Iron Chloride Lab Report

One change that demonstrates a positive test in this lab is precipitate forming. If silver nitrate solution is mixed with a substance and a precipitate forms, chloride ions must be present in that substance. Another change the demonstrates a positive test in this lab is a colour change to a dark red colour. If potassium thiocyanate is mixed with a substance and the colour of the substance changes to dark red, Iron (III) ions must be present in the substance. Why do you think chemical tests, similar to tests used in this investigation are called

The primary goal of this laboratory is to correctly identify an unknown substance. To achieve this task, one may use various tests that reveal both chemical and physical properties of a substance. By comparing the results of a known substance and the unknown substance, one may eliminate alternative possibilities and more accurately predict the undisclosed compound. Furthermore, by performing these tests, data can be collected and verified regarding chemical and physical properties of the unknown. Understanding the chemical properties of a known substance aids one’s understanding of the unknown based on comparative analysis of the results of the tests.

Continually, the solution was allow to cool down, before it was reheated to dissolve the solid. The solution stood undisturbed until crystals were formed. Solubility tests were performed on all possible solvent-solute pairings. The most efficient pair was

Objective: The purpose of this experiment was to test various materials, using benedicts reagent, iodine, and biuret reagent

The sticks were then briefly placed under a flame, and the respective colors were identified. Barium chloride produced a yellow color, copper chloride produced a green color, calcium chloride gave off a neon orange hue, potassium chloride emitted a lavender flame, lithium chloride gave off a red pink color, and sodium chloride gave off an orange color. Now, in Part A the silver cation was found present in unknown solution number 4. In Part B, the barium cation was also identified in the solution. By the creation of a precipitate, or lack thereof, the presence of either cation was discovered.

The original color of each compound was recorded. After this, two more drops of the compounds were added to the individual wells so that each well would contain a unique combination of two compounds. Once this was completed, it was determined which solutions had reacted by whether or not a precipitate formed in the solution. If a precipitate had formed, the new color of the solution was recorded.

These test tubes were mixed thoroughly and then each one was placed into the Spectrophotometer to measure the absorbance of each using the maximum wavelength of absorption found in the first part of the lab. Students recorded the absorbance of each solution and then calculated the concentration of each. Using the same wavelength maximum, students measured the absorbance of the beverage solution in the

Flame Test Lab Report The purpose of this lab was to identify the colors of specific elements in there solid and liquid state when put into a flame. My theory was that when we put the element into the fire it would become excited and absorb the flame to make a different colored light appear. When it is in its ground state it is just plain and dull with no light coming off of the element. The element will absorb many stuff while getting into the excited state.

In order to identify the six unknown substances, the experimenter must perform multiple tests. Such as solubility tests (water and hexane), melting point, conductivity, and bond type. The solubility test will narrow down the list of potential unknown substances, given in the packet, by considering the characteristics of the unknown substances. For instance, unknown substance #2 was tested in both water and hexane solubility; at the end of the trial of solubility tests of unknown substance #2 resulted only soluble in hexane.

The purpose of this lab was to distinguish observation from interpretation during a chemical reaction. In the lab, copper (II) chloride dihydrate, CuCl2 was added to water to make a solution and aluminum foil was then also added after. CuCl2 crystals were the color turquoise and when added to water turn green. After stirring, they all dissolved to make a teal solution. When the aluminum foil was added, the temperature of the solution went from 24.9 C to 94.2 C. The solution also started to bubble and foil started corroding before falling off to the bottom then most of the foil dissolved which made the water a brownish red color.

When the ion Fe3+ combines with another element the compound it forms is called a ferric compound. Rust is a classic example of a iron compound. For something to rust it requires metal water and oxygen. Iron won’t rust in pure oxygen that is moisture free just like it won’t rust in pure water that is free of extra oxygen. When I and oxygen and water meet rust is formed, rust is the common name for ferric oxide.

This experiment needed water, alcohol, and oil. To begin with, obtained a small amount of water into a test tube, then obtained the small amount of oil into the same test, and finally obtained a small amount of oil to the same test tube. Last but not least was to observe the reaction and record the result to the lab notebook. These steps were repeated with the same liquids but different order of liquids were obtained in the test tube.

Hypothesis: If the solutions react with a particular halide ion, then it will be able to identify each halide as an unknown and subsequently identify two halide ions mixed together in solution.

Unfortunately, due to me getting sick me and my partner were not able to pick a powder for are partner to identify, while they were out of the room. Our guess of what we thought the powder was, was suppose to be are hypothesis. Since we weren’t able to that, we don’t have a hypothesis. Also me and my partner weren’t able to look at the four different powders under a microscope, due to me getting sick and leaving early.

4. Spot the solution on a TLC plate and check with UV light to see