Titration of Sodium Hydroxide Against Hydrochloric Acid Solution PDF

**Title:** **Tit Today 2:00 AM No category ‫ﺑﺴﻢ ﷲ اﻟﺮﺣﻤﻦ اﻟﺮﺣﻴﻢ‬ University of Bahri Faculty of Public Companions Prepared by : Niema Yagoup Hassan Abdalla Titration of Sodium Hydroxide Against Hydrochloric Acid Solution Introduction: T...

**Title:** **Tit Today 2:00 AM No category ‫ﺑﺴﻢ ﷲ اﻟﺮﺣﻤﻦ اﻟﺮﺣﻴﻢ‬ University of Bahri Faculty of Public Companions Prepared by : Niema Yagoup Hassan Abdalla Titration of Sodium Hydroxide Against Hydrochloric Acid Solution Introduction: Titration is an analytical technique used to determine the concentration of an unknown solution by reacting it with a solution of known concentration. In this experiment, a solution of sodium hydroxide (NaOH) will be titrated against a solution of hydrochloric acid (HCl). The goal of this titration is to determine the concentration of HCl by measuring the amount of NaOH needed to neutralize the acid. Objectives: 1. Understand the principle of titration and apply it to determine the concentration of hydrochloric acid. 2. Identify the equivalence point of the titration using a color indicator. 3. Calculate the concentration of HCl using titration data. Materials and Equipment: - Sodium hydroxide solution (NaOH) of known concentration. - Hydrochloric acid solution (HCl) of unknown concentration. - Burette. - Conical flask. - Volumetric pipette. - Indicator (phenolphthalein or methyl orange). Procedure: 1. Preparation: - Fill the burette with the sodium hydroxide solution. - Use the volumetric pipette to transfer a measured volume of the hydrochloric acid solution into the conical flask. 2. Add Indicator: - Add a few drops of the phenolphthalein indicator to the HCl solution in the conical flask. The solution should remain colorless if it is acidic. 3. Perform the Titration: - Begin adding the NaOH solution from the burette to the HCl solution gradually while continuously swirling the conical flask. - Continue adding NaOH until the solution in the flask reaches the equivalence point, indicated by a noticeable color change (from colorless to light pink using phenolphthalein). 4. Record Data: - Record the volume of NaOH used to reach the equivalence point. Calculations: - Use the formula: \[  C_1V_1 = C_2V_2 \] where: - \( C_1 \) is the concentration of NaOH. - \( V_1 \) is the volume of NaOH used. - \( C_2 \) is the concentration of HCl (to be determined). - \( V_2 \) is the volume of HCl used. Graphical Representation: - To better visualize the results, a graph can be plotted with the volume of NaOH added (x-axis) against the pH of the solution (y-axis). The graph will typically show a gradual increase in pH until the equivalence point, where there is a sharp rise. This sharp rise indicates the point at which the acid has been completely neutralized by the base. If phenolphthalein is used as the indicator, the equivalence point will correspond to a pH of around 8.2, where the solution changes to a light pink color.  Conclusion: - After performing the calculations, the concentration of hydrochloric acid can be determined. This experiment demonstrates the precise application of titration in chemical analysis. Discussion: - Discuss the accuracy of the experiment and the factors that may affect the titration results, such as the precision of the equipment and the correct identification of the endpoint. Summary: - This experiment highlights the importance of titration in chemical analysis. It is a valuable technique for obtaining accurate results in various chemical and industrial applications. Thank you