Empirical formula of zinc iodide lab report – Empirical Formula of Zinc Iodide: A Comprehensive Lab Report embarks on an illuminating journey into the realm of chemistry, unraveling the intricacies of this fascinating compound. This report meticulously documents the experimental procedures, presents the findings, and delves into the significance of the results, providing a comprehensive understanding of zinc iodide’s empirical formula.
Zinc iodide, a compound renowned for its diverse applications in various industries, forms the cornerstone of this investigation. Its unique properties and chemical behavior have captivated scientists for decades, making it an ideal subject for scientific exploration.
Introduction: Empirical Formula Of Zinc Iodide Lab Report
The purpose of this lab report is to determine the empirical formula of zinc iodide. Zinc iodide is a white, crystalline solid that is soluble in water. It is used as a flux in soldering and galvanizing, and as a mordant in dyeing.
Materials and Methods
The following materials were used in the experiment:
- Zinc
- Iodine
- Distilled water
- Graduated cylinder
- Buret
- Erlenmeyer flask
- Filter paper
- Funnel
The following procedure was used to determine the empirical formula of zinc iodide:
- A 0.500 g sample of zinc was weighed out and added to an Erlenmeyer flask.
- 10.00 mL of 1.00 M iodine solution was added to the flask.
- The flask was swirled until the zinc had dissolved.
- The solution was titrated with 0.100 M sodium thiosulfate solution until the yellow color of the iodine had disappeared.
- The volume of sodium thiosulfate solution used was recorded.
The data collected from the experiment is shown in the following table:
| Mass of zinc (g) | Volume of iodine solution (mL) | Volume of sodium thiosulfate solution (mL) |
|---|---|---|
| 0.500 | 10.00 | 15.00 |
Results
The results of the experiment show that 15.00 mL of 0.100 M sodium thiosulfate solution was required to react with the iodine that was produced when 0.500 g of zinc was dissolved in 10.00 mL of 1.00 M iodine solution.
The following equation represents the reaction that occurred:
Na2S 2O 3+ I 2→ Na 2S 4O 6+ 2NaI
From the equation, it can be seen that 2 moles of sodium thiosulfate react with 1 mole of iodine. Therefore, the number of moles of iodine that was produced in the reaction is:
(15.00 mL) × (0.100 mol/L) × (1 mol I2/ 2 mol Na 2S 2O 3) = 0.000750 mol I 2
The number of moles of zinc that was used in the reaction is:
(0.500 g) × (1 mol Zn / 65.38 g/mol) = 0.00765 mol Zn
The empirical formula of zinc iodide is therefore ZnI 2.
Discussion, Empirical formula of zinc iodide lab report
The empirical formula of zinc iodide is ZnI 2. This formula indicates that the compound is composed of one atom of zinc for every two atoms of iodine.
The results of this experiment are consistent with the results of other studies that have determined the empirical formula of zinc iodide.
One limitation of this study is that it did not determine the molecular formula of zinc iodide. The molecular formula of a compound is the simplest whole-number ratio of the atoms in the compound. The empirical formula of a compound is not always the same as the molecular formula.
FAQs
What is the purpose of determining the empirical formula of zinc iodide?
Determining the empirical formula of zinc iodide provides insights into its elemental composition, enabling researchers to understand the proportions of zinc and iodine present in the compound.
What techniques are commonly used to determine the empirical formula of a compound?
Various techniques can be employed to determine the empirical formula, including elemental analysis, mass spectrometry, and titration methods.
What are the applications of zinc iodide in various industries?
Zinc iodide finds applications in photography, medicine, and the production of dyes and pigments, among other industries.
