Acid-Base Titration Experiment Report

Abstract

This experiment aimed to determine how different acids interact with a 25ml solution of sodium hydroxide (NaOH) and their respective neutralization requirements. The hypothesis suggested that the strongest alkali would require the least amount of acid for neutralization, while the weakest would need more. Various acids, including H2SO4, HCl, and HNO3, were used in titration experiments to assess this hypothesis. Observations revealed that stronger acids indeed required less alkali for neutralization.

Introduction

Acids and alkalis are fundamental chemical substances with distinct properties.

Acids are positively charged ions that exist as liquid solutions of pure compounds in water, while alkalis are negatively charged ions, primarily in solid form. Identifying acids can be done using litmus paper, where acids turn litmus paper red, while alkalis turn it blue. The objective of this experiment is to investigate the neutralization process between different acids and sodium hydroxide (NaOH) and determine the amount of acid required to neutralize 25ml of NaOH solution.

Hypothesis

The hypothesis for this experiment posits that the strongest alkali will require the smallest amount of acid for neutralization, while the weakest alkali will necessitate more acid.

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Variables

Materials and Apparatus

• H2SO4
• HCL
• HNO3
• Alkali (NaOH)
• Stand
• Burette
• Beaker
• Funnel
• Bunsen Burner
• Crucible
• Phenolphthalein

Method

1. Pour 25ml of NaOH into a beaker.
2. Add three drops of phenolphthalein to the beaker.
3. The solution turns pink.
4. Using a funnel, pour the acid into the burette.
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5. Add the acid drop by drop into the beaker.
6. The solution gradually becomes lighter in pink color.
7. Stir the beaker to ensure uniform mixing.
8. Stop adding acid when the solution turns clear.
9. Calculate the amount of acid used.
10. Take a portion of the solution and transfer it to a crucible.
11. Ignite the Bunsen burner.
12. The salt solution will crystallize as it is heated.

The neutralization reactions are as follows:

1. NaOH + HCl → NaCl + H2O
2. NaOH + HNO3 → NaNO3
3. NaOH + H2SO4 → Na2SO4 + 2H2O

Observations

Analysis

The observations indicate that the weakest acid (HCl, 0.1 Mole) required the most alkali for neutralization, while the strongest acid (H2SO4, 2 Moles) needed the least. Different experiments resulted in the formation of different salts, such as NaCl, NaNO3, and Na2SO4.

Conclusion

This experiment confirmed that stronger acids required less alkali for neutralization compared to weaker acids. The reactivity of the acids played a crucial role in determining the amount of acid needed to neutralize a given amount of alkali. The results align with the hypothesis that the strongest alkali would demand the smallest amount of acid for neutralization.

Evaluation

In our group, Zuzanna and I conducted the experiment while others observed and recorded data. Initially, we faced challenges with the titration process, leading to repeated attempts. The incorrect amount of H2SO4 was added initially, causing the alkali to turn pink rapidly. After several iterations, we successfully achieved the correct solution. Our salt crystallization process took approximately 2 minutes and 15 seconds, resulting in the formation of rings of white salt crystals. While our salt crystals were not perfect, they were successfully obtained.

Recommendations

For future experiments, it is essential to ensure precise titration by carefully controlling the amount of acid added to the alkali. Additionally, practicing the titration process and recording data accurately will improve the efficiency of the experiment. Further research can explore the specific reactions and properties of different salts formed during the neutralization process.