Water Hydration Lab Report

Coursework Equipment List • Boiling tubes (8) I will use these because this is where I will mix both the sodium carbonate and the strontium nitrate in order to form the precipitate. I need 8 because I am going to add 8 different amounts of strontium nitrate (1-8cm³) to the 8cm³of sodium carbonate. • Measuring cylinder (1) I will use this to measure the 8cm³ of sodium carbonate and the varying amounts of strontium nitrate to put into the test tubes. • Sodium Carbonate (enough to fill 8 boiling tubes with 8cm³/64cm³)

The goal of this experiment is to find out what is the identity of the unknown hydrate? To answer this question first, we should know what a hydrate, and how to identify a hydrate using the law of constant proportions. A hydrate is a pure substance because it contains water molecules embedded in its crystal structure that does not vary. By heating the unknown hydrate, we can calculate the mass of the hydrated, and the percentage of water in the hydrate.

Students first prepped for the lab by cleaning out the crucible. Three boiling chips were added in the crucible once it was wiped out with a paper towel. The crucible was then placed on a clay triangle two finger widths above the Fischer burner. After 10 minutes of the crucible being directly under the flame, the it was clean and students allowed time for it to cool down. Next, the students from then on used tongs to transport the crucible from weighing it and back to the clay triangle.

Goals The primary goal of this experiment was to identify an unknown compound by running various tests to determine the qualitative solubility, conductivity, and pH value of the compound. Tests were also performed for the presence of specific cations and anions in the compound. The second goal was to discover the reactivity of the unknown compound by reacting it with different types of substances. The third goal of this project was to calculate the quantitative solubility of the unknown compound in water.

Then an estimated (by trial and error) 1-3 grams of hydrated copper sulfate was added to a crucible with the lid on top. The total mass of the hydrated copper sulfate was recorded by subtracting the total mass of the crucible, lid, and sample from the mass of the crucible and lid (described in table 1.3). By attaching the wire triangle to the ring, the crucible was able to sit securely while having the bunsen burner underneath. Lighting the burner once again, each substance was heated for several minutes until estimated that the compound had changed color. Once a prevalent color change had been observed at approximately 4 minutes (blue green color) the crucible was set on the counter using the tongs to cool for approximately 5 minutes.

The dehydration of 2-methylcyclohexanol takes place at the bottom of the Hickman still. As the Hickman still heats up within the sand bath, the products evaporate and travel higher up in the still where they condense into a liquid and fall within the collection ring, thus separating the product from the remaining water. Drierite (CaSO4) is also added as a drying agent to absorb any leftover water within the product. The purity of the product will then be analyzed with infrared spectroscopy, paying attention to OH peak if it is present. Chemical Reactions: Data and Observations: Material Volume Mol.

3mL of the liquid in each of the vials were added into cuvettes and measured in the spectrophotometer. Before each time point the photo spectrometer was zeroed using a cuvette with 3mL of distilled water. If any of the results were considered unusual the machine was zeroed again and the sample was retested. The results from the spectrophotometer test were recorded in a table. The experiment was repeated six times to gain a sample size of six.

Introduction The intent of this experiment is to understand how hot and cold water interact with each other by combining clear hot water and black ice cold water. I hope to learn more about how hot and cold water interact with each other. As of now, I know that cold water is denser than hot water. Knowing this I formed my hypothesis.

In the round-bottom flask (100 mL), we placed p-aminobenzoic acid (1.2 g) and ethanol (12 mL). We swirled the mixture until the solid dissolved completely. We used Pasteur pipet to add concentrated sulfuric acid (1.0 mL) to the flask. We added boiling stone and assembled the reflux. Then, we did reflux for 75 minutes.

Materials: The materials that I will be utilizing during these experimentations are three to four ice cubes, one cup for measuring, six unblemished cups, one stopwatch, one hot water source, three tablets of Alka-Seltzer, one thermometer that measures from negative

Weighed 1 gram of NaC2H3O2 and mixed it with ionized water. Boiled 12 mL of 1.0M Acetic Acid added into a beaker containing the sodium carbonate on a hot plate until all the liquid is evaporated

To start this experiment the first step is to equip a 500-mL three-neck round bottom flask with a reflux condenser, dropping funnel, glass stopper, and a calcium chloride drying tube. Place a heating mantle under the flask in order to aid stirring. Next, grind 0.0411 moles of magnesium turnings and place them into the flask. Once added, prepare a 1.1 equivalent of bromobenzene, and then

The objectives of this experiment were to use knowledge of chemical formulas and chemical nomenclature to experimentally determine the empirical formula of copper chloride. Common laboratory techniques were used to conduct a reaction between copper chloride and solid aluminum in order to get rid of the water of hydration. The amount of water of hydration in the sample of copper chloride hydrate was calculated by measuring the mass before and after heating the sample. Afterwards, an oxidation-reduction reaction was conducted, resulting in elemental copper.

Materials 1 calibrated thermometer, 1 scale that reads mass, 2 Styrofoam cups, 1 small lead sinker, boiling water in a beaker, 1 pair of kitchen tongs, 1 small cooking pot, stove top, distilled water, and 1 pair of safety goggles (I did not use a cork stopper). III. Procedure First, the beaker

Afterwards, have the flask sit on the wire guaze on the iron ring and stand and attach it to the distillation