Hydrates Lab

The purpose of this lab is to determine the formula of an unknown hydrate. To achieve this, we heated a hydrate over a Bunsen burner to drive out the water. As a result, the anhydrate is left and the data is used to calculate the mole ratio between the amount of anhydride and water. Then the mole ratios are used to calculate the hydration number, which was 4.8, but was rounded to 5 in the formula. The accepted formula is 〖CuSO〗_4∙5H_2 O and the percent of error was 4%.

6-3: This process is used by cells to manufacture _biochemical energy from nutrients into adenosine triphosphate (ATP), and then release waste products__

This experiment is based on determining the chemical formula for a hydrated compound containing copper, chloride, and water molecules in the crystal structure of the solid compound, using law of definite proportion. The general formula of the compound is CuxCly•zH2O, and aim is to determine chemical formula of this compound.

The main objective of this experiment is to differentiate between a physical change and a chemical change.

The purpose of this experiment was to determine the percent by mass in a hydrated salt, as well as to learn to handle laboratory apparatus without touching it. The hydrated salt, calcium carbonate, was heated with high temperature to release water molecules. Gravimetric analysis was used in this experiment to determine the percent by mass of water in a hydrated salt. The hypothesis of this experiment was accepted on the basis that the percent by mass of volatile water in the hydrated salt would be fewer than 30%. The percent by mass was determined by the mass of water loss devised by the mass of hydrated salt multiplied by total capacity

The objective of this experiment will be to combine various substances, liquids and metals, and to observe their behavior when they are combined. The types of reactions observed shall determine the nature of these reactions: physical or chemical.

The mass percent of water was determined using the mass of water and dividing it by the total mass of the hydrate and then multiplying that answer by 100%. The number of moles of water in a hydrate was determined by taking the mass of the water released and dividing it by the molar mass of water. The number of moles of water and the number of moles of the hydrate was used to calculate the ratio of moles of water to moles of the sample. This ratio was then used to write the new and balanced equation of the dehydration process. The sample was then rehydrated to the original state and the percent of the hydrate recovered was calculated by using the mass of the rehydrated sample by

Background: According to George B. Kauffman of Britannica, a hydrate is “any compound containing water in the form of H2O molecules, usually, but not always, with a definite content of water by weight.” Within this, there are two aspects of the compound; the “water of hydration” and the anhydrous salt. When a hydrate is heated, the “water of hydration” leaves the compound as vapor due to the unsteady bonds between the water and salt molecules. The anhydrous salt ends up becoming the only piece that is leftover. From the two, the percent water in a hydrate and the mass of the salt can be determined from the loss of the “water of hydration.” As a result, the formula of the compound can be found because the masses of the salt and the water can be used to determine the mole ratio, which are both small, whole numbers.

There was an assortment of different changes indicating that chemical changes were taking place such as change in color or chemicals bubbling when combined with another chemical.

1. Place a small amount of wax from a birthday candle into a test tube. Heat gently over a burner flame until the wax melts completely; then allow

The first part of the lab began by one lab member adding 10.0 mL of DI water to a test tube while another lab member obtained a beaker full of ice and salt. After both these steps were complete the test tube was put in the beaker full of ice. Immediately following the test tube be being placed in the beaker, a temperature probe was inserted into the test tube. The initial temperature was recorded and after the temperature was recorded in 30 second increments. Once the water exhibited supercooling and then remained consistent at .1 °C for 3 readings it was determined that the water had froze and formed crystals. Evidence that crystals formed allowed for it to be confirmed that the water actually hit freezing point at .0

The goal of this experiment was to determine the empirical formula for a hydrate of magnesium sulfate and water. The technique that was used was measure the mass of the hydrate and then apply heat to evaporate the water. Then determine the mass of water that was in the hydrate and the mass of the remaining magnesium sulfate. The equation for the hydrate is determined by calculating the mole to mole ratio of the water and the anhydrous. The resulting formula will be formated as: MgSO4*_H2O

The results of the experiment show that the mass of the hydrate decreases as the temperature increases. In the Hydrate Lab, this was found when every single time the hydrate was heated, the mass got lower, but slowly for this specific experiment. When it was heated, all the water was disappearing. This fact can also be defended when Weiner, Susan A., and Edward L Peters states, “Upon heating, the water can be evaporated leaving an anhydrous salt”(para.3). The purpose of this lab is to determine the percent composition of water in a hydrate and to calculate the number of moles of water found in the hydrated salt.

A compound had a constant composition and as a hydrate it is considered a pure substance. According to the law of definite proportions, a compound always contains the same elements in the same proportions by mass, regardless of the amount of the sample, where it was found, or how it was prepared. The hydrate contains water molecules that are not easily detected by the naked eye, it looks rather dry and

The dissociation process of Kr hydrate at 260 K were further examined in detail. The radial distribution functions (RDFs) for O–O, O–H, Kr–O, Kr–Kr pairs simulated at five different time period (0-30 ps, 90-120 ps, 120-150 ps, 150-180 ps and 180-210 ps) at temperatures of 260 K and pressure of 1.05 MPa are compared in Fig. 3. The first O–O peak locates at 2.75 Å, corresponding to the typical O–O distance between two neighboring water molecules interacting with a hydrogen bond. The second O–O peak (at 4.51 Å) in Fig.