Water of crystallization

Purpose Hydrates are inorganic salts that lose water when heated and undergo a color change. The loss of water makes the hydrate anhydrous. Copper chloride hydrate is what will be used in the lab to show what happens when a hydrate is heated which can lead to a better understanding of hydrates as a whole and their reactions that can be observed to discover things about the environment they’re in. After the removal of water from the copper chloride hydrate, the solid ,when reacted with aluminum and

Physical Quality in nutrisari, there are 3 main parameters to maintain physical stability: 1. Water and Crispness The relation between water and crispness is that the more aw in the food products, then the less crispness in it. In this case, as we talk about nutrisari (dehydrated juice) the water and crispness parameter has no interaction for the product as it is not one of the parameter for nutrisari. 2. Water and Stickiness, Caking and Collapse In dehydrated juice, caking is categorized as a problem

percent of water in a series of crystalline compounds called hydrates. Introduction Percent composition is “the relative amount of the elements in a compound, or the percent by mass of each element in the compound” (Wilbraham, Staley, Matta, Waterman). It can be calculated by two ways, and it can also be used as a conversion factor. In this lab experiment, the percent composition will be determined to figure out how much water is in three hydrates, “a chemical compound that has water in its composition

crystalline one, in which water molecules are chemically bound to another compound or an element. B) Water of hydration (crystallization)- water that is chemically combined with a substance to form a hydrate and can be expelled (as by heating) without essentially altering the composition of the substance. C) Dehydration- the loss or removal of water from something. D) Anhydrous Salt- where the crystal has had the water driven out. Purpose: To determine the number of water molecules bonded to a hydrated

may cause the release of both water and acidic vapors. A hydrate itself is a chemical, typically a crystalline salt, which incorporates water (H2O) into its chemical structure. For example, the compound CoCl2 is merely cobalt (II) chloride, however, take the original compound and attach a water molecule and it becomes CoCl2 + 6 H2O. In other words, the original cobalt (II) chloride is now cobalt (II) chloride hexahydrate. The bond between the compounds and the water molecules is weak and therefore

formula for the hydrated sample was CuCl2 ·2H2O. Thorough experimental procedure was taken to obtain the water loss of the hydrated sample, therefore defining its chemical formula. As the hydrated sample of copper chloride changed colors throughout the heating process, a change in chemical composition was noted. The hydrate was originally a blue/green color, but as it was heated and lost its water, the hydrate turned brown. This chemical composition is known as the anhydrous residue. It was observed

Performing a Procedure Used to Determine the Percent of Water in a Hydrate Objective: To determine the chemical formula for the “Mystery Hydrate” Problem: Determining the formula for the “Mystery Hydrate” Variables: Independent Variable (IV) What percent water is the Mystery Hydrate Dependent Variable (DV) The amount of hydrate left after heating Introduction “Hydrates are substances that include water in their formula. The water is not actually part of the chemical substance and this

CAPILLARY ELECTROPHORESIS Quartez O. Buckley Falcon High School/Striebel Author Note First paragraph: History behind Capillary Electrophoresis. Second paragraph: The theory behind its creation. Third paragraph: Cost of the items and it as a whole. Fourth paragraph: How’s it's used in modern times and the value of it.  Abstract Electrophoresis is the separation of proteins by the electric sequence. Electrophoresis has older and now a new technology. Gel electrophoresis is the older form, while

if it is ingested. It may also cause some skin irritation, however as long as we don’t get it into our eyes or ingest it, it is considered a safe hydrate. As for disposal, it must be transferred to a disposal or recovery container and not into open water or sewage system. This hydrate is not hazardous to keep in the house, we just need to make sure that it is kept in a container and in cool and compatible areas. The hydrate is also not too expensive and we can split the cost of twenty dollars that

Chemistry 1211L - 146 - Spring 2012   Procedure The Synthesis of Cobalt Oxalate Hydrate Place 100 ml of distilled water in a 250-ml (or 400-ml) beaker. Add 1.26g of oxalic acid dihydrate (H2C2O4.2H2O) and 1 ml of concentrated ammonia. Stir the mixture until the solid has dissolved completely. Dissolve 2.34 g of cobalt chloride hexahydrate (CoCl2.6H2O) in 100 ml of water in an Erlenmeyer flask. While stirring the oxalic acid solution constantly, add the cobalt chloride solution drop by drop