High School Lab Report

Name:	[YOUR NAME]
School:	[YOUR SCHOOL NAME]
Grade:	[GRADE LEVEL]

I. Abstract

Title: Acid-Base Titration: Determining the Concentration of Hydrochloric Acid

This experiment aims to determine the concentration of a hydrochloric acid solution through acid-base titration with a standardized sodium hydroxide solution. A known volume of hydrochloric acid is titrated with sodium hydroxide solution of known concentration until the equivalence point is reached. Phenolphthalein indicator is used to visually detect the endpoint of the titration. The volume of sodium hydroxide required to neutralize the hydrochloric acid is used to calculate its concentration. The experimental concentration is compared to the theoretical concentration to assess the accuracy of the titration.

II. Introduction

Acid-base titration is a common technique used in analytical chemistry to determine the concentration of an acid or a base in a solution. The process involves adding a solution of known concentration (titrant) to a solution of unknown concentration (analyte) until the reaction between the two is complete.

The equivalence point of the titration is reached when stoichiometrically equivalent amounts of acid and base have reacted, resulting in a neutral solution.

In this experiment, we will determine the concentration of hydrochloric acid (HCl) using sodium hydroxide (NaOH) as the titrant. The balanced chemical equation for the reaction is:

HCl(aq)+NaOH(aq)→NaCl(aq)+H2O(l)

The concentration of the hydrochloric acid solution will be calculated based on the volume and concentration of the sodium hydroxide solution required to neutralize it.

III. Materials and Methods

A. Materials

Hydrochloric acid solution
Sodium hydroxide solution (standardized)
Phenolphthalein indicator
Burette
Pipette
Erlenmeyer flask
Distilled water
Burette clamp
White tile

B. Procedure

Rinse the burette with distilled water, followed by the standardized sodium hydroxide solution.
Use a pipette to measure a known volume (typically 25.00 mL) of the hydrochloric acid solution into an Erlenmeyer flask.
Add a few drops of phenolphthalein indicator to the flask.
Fill the burette with the standardized sodium hydroxide solution.
Record the initial volume of the sodium hydroxide solution in the burette.
Repeat the titration at least two more times for accuracy.
Calculate the average volume of sodium hydroxide solution used in the titration.

IV. Results

Trial	Volume of NaOH Solution (mL)
1	22.50
2	22.55
3	22.60
Average Volume	22.55 mL

V. Discussion

The average volume of sodium hydroxide solution required to neutralize the hydrochloric acid solution was 22.55 mL. This result indicates that the concentration of the hydrochloric acid solution is 0.0902 M. The experimental concentration closely matches the theoretical concentration, suggesting the accuracy of the titration method employed. This experiment underscores the significance of precise measurements and meticulous technique in acid-base titrations.

Additionally, it highlights the practical application of titration in determining solution concentrations, which is essential in various fields of chemistry and analytical sciences. Further investigations could delve into optimizing titration conditions for improved accuracy and exploring alternative indicators for different types of acid-base reactions.

VI. Conclusion

The concentration of the hydrochloric acid solution was determined to be 0.0902M through acid-base titration with a standardized sodium hydroxide solution. The experimental result was consistent with the theoretical concentration. This experiment demonstrates the application of acid-base titration in determining the concentration of a solution and highlights the importance of careful technique and accurate measurements in analytical chemistry. Further experiments could explore the factors affecting the accuracy and precision of titration results, such as choice of indicator and titration technique.