Empirical Formula Lab Report

The empirical formula is base on the ratio of moles of silver and the moles of oxygen. The empirical formula needs to show the simplest integer number. For trial one the ratio between moles of silver and moles of oxygen is 5/4, and the ratio between the moles of oxygen and moles of oxygen is 1. According to the law of empirical formula, there can not be a fraction in the formula. So, the empirical formula is Ag5O4.

2. The second source of error in the lab is when opening the lid of the crucible which allowed smoke of magnesium oxide to escape. During the lab, we removed the lid a couple of times to allow oxygen to enter the crucible so the magnesium reacts with the air to form magnesium oxide. However, the smoke could have easily escaped from the crucible because of the strong force of heat from the laboratory burner. This could have affected the lab results by decreasing the final mass when some of the product have escaped.

Materials:Magnesium stripCrucibleCrucible coverClay triangleIron ringRetort standTongsBalanceBunsen burnerProcedure:1.obtained a strip of magnesium between 30-40 cm long2.coiled magnesium strip into a tight roll3.measured the mass of the crucible and cover4.Added the magnesium strip to the crucible and measured the

Based on my and other classmates' observations and results it can be proved that every time magnesium combines with oxygen to form Magnesium oxide the percent composition for magnesium will be 60.31% and for oxygen it will be 30.69 % (the results achieved by experiments are

Washing of the copper is necessary in this experiment to separate the iron from the copper and make sure the iron is not counted in the mass of the copper.

About 80 mL of HCl was obtained and mixed with phenolphthalein. Using a LabQuest unit and Gas Pressure Sensor kit, the HCl mixture was added to the flask with the magnesium ribbon and allowed to react. When reaction was complete, the change of temperature and gas was recorded. This procedure was repeated for different masses of magnesium ribbon (masses found on page 89 of the lab manual). After the completed procedure, moles of H₂ produced in each trial were calculated. (The actual procedure can be found on pages 87-89 of the lab manual)

There is a very easy way to find the empirical formula of a compound using the mass percentages found through elemental analysis. First, convert the mass percentages to a mass, assuming that the compound is 100g. Then convert each mass into moles using the molar masses. Then divide each of these moles by the element with the smallest amount of moles. That is the ratio of the empirical formula. Just make sure that the numbers are in whole numbers, if not, multiply by common denominators to get all of them to a whole number (3).

The purpose of this experiment is using Compleximetric titration and EDTA to determine the concentration of Mg2+ in solution; and also calculating the percent by mass of MgO in the unknown sample. This procedure results no significant deviations.

The solubility of Mg(OH)2 (Ksp = 8.9 10-12) in 1.0 L of a solution buffered (with large capacity) at pH 9.58 is:

molality m= (grams MgCl2÷95.21gmol of MgCl2)10mL H2O×1g H2O1 mL H2O×1 kg H2O1000 g H2O+grams of ice×% of ice melted×1 kg ice1000 g ice

The magnesium strips were cleaned and cut correctly by the lab technician and I measured and inspected the strip each time I started the experiment to make sure it was ok for the experiment. Most of these variables

How empirical formula of Magnesium Oxide is obtained by heating Magnesium in the presence of air?

Magnesium is a chemical element that is essential to the proper function of the human body. According to, Wikipedia, it is the eleventh most abundant element of mass in the human body. Ions found in magnesium are essential to all cells and interact with DNA, RTA and RNA; many ions require magnesium for proper function. Magnesium is also commonly used in laxatives, antacids and to help with certain diseases, such as Eclampsia.

Magnesium is an element on the periodic table with an atomic number of 12 and an atomic mass of 24.305. Its complete electron configuration is 1s2, 2s2 2p6, 3s2. The most common ion formed from magnesium is Mg+2. Magnesium can be extracted from the minerals dolomite (CaCo3 MgCO3), carnallite (KCL MgCl2 5H2O), magnetite, olivine, and serpentine. It is most often obtained from seawater, in which each cubic kilometer contains about 1.3 billion kilograms of magnesium. It is also the third most abundant structural metal in the earth’s crust, exceeded only by aluminum and iron.

Magnesium is a shiny grey solid that assembles to five other elements. Magnesium’s atomic number is 12 and it has 12 neutrons, 12 electrons and 12 protons. Magnesium’s symbol is known as Mg. It is the ninth abundant element in the universe. Magnesium was discovered by Joseph Black in 1775. It was isolated by Sir Humphry Davy in 1808. The name magnesium originates from the greek word for a district in Thessaly called Magnesia. It is related to magnetite and manganese, which too was originated from the area, and used differentiation as separate substances. Magnesium can be found both on Earth and other places in the universe. On Earth, it can be found in the crust as a compound with oxygen. A compound is when two or more elements chemically