Percent water in a hydrate
What is the identity of the unknown hydrate? Statements like, "see data table for values" are not acceptable! On the other hand, some hydrated compounds tend to spontaneously loose their water of hydration when they are placed in a dry environment.
Percent hydrate calculator
Solution: 4. Accurately weigh a clean, dry crucible. This third section is where you not only present your data, but also use the values you obtain as evidence in your reasoning. Be sure to write in a persuasive style; you are trying to convince others that your explanation is acceptable or valid! Solution: 1 Determine mass of water driven off: 4. We can also via stochiometric and molar ratios , calculate the ratio of salt to water. Note that the dot in the formula or multiplication sign indicates that the waters are there. The water in the hydrate referred to as "water of hydration" can be removed by heating the hydrate. Place the crucible with cover on the clay triangle. During heating, some of the hydrous salt may have spattered, thus removing a portion of the hydrous salt from the crucible A more likely source of error, considering that this would result in a greater difference between the two ratios, and percentages. Generally, you need one page for the first two sections and the second page for the third section. Dispose of the barium chloride in the container provided. This will ensure that all the water is driven completely out of the compound.
What is the formula of the hydrate? Some of these compounds absorb water to such an extent that they actually dissolve in the water that they take up. To achieve this, a known mass of hydrated salt was heated, evaporating the water essentially distillation. As such, there is always the possibility of inaccuracies with measurement, perception of measurement, inaccuracies of equipment, and other such errors.
Percent composition of water in a hydrate lab
See the handout provided for details on this process. The mass was reduced to 7. In this experiment, the amount of water associated with a salt will be determined. The difference between the hydrate mass and anhydrate mass is the mass of water lost. Calculate the number of waters of hydration in the formula from this information. However, this is not likely to be the sole cause of the inaccuracies within this experiment, though it may contribute to it. Determine the value of n. Your report should answer these questions in 2 pages or less. When I realized the lack, I put three examples here as opposed to their own separate file and included another in the problems. Solution: Ignore the water of hydration for a moment. The Bunsen Burner Getting Started The unknown hydrate may be any of the compounds in the table on the design page. Find the mass of anhydrous salt remaining.
What is the experimental value of the percent water of hydration? Suppose the crucible and cover were not heated to dryness after being rinsed with distilled water.
When I realized the lack, I put three examples here as opposed to their own separate file and included another in the problems. Gypsum is a hydrate with two water molecules present for every formula unit of CaSO4.
We can also via stochiometric and molar ratioscalculate the ratio of salt to water. Example 1: A
Mass percentage of water in copper sulfate
Make sure that the cover is askew. Caution: Only heat to temperature needed to remove water, excess heat will result in oxidation of the salt. Caution: Wear goggles at all times. Procedure 1 Be sure to weigh your empty test tube, so you do not lose material transferring between containers. Then heat the sample more strongly for 10 more minutes by bringing the flame of the bunsen burner directly under the dish. Section 3: What is your argument? Many anhydrous compounds have a strong tendency to absorb water vapor from the air, thus becoming hydrated compounds. After receiving directions from your instructor, heat the crucible and cover using a Bunsen burner for about five minutes. Would the calculated percent water be lower or higher than the actual one? Unlikely, considering that the ratios between the two, both stoichiometric and percent water content, would be smaller in such an instance.
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