reading the buret scale.

Conducting the experiment in triplicate to ensure accuracy and repeatability of the results.