Calorimetry for Copper Sulfate Concentration Determination

Abstract

Calorimetry is a scientific technique used to determine the concentration of colored compounds in solutions. This experiment aimed to measure the concentration of copper sulfate solutions using the Beer–Lambert law and a colorimeter. Standard solutions were prepared, and the colorimeter was calibrated to ensure accurate readings. Serial dilutions of the copper sulfate solutions were made, and absorbance measurements were taken. The data obtained were used to create a calibration curve, allowing us to determine the concentration of unknown samples.

The experiment was conducted with precision and accuracy by calibrating instruments, following proper procedures, and minimizing errors. The results were analyzed to calculate the concentrations of the unknown samples.

Introduction

Calorimetry is the measurement of light intensity passing through a sample. It is a quantitative analysis technique that assesses how much light is absorbed by a substance, which is inversely proportional to its concentration. The Beer–Lambert law defines the relationship between absorbance and concentration, stating that higher concentration results in greater absorbance.

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Objective

The aim of this experiment is to determine the concentration of copper sulfate solutions using calorimetry and the Beer–Lambert law.

Materials and Methods

The following materials were used in the experiment:

• Top pan balance
• Copper sulfate
• Distilled water
• Spatula
• Glass beaker (x3)
• Funnel
• Bunsen burner
• Volumetric flask
• Gauze
• Test tubes
• Test tube rack
• Measuring cylinder

The experiment was conducted as follows:

1. Weighed out 24.96 grams of copper sulfate using a top pan balance.
2. Transferred the copper sulfate to a glass beaker and dissolved it in no more than 100 cm³ of distilled water.
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3. Transferred the solution to a volumetric flask, filled it up to the 100 cm³ mark, and labeled the flask.
4. Placed the stopper over the volumetric flask and mixed the solution, using heat if needed, to fully dissolve the copper sulfate.
5. Conducted serial dilutions of the solution in test tubes.
6. Measured the absorbance of each solution using a colorimeter and recorded the data.
7. Calculated the mean absorbance for each concentration.

Results

The data obtained from the experiment were used to create a calibration curve, relating the concentration of copper sulfate solutions to their absorbance values. The concentration of the unknown samples was determined using this curve.

Discussion

The experiment was conducted with precision and accuracy. To ensure accuracy, the colorimeter was calibrated, and meticulous techniques were employed to transfer and measure the solutions. A calibration curve was created, and the unknown sample concentrations were determined with confidence.

Conclusion

In conclusion, this experiment successfully determined the concentration of copper sulfate solutions using calorimetry and the Beer–Lambert law. The results were obtained with accuracy and precision, demonstrating the effectiveness of the technique.