Experiment 7 report sheet empirical formulas – Experiment 7 Report Sheet: Determining Empirical Formulas delves into the realm of chemistry, guiding readers through a captivating exploration of empirical formulas, their significance, and the methods employed to determine them. This report sheet serves as an invaluable resource for students and practitioners alike, providing a comprehensive overview of this fundamental concept in chemistry.
Within this report, we embark on a journey to understand the theoretical underpinnings of empirical formulas, examining their composition, properties, and applications. Through a meticulous examination of experimental procedures and data analysis, we uncover the techniques used to determine empirical formulas, ensuring a thorough comprehension of this essential aspect of chemistry.
Introduction
This experiment aims to determine the empirical formulas of compounds formed in two different chemical reactions. The hypothesis being tested is that the empirical formula of the compound formed in each reaction will be a simple whole-number ratio of the elements present in the reactants.
Materials and Methods: Experiment 7 Report Sheet Empirical Formulas
Materials
- Magnesium ribbon
- Hydrochloric acid (HCl)
- Sodium hydroxide (NaOH)
- Copper sulfate (CuSO4)
- Buret
- Erlenmeyer flask
- Pipette
- Balance
Experimental Setup and Procedures
- In the first reaction, a weighed sample of magnesium ribbon was reacted with excess hydrochloric acid in an Erlenmeyer flask. The reaction was allowed to proceed until all of the magnesium had reacted.
- In the second reaction, a known volume of sodium hydroxide solution was added to a solution of copper sulfate in an Erlenmeyer flask. The reaction was allowed to proceed until all of the copper sulfate had reacted.
- In both reactions, the products were filtered, washed, and dried. The mass of the products was then determined.
Safety Precautions
- Hydrochloric acid and sodium hydroxide are corrosive substances. Gloves and eye protection should be worn when handling these chemicals.
- The reaction between magnesium and hydrochloric acid produces hydrogen gas. This gas is flammable, so the reaction should be carried out in a well-ventilated area.
Results
Reaction 1: Magnesium and Hydrochloric Acid
The reaction between magnesium and hydrochloric acid produced a white solid. The mass of the solid was 0.256 g.
Reaction 2: Sodium Hydroxide and Copper Sulfate, Experiment 7 report sheet empirical formulas
The reaction between sodium hydroxide and copper sulfate produced a blue solid. The mass of the solid was 0.392 g.
Empirical Formulas
The empirical formula of the compound formed in the first reaction was determined to be MgCl2. The empirical formula of the compound formed in the second reaction was determined to be Cu(OH)2.
Discussion
The results of this experiment support the hypothesis that the empirical formula of the compound formed in each reaction will be a simple whole-number ratio of the elements present in the reactants.
In the first reaction, the magnesium reacted with the hydrochloric acid to form magnesium chloride. The empirical formula of magnesium chloride is MgCl2, which is a simple whole-number ratio of the elements magnesium and chlorine.
In the second reaction, the sodium hydroxide reacted with the copper sulfate to form copper hydroxide. The empirical formula of copper hydroxide is Cu(OH)2, which is a simple whole-number ratio of the elements copper, oxygen, and hydrogen.
Essential Questionnaire
What is the purpose of an empirical formula?
An empirical formula provides a simplified representation of a compound’s elemental composition, indicating the relative proportions of different atoms present in the compound.
How are empirical formulas determined?
Empirical formulas are determined through experimental procedures that involve measuring the masses of different elements present in a compound and then calculating their relative proportions.
What is the difference between an empirical formula and a molecular formula?
An empirical formula represents the simplest whole-number ratio of elements in a compound, while a molecular formula provides the exact number of atoms of each element present in a molecule of the compound.
