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The electrical conductivity of solutions is a fundamental property that can provide insights into the ability of ions to carry an electric charge in an aqueous environment. In this laboratory experiment, we aim to explore and compare the conductivity of various solutions by measuring their electrical conductivity using a conductivity meter. The hypothesis is that the concentration and type of ions present in a solution will influence its conductivity.
Materials:
Methods:
The solutions will include NaCl, CuSO₄, HCl, and NaOH.
Table 1: Initial Conductivity Readings and Solution Properties
| Solution | Concentration | Initial Temperature (°C) | Initial Conductivity (µS/cm) |
|---|---|---|---|
| Distilled Water | N/A | 25 | 5 |
| NaCl Solution | 0.1 M | 25 | 200 |
| CuSO₄ Solution | 0.01 M | 25 | 150 |
| HCl Solution | 0.5 M | 25 | 250 |
| NaOH Solution | 0.2 M | 25 | 180 |
Calculations:
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Calculate the change in conductivity for each solution at different time intervals. b. Formula: ΔConductivity = (Final Conductivity - Initial Conductivity)
b. Formula: Adjusted Conductivity = Initial Conductivity + (Temperature Change * Temperature Coefficient)
Graphs:
The results demonstrate a clear correlation between the type and concentration of ions in a solution and its electrical conductivity. As expected, electrolyte solutions (NaCl, CuSO₄, HCl, NaOH) exhibit higher conductivity than the distilled water control. The conductivity readings over time reveal dynamic changes in ion mobility within the solutions.
The conductivity of NaCl solution, with a concentration of 0.1 M, increased steadily over time, reaching a plateau. This behavior is consistent with the dissociation of NaCl into ions, contributing to increased conductivity. Similar trends were observed for CuSO₄, HCl, and NaOH solutions, albeit with varying rates of conductivity change.
Temperature changes can influence conductivity readings, necessitating adjustments to ensure accurate comparisons. The temperature-compensated conductivity values provide a more reliable basis for assessing the inherent conductivity of each solution.
In conclusion, this laboratory experiment effectively investigated the electrical conductivity of aqueous solutions. The data collected and analyzed demonstrated the impact of ion concentration and type on the conductivity of solutions. The findings contribute valuable insights into the behavior of electrolytes in solution, with potential applications in fields such as chemistry, environmental science, and industry.
The observed trends in conductivity changes over time provide a foundation for further research and exploration of ion dynamics in aqueous solutions. This experiment highlights the importance of considering environmental factors, such as temperature, in conductivity measurements. Overall, the knowledge gained from this investigation enhances our understanding of solution conductivity and its practical implications.
Investigation of Electrical Conductivity in Aqueous Solutions. (2024, Feb 27). Retrieved from https://studymoose.com/document/investigation-of-electrical-conductivity-in-aqueous-solutions
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