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Percent of water in hydrate theoretical Moles of water. Mass of water 360 grams.
Thus in this experiment it is our goal to determine the percent of water in an unknown hydrate as well as the formula of the hydrate.
Determining the formula of a hydrate lab. For example the anhydrous compound cobalt II chloride is blue while the hydrate is a distinctive magenta color as seen below. The hydrated form of cobalt II chloride contains six water molecules in each formula unit. The name of the compound is cobalt II chloride hexahydrate and its formula is CoCl2.
Determining the Formula of a Hydrate. A hydrate is an ionic compound that has a definite amount of water molecules attached to its crystalline structure. The ratio of water mol ecules to the anhydrous salt is constant.
Many compounds exist as hydrates. Some examples are copper II sulfate. Determining the Chemical Formula of a Hydrate Lab Denisa Wood Title.
Determining the Chemical Formula of a Hydrate Lab Purpose. In this laboratory exercise we will determine the relative amount of water in a hydrated compound. We will do this by determining the mass of Water driven out of the compound when it is heated.
When the hydrate is heated water is given off. MªXᵇ H₂O MªXᵇs H₂O You can determine the mass of water lost when a known mass of a hydrate is heated and use that information to calculate the percentage of water by mass in the hydrate. Water mass of water lost mass of hydrate x 100 This value can be compared to the value to the percentages of water in the hydrates on the list.
Then it will be possible to identify the unknown hydrate. An empirical formula of a chemical compound is the ratio of atoms in simplest whole-number terms of each present element in the compound. For example Glucose is.
Picture Data Collection Table Data Analysis Conclusion. In this lab we were trying to determine the empirical hydrates of copper II Sulfate Hydrate and of Magnesium Sulfate. In order to determine this we put both copper II Sulfate Hydrate and Magnesium Sulfate under extreme heat to evaporate the excess water.
Determining the Chemical Formula of a Hydrate Lab PurposeIntroduction. In this laboratory exercise we will determine the relative amount of water in a hydrated compound. We will do this by determining the mass of Water driven out of the compound when it is heated.
Therefore the formula is MgSO4. What is the formula for copper II sulfate. What is the mass of copper II sulfate.
Use the following data to find the formula of the hydrate BeO. Mass of hydrate 861 grams. Mass of water 360 grams.
What is the mass of the anhydrous salt. What is the formula of. Thus in this experiment it is our goal to determine the percent of water in an unknown hydrate as well as the formula of the hydrate.
This will be done through a knowledge of finding empirical formulas and percent composition. Along with you introduction and procedure construct a data table for the lab. The formula of the hydrate shows the ratio of the moles of anhydrous salt to the moles of water.
In the above case that ratio is 15. In this experiment you will be given a sample of hydrate. You will determine the mass of the water driven off by heating as well as the amount of anhydrous salt that remains behind.
The data obtained from the lab is here. Determining the Chemical Formula of a Hydrate Purpose Find the molecular formula of the hydrate of Copper II Sulfate CuSO4 x H20. Prediction When the solution is heated the hydrate will convert to an anhydrous ionic compound.
According to this calculation the empirical formula for the hydrate is BaCl 2 2H 2 O. Knowing the relative proportions of substances present make it possible to determine the empirical formula of a substance. To quickly obtain about 1 g of hydrate sample take a test tube from your locker and obtain about the same quantity of hydrate from a reagent bottle as you find in one of the reference samples.
After you obtain your sample quickly replce the cap to the reagent bottle and tighten securely. Lab 5 Determining Chemical Formula of a Hydrate Zeeshan Saleem Nikki Pandey Brandt Farazian Hoang Phan 6152015 Chem 1411S2L Abstract. The Purpose of this lab was to find the chemical formula for ZnSO 4 through determining the amount of anhydrate and hydrate.
Furthermore in order to determine the exact name of the hydrate we must find out the ratio between the anhydrate and water that are associated with the hydrate. By multiplying the mass of the anhydrate which is magnesium sulfate in the experiment with its molar mass the number of moles present at the end can be determined. By taking the mass of the hydrate and its anhydrate the molar ratio of water to salt can be found to determine the chemical formula of a hydrate.
The Law of Definite Proportions states that all samples of a given compound have the same proportions of their constituent elements. In this lab you will calculate the percent composition of water in a hydrate and determine the empirical formula of the hydrate you are working with. What two things make up hydrates.
In order to determine the percent composition and the empirical formula of a hydrate you must know how much water is in the hydrate. LAB Report 10 - Determination of the Gas Law Constant Chemlab 3 - Classification of Chemical Reactions B YOGI-bleaches - Determining the Empirical Formula of a Hydrate D. Lab - Determining the Chemical Formula of a Hydrate Some ionic compounds form crystalline structures that trap water molecules within the crystalline framework.
They are known as hydrated salts or simply hydrates. Their formulas are written in two. Mass of hydrate mass of H 2 O mass of anhydrous salt after heating.
The law of definite proportions or constant composition states that the elements in a pure compound are present in a definite. Water is not actually a part of the formula for a hydrate which is why it is written slightly different than normal chemical formulas. For copper II sulfate tetrahydrate it would be written CuSO 4H 2 O.
The indicates that 4 water molecules are loosely bonded to. Please complete BEFORE lab day. Calculate the formula of the hydrate.
For a sample data showing all work. Mass of anhydrous salt. 15961 Mass of water.
9010 Mass of Hydrate. Percent of water in hydrate theoretical Moles of water. Formula of the Hydrate.