either barium (Ba 2+ ) or calcium (Ca 2+ ). Part C consisted of a series of cation flame tests using metal
In the last test, we had to test out a mystery powder (powder A, B, C), in its own separate test tube, in order to solve the Sherlock Holmes Mystery. Our group had powder C. When we mixed water in the mystery powder, it did not dissolve. When the litmus paper was put into the test tube it turned blue. When the vinegar was mixed it bubbled/foamed up. When we mixed the iodine solution, there was no reaction and the solution turned to a dark brown/black color. When we mixed in the baking soda there was no reaction and it turned to an even darker color.
The cations in both the known and unknown samples were identified by using qualitative analysis, of which were determined to be acidic, basic, or neutral by using litmus paper. Acid-base reactions, oxidation-reduction reactions, and the formation of complex ions are often used in a systematic way for either separating ions or for determining the presence of specific ions. When white precipitate formed after adding hydroxide, aluminum ion was determined to be present in the solution. However, nickel was determined to test positive when the solution changed to a hot pink color after adding a few drops of dimethylglyoxime reagent and iron was present when the solution was a reddish brown color when sodium hydroxide was added to the mixture at the very beginning of the experiment. Qualitative analysis determines that ions will undergo specific chemical reactions with certain reagents to yield observable products to detect the presence of specific ions in an aqueous solution where precipitation reactions play a major role. The qualitative analysis of ions in a mixture must add reagents that exploit the more general properties of ions to separate major groups of ions, separate major groups into subgroups with reactions that will distinguish less general properties, and add reagents that will specifically confirm the presence of individual
When combined Sodium Bicarbonate and Hydrochloric Acid, Carbon Dioxide is produced. The two chemicals do not undergo a change in color but a chemical change when CO2 is produced.
Next, chemicals and color. How can certain chemicals turn fire into a color? Well, any element placed into or within a fire will change the color. Quantum mechanics and orbitals are a couple things that are also involved in the process. Quantum mechanics constrains them to appear in various distinct patterns which are also called orbitals. Orbitals are a lot like planetary orbits, but blurrier, so you will never really be sure on where the electrons
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 observed flame colors do correlate with the brightest bands on the atomic emission spectrum for each element. Based on the information from the “ Periodic Table with Atomic Emission Spectra”, which indicates that lithium obtained the brightest band for red, sodium obtained the brightest band for orange, potassium obtained the brightest band for purple, and strontium obtained the brightest band for red. We might account for major differences in observed flame colors due to there are several brightest band on some of the elements such as barium, which obtained red, orange and blue as the brightest bands.
In this experiment, we mixed different chemicals together to see what gases we could produce. The three different gases we ended up with were Oxygen which you get when you mix Manganese Dioxide & Hydrogen Peroxide together, Carbon dioxide which you get when you mix Hydrochloric acid and Baking Soda together, and Hydrogen which you get when you mix Hydrochloric acid and Mossy Zinc together. We did a burning and glowing splint test where we would bring a burning or glowing splint to the opening of the test tube to see how the gases reacted with the flame.
In this experiment, I saw that the product of Tin (ll) Chloride mixed with Potassium Dichromate is different from the product that resulted from Tin (lV) Chloride when mixed with the same reactant that was used with Tin (II) Chloride, Potassium Dichromate. They both resulted with different colours and smell. Tin (II) Chloride resulted with a light green colour, whereas Tin (IV) Chloride resulted with bright yellow colour. Similarly, Iron (llI) Chloride had a different product when mixed with Sodium Hydroxide, Ammonium Chloride added with Aqueous Ammonia, and Potassium Ferrocyanide compared to the product of Iron (ll) Sulfate, when mixed with the same reactants that was used to react with Iron (III) Chloride. And also same for Copper (ll) Thiocyanate
Red is produced by strontium salts and lithium salts. Incandescence is light produced from heat. Heat causes a substance to become hot and glow, initially emitting infrared, then red, orange, yellow, and white light as it becomes increasingly
addition, it can be seen that the emissions intensity of the luminous flame becomes darker as the dissolved pressure increases. The Luminescence of the luminous flame is generated by carbon particles receiving heat from the flame surface, so it is deeply related to the generation of PM . Therefore, it is conceivable that the effect of effervescence of CO2 gas greatly affects the amount of PM generated.
Based off of prior knowledge the hypothesis for Lab six was that the first reaction would produce Lead Iodide, the second reaction would produce Copper II sulfide, and the third reaction would produce Iron II Hydroxide. For the unkonown solution B this hypothesis was incorrect. Based off of the calculations and the color observations the the metal product present in the first reaction was Silver Iodide, the product present in the second reaction was Copper II Sulfide, and the product present in the third reaction was Nickel II Hydroxide. Although the hypothesis was incorrect the experiment was a success because the ultimate goal were reached. The lab was created to generate understanding of solubility and stoichemtry. Through observation of
My hypothesis was if manufacturing guidelines are not followed it will dramatically affect the flame resistancy of the material. My hypothesis was supported by the data collected from the test results. I tested washing the flame resistant material as directed by the manufacturer. I also tested washing the flame resistant material not following the manufacturer’s guidelines. My results showed that following the manufacturer’s washing guidelines increased extinguish time and damage to the material. The first test showed an extinguish time of 1.99 seconds when following manufacturer’s guidelines. The first test not following manufacturer’s washing guidelines had an extinguish time of 3.13 seconds.
5mL is removed from this suspension and placed in a test tube. This is the centrifuged.