Discussion Unknown Solution 1 I believe that the first unknown solution is made up of molecular compounds. This is because the solution had very little conductivity, meaning there was not an equal amount of ions broken down in the solution. The solution had no scattering, which means the molecular compounds were fully dissolved in their solvent, which was not water. When tap water was added to solution 1, the color changed from green to blue. If water was the original solvent, we would not see this color change. The absorption spectrum follows most of what the color green would absorb on its own: red, blue, and purple wavelengths. However, there was some absorption of the green wavelength. The first solution has the highest overall absorbance …show more content…
The transition metals are known for giving solutions a pigmentation, such as the yellow of solution 2. Furthermore, I believe the solution is made up of ionic bonds because it has the highest conductivity out of all three solutions. The ions, when broken down, create a hospitable environment for conduction. The absorbance spectrum makes sense because of the color of the solution, yellow. The wavelengths absorbed the most were blue and purple. When the sodium hydroxide was added to the solution, an orange precipitate formed. Precipitates are insoluble ionic solids, such as the precipitate formed when FeCl3 and NaOH were mixed in a previous lab session. The solution was also determined to be a strong acid by the pH strip. This means that when the bonds of the ionic compound were broken by the solvent, there was a high concentration of protons. Only metals can be positive ions, so therefore the solution must contain a heavy concentration of metal ions, and due to the conductivity, there is also a high concentration of nonmetal ions present. The last experiment we performed only proved that there were no hydroxides present, as previously mentioned. This furthers my explanation that the solution is ionic, and contains a transition …show more content…
There was scattering present, which means that there are particles present in the solution, and the clear color means that there are no dyes or transitions metals present. The absorption was extremely low for this solution, meaning that there is a low concentration of particles in the solution. However, the compounds are ionic because there was a high conductivity for this solution. When NaOH was added, there was no precipitant, because all of those molecules are already present in the solution, or at least molecules that behave in a similar fashion. There was no change in the scattering when the sodium hydroxide was added, which means the particles present remained constant. A pH strip proved the solution was neutral, much like a salt would be. The solution, when mixed with solution 1, turned solution 1 blue. This change was most likely due to the presence of hydrogen and oxygens atoms in solution 3. When tap water was added to the solution, there was no change macroscopically or with the scattering. This most likely means the solution is made up of a salt dissolved in
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
Compress the safety bulb, hold it firmly against the end of the pipette. Then release the bulb and allow it to draw the liquid into the pipette.
Thorough analysis of the graph displayed enough evidence suggesting that an increase in substrate concentration will increase the height of bubbles until it reaches the optimum amount of substrate concentration, resulting in a plateau in the graphs (figure 2). Hence; supported the hypothesis.
An explanation of the links between the topics: The dye was diffusing through the potato cells, this is the link between diffusion. Osmosis is linked to the experiment because in order for the diffusion to work the water would have to first need to go through the holes in the cells also known as osmosis. And finally Tonicity was a major part because the solution that the potato was in (pure water) was hypotonic which means that the cells had swollen which made it harder for the dye to move through the potato, and the hypertonic solution (50%salt water) did the complete opposite because instead of making the cells swell it made them shrink which made it easier for the dye to pass through the potato.
In the second experiment with the green color, I can safely conclude that the color green in this case is very soluble and we would need longer filter paper, perhaps more time to safely separate the different colors that make up the color green.
I did accomplish the purpose of the lab. First, I determined the percentage of water in alum hydrate, and the percentage of water in an unknown hydrate. The results are reasonable because they are close to the example results. Second, I calculated the water of crystallization of an unknown hydrate. Furthermore, I developed the laboratory skills for analyzing a hydrate.
In procedure A, one must know what an electrolytes is, which is a substance that produces an electrically conducting solution when dissolved in a polar solvent, in this case water is the solvent. Based on the results of the experiment it is can be concluded that the sodium chloride solution best conduct electricity. This is due part by ions being separated into Na+ and Cl- ions from the original NaCl. In other words NaCl(s) becomes Na+ (aq) + Cl- (aq). In doing so allows electricity to flow in the solution. As for the pure/distilled water not conducting electricity it is because it is very filtered free of minerals. Essentially, distilled water lack ions to efficiently conduct electricity, this also applies to the pure substance of sodium chloride and sucrose which lack ions, atoms that have a net negative or positive charge. However, according the results the sucrose is slightly conductive, which may suggest a possible contamination in the solution. At the end it can be reasoned that because ions were made in the NaCl solution, ions contribute to the conductivity.
The red and blue were most visible and were near the purple. Blue and yellow were also seen on the green. The solution line made it to around 55-60%. After a few minutes had gone by waiting to see the results from the alcohol solution, the colors showed up well. It also took about twenty minutes, and the colors showed up
The purpose of this lab is to see if changing the temperature and the surface area affects the speed of the solute dissolving. This lab relate to the things you have been learning in class because it connects to solubility and how the change in temperature, surface area, and concentration affects the rate in which a substance dissolves. In this lab we hypothesize if we increase the temperature of the vinegar, then the speed of the Alka-Seltzer would increase as well because the speed of the molecules breaking down will be faster. If we also increased the surface area of the Alka-seltzer, it will also dissolve quickly because the pieces are little. In order to complete the surface area experiment, we put our safety goggles on to prevent any
When shone through a coloured solution, the solution absorbs some wavelengths of the white light and transmits wavelengths that are not absorbed. When we look at the coloured solution, we see the transmitted light. The transmitted light is the only wavelength that is not absorbed. For example, if a solution absorbs all wavelengths except blue, the transmitted light will be blue. The transmitted light is complementary to the absorbed colour. Complementary colours are based on the three primary colours and the secondary colours that are made by mixing two of these primary colours. When two primary colours, for example, yellow and red, are mixed together, they create a secondary colour, in this example orange, that is complementary to the third primary colour, blue in this example. This is why if only orange light is absorbed from a solution, leaving primarily blue light to be transmitted, we see the solution as blue. Similarly, a solution may appear blue if it absorbs both red and yellow
To wrap things up, the lab was made for us to really comprehend about the physical properties of substances. As a result, salt, sand, and iron was used for the purpose. Then our jobs were to figure out how to separate an unknown mixture and to revive them back away from one another. By doing this lab, I got to understand the differences between pure substances, compounds, elements, and mixtures.The reason why was because we observed substances by themselves and did not use them any further such as salt and iron, this hinted these were elements due to the fact that they could not be broken down any further since they had nothing else added to them. Plus, substances such the combination of salt and iron or sand and salt were mixtures since several
Solid A was identified to be sodium chloride, solid B was identified to be sucrose, and Solid C was identified to be corn starch. Within the Information Chart – Mystery White Solid Lab there are results that distinguishes itself from the other 4 experimental results within each test. Such as: the high conductivity and high melting point of sodium chloride, and the iodine reaction of corn starch. Solid A is an ionic compound due to its high melting point and high electrical conductivity (7), within the Information Chart – Mystery White Solid Lab there is only one ionic compound which is sodium chloride, with the test results of Solid A, it can be concluded that is a sodium chloride. Solid B was identified as sucrose due to its low electrical
The presence of a colored precipitate represents a pattern in the electron configuration of cations. When the outer p orbital of the ion of the metal is full, the precipitate of the product is white and no other color is present. When the outer d orbital of an ion is not completely full, the precipitate of the product is a true color. When the d orbital is completely full, the color of the precipitate is not a true color. Magnesium sulfate, aluminum chloride, and calcium chloride had a white precipitate after reacting with sodium hydroxide. Sodium chloride remained a clear liquid. The ions of magnesium, aluminum, calcium, and sodium have complete outer p orbitals and have no d orbitals. The precipitates and/or the liquids were colorless because
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
In this experiment the Sodium Hydroxide solution went through three different phases where its quality and quantity changed. The first phase was called I. Preparing Approximately 0.1M NaOH, 1000mL of clear distilled water was boiled and then chilled to room temp.