In conclusion, hydrates were determined and identified. A hydrate is a compound, typically a crystalline one, in which water molecules are chemically bound to another compound or an element. If a hydrate is heated in a test tube and water condenses inside it, we determined that the substance was a hydrate. Hydrates were identified as nickel chloride, sodium tetraborate, sucrose, calcium carbonate, and barium chloride. Sucrose, in particular, showed a high percentage of water. A true hydrate will dissolve in water and produce a solution with a color very similar to the hydrate’s original color. If not, then the solution was not classified as a hydrate. Water solubility also has a play in whether a solution is a hydrate or not. The hydrates …show more content…
In our observations, chloride hexahydrate began as the color pink and, when heated, changed from purple then to light blue. When water was added to the residue, it turned pink yet again, then turned from purple and finally to light blue. It was concluded that the dehydration and hydration of CoCl2 is reversible. The reversibility of hydration for chloride hexahydrate:
CoCl2 ∙ 6 H2O ↔ CoCl2 + 6 H2O The efflorescence and deliquescence was determined for all the compounds. Efflorescence is the tendency of a compound to lose water to the air while deliquescence is the tendency of a compound to gain water from the air. KAl(SO4)2 ∙ 12 H2O was classified as an efflorescent compound because it lost mass after being opened to the air. The other compounds, CaCl2, CuSO4, and CoCl2, were all deliquescent compounds and gained mass after being opened to the air. Percent water in the unknown hydrate was determined to be twenty-one percent. Number of moles of water per mole of unknown hydrate was found to be in a ratio of 2:1. Observations were slightly incorrectly recorded in the identification of hydrates. Calculations to determine percent water in the unknown hydrate and the number of moles of water per mole of unknown hydrate were miss
The purpose for this lab was to use aluminum from a soda can to form a chemical compound known as hydrated potassium aluminum sulfate. In the lab aluminum waste were dissolved in KOH or potassium sulfide to form a complex alum. The solution was then filtered through gravity filtration to remove any solid material. 25 mLs of sulfuric acid was then added while gently boiling the solution resulting in crystals forming after cooling in an ice bath. The product was then collected and filter through vacuum filtration. Lastly, crystals were collected and weighed on a scale.
The purpose of the Unknown White Compound Lab was to identify the unknown compound by performing several experiments. Conducting a solubility test, flame test, pH paper test, ion test, pH probe test, conductivity probe test, and synthesizing the compound will accurately identified the unknown compound. In order to narrow down the possible compounds, the solubility test was used to determine that the compound was soluble in water. Next, the flame test was used to compare the unknown compound to other known compounds such as potassium chloride, sodium chloride, and calcium carbonate. The flame test concluded that the cation in the unknown compound was potassium. Following, pH paper was used to determine the compound to be neutral and slightly
At this point the identity of the unknown compound was hypothesized to be calcium nitrate. In order to test this hypothesis, both the unknown compound and known compound were reacted with five different compounds and the results of those reactions were compared. It was important to compare the known and unknown compounds quantitatively as well to ensure that they were indeed the same compound. This was accomplished by reacting them both with a third compound which would produce an insoluble salt that could be filte...
Solubility test was used to determine if unknown white compound was soluble in water. To conduct the solubility test, many materials were used such as flask, glass rod, scale, and chemical used was unknown white compound. First, 0.25 gram of unknown white compound carefully measured on scale. Then, the 0.25 gram of unknown white compound added to 100 mL of water and dissolved it using the glass rod. While the unknown
Afterwards, we conducted crystallization to evaporate the liquid in an attempt to detect the presence of a salt. Before stating which of the potential
This can be done by first finding the products of the chemical reactions, which are found by swapping the anions on each reactant. Once this is done, predictions can be made. The table above, describes the solubility rules, these are used to decide whether a compound will be soluble, and then consequently to this reveal a precipitate. Barium sulfate for example is insoluble and if it was to be mixed with an aqueous compound, barium sulfate would be the precipitate. This is an example of how a prediction can be made, without physically viewing the experiment or given the results. It is also a way of identifying what the precipitate is once the experiment has been
We collected 0.994 g of (NH4)2HPO4, which was less than our initial calculations recommended. This caused the (NH4)2HPO4 to be the limiting reagent in our reaction instead of the hydrate, which lowered the amount of hydroxyapatite produced. While transferring the reaction solution into the vacuum filter, some of it was left behind on the walls of the beaker. Also when we took filtered product out of the vacuum funnel, some product was lost, causing our weighed mass of the product to be less than was actually produced in the reaction.. Lastly, while testing the solubility of the product in acid, we did not record the amount of product dissolved in the acids, and so we lost an unknown amount of product in this step as well. All of these losses of product will contribute to a lower percent yield calculation when we weigh the dry sample of the
The experiment is aimed at giving a better understatement of osmosis process and the different conditions in which osmosis occurs.
The % composition by mass of oxygen in Potassium Chlorate was found to be 43.4%.
A cuvette was filled 3/ 4ths of the way and the absorbance measured in a spectrophotometer. The data was compiled as a class and recorded. The Spectrophotometer was blanked using a test tube of distilled water.
For the solubility test we were told to try and dissolve our unknown substance into water (H20), Sodium Hydroxide (NaOH), Hydrochloric Acid (HCl), Toluene, and Acetone. Our unknown substance was soluble in water, but not soluble in Toluene or Acetone.Our substance dissolved in water that means that it has to be some type of ionic compound. But, if our substance dissolved in Toluene, which is an organic solvent, then our substance would be non-polar. From these results we concluded that our substance was ionic because substances dissolve in other substances that are similar to it: “like dissolves like.” A substance will dissolve in something that it is similar to.
...dity variation, largely because RH is not a variable expressed in the Arrhenius equation. It is likely that the Copan researchers, like the experimental parameters of Michels and colleagues (1983) might consider the RH of tropical soils to be always 100 percent. For contexts deeper than 50 cm, this may be a reasonable assumption. However, it should be borne in mind that the majority of the variability in hydration rates occurs between RH values of 90 and 100 percent, and a 1 percent change in RH translates to approximately a 3 percent change in hydration rate (Tremaine 1989). So if blades from Copan were recovered from contexts with 90 percent RH, their OHD dates would be in error by approximately 30 percent, excluding all other sources of error.
Brackish water, brine, or chlorinated water may be trapped in a geological medium may be mixed with water closer to the surface, given the right conditions.
Water is a good solvent and picks up impurities easily. Pure water -- tasteless, colourless, and odourless -- is often called the universal solvent. Dissolved solids" refer to any minerals, salts, metals, cations or anions dissolved in water. Total dissolved solids (TDS) comprise inorganic salts (principally calcium, magnesium, potassium, sodium, bicarbonates, chlorides, and sulphates) and some small amounts of organic matter that are dissolved in water. TDS in drinking-water originate from natural sources, sewage, urban run-off, industrial wastewater, and chemicals used in the water treatment process, and the nature of the piping or hardware used to convey the water, i.e., the plumbing. In the United States, elevated TDS has been due to natural environmental features such as mineral springs, carbonate deposits, salt deposits, and sea water intrusion, but other sources may include: salts used for road de-icing, anti-skid materials, drinking water treatment chemicals, storm-water, and agricultural runoff, and point/non-point wastewater discharges. In general, the total dissolved solids concentration is the sum of the cations (positively charged) and anions (negatively charged) ions in the water. Therefore, the total dissolved solids test provides a qualitative measure of the
The simplest experiment for this type of situation would be to use red and blue litmus paper to distinguish between acids, bases and salts. Hydrochloric acid (HCl) makes blue litmus paper change color going from blue to red, making it an acid. Sodium hydroxide (NaOH) makes red litmus paper change color going from red to blue, making it a base. Sodium chloride solution (NaCl) is neutral, since it would only soak blue and red litmus paper, considering that it is a by product of when an acid and a base mix together, neutralizing each other.