Acid-Base Titration Experiment Report

Categories: Chemistry

Report, Pages 3 (632 words)

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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.

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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.

Variables

Control	Independent	Dependent
The indicator, NaOH	H2SO4, HCl, HNO3	The chemical reaction between the acids and alkali.

Materials and Apparatus

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

Method

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

The neutralization reactions are as follows:

NaOH + HCl → NaCl + H2O
NaOH + HNO3 → NaNO3
NaOH + H2SO4 → Na2SO4 + 2H2O

Observations

Alkali	Acid	Moles	Observation
NaOH	HCl	1 Mole	Took 4 ml to neutralize. Get to Know The Price Estimate For Your Paper Topic Deadline: 10 days left Number of pages Email Invalid email By clicking “Check Writers’ Offers”, you agree to our terms of service and privacy policy. We’ll occasionally send you promo and account related email "You must agree to out terms of services and privacy policy" Write my paper You won’t be charged yet! Get quality help now Doctor Jennifer Verified writer Proficient in: Chemistry 5 (893) “ Thank you so much for accepting my assignment the night before it was due. I look forward to working with you moving forward ” +84 relevant experts are online Hire writer No further experiment was made.
NaOH	HCl	0.1 Mole	Took 31 ml to neutralize. Pink salt crystals formed in 2.30 minutes.
NaOH	HNO3	1 Mole	Took 19.2 ml to neutralize. White salt crystals formed in 2 minutes.
NaOH	H2SO4	2 Moles	Took 1.1 ml to neutralize. Rings of white salt formed in 2.15 minutes.

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.