Three Unknown Red Solutions
Discussion
The four experimental techniques used in this proposal was aimed to complete the goal of answering questions about the system of three unknown red solutions. Based on the experiments conducted and the data collected, I am able to conclude information about the three red solutions that will lead to a possible identity of each red solution. Starting with red solution #1, we are able to conclude that there are no nanoparticles in this solution and that is a molecular compound due to the fact that when potassium iodide was added, there was no color change and no precipitate formation to indicate that a chemical reaction had happened. Having no color change occur when an ionic compound is added to a solution means that the solution is …show more content…
not ionic because there is no reaction happening, and no dissociation. We can conclude that there are no nanoparticles in Red #1 because when ionic solutions are added to nanoparticles, they clump together and cause a color change. Now that we know Red #1 is a molecular compound, we can bring in the possibility of Red #1 being water with food dye or some sort of powder causing the color to be light pink. I had also smelled this solution and it smelled very sweet, much like Kool-Aid or pink lemonade. This data could lead to future experiments to try and solidify the hypothesis of Red #1 being Kool-Aid or pink lemonade by obtaining water, a packet of each power, two 50 mL beakers, a graduated cylinder, and 10 mL of red solution #1. Measuring out 10 mL of water into each beaker and adding each powder into the beaker until the color of that solution is extremely similar to that of Red #1 then looking through a microscope to see if the molecular structure is the same, can conclude the hypothesis of whether or not Red #1 is in fact Kool-Aid or pink lemonade. If it is not, then further experiments can be determined afterwards.
Based off of data collected for red solution #2, we concluded that this solution is an ionic compound because there was a color change in the solution when potassium iodide was added and nanoparticles were present.
The reason that a color change occurred when KI was added to the solution was because KI is ionic and when it was added to Red #2, the molecules dissociated causing the color to change. Also, due to the fact that when ionic solutions are added to nanoparticles, they clump together and cause a color change, we can conclude that there are indeed nanoparticles in this red solution. There are a wide variety of ionic compounds to choose from that could potentially match the molecular structure of Red #2. In order to determine the identity of this solution, a future experiment will have to be conducted because there is not enough evidence to fully conclude what Red #2 is based off of the four experiments conducted. Since we know that Red #2 is ionic, we know that a precipitate will form if a certain ion is added to the solution and they are not soluble. A future experiment that can be performed to try and identify this red solution is to obtain 50 mL of red solution #2, a graduated cylinder, ten 50 mL beakers, a scale, a stir bar, and different elements that are known to be insoluble using a common solubility chart such as one found here: http://www.flinnsci.com/store/Scripts/prodView.asp?idproduct=16645. Measure equal amounts of Red #2 into each of the beakers, then …show more content…
add different compounds to each beaker that are insoluble, and stir until a precipitate forms. After recording observations, we will be able to narrow it down to a certain ionic compound that red solution #2 will be.
Based off of data collected for red solution #3, we concluded that this solution is a highly ionic compound because the conductivity of this solution was the highest (31210 µS/cm) out of all the other solutions.
There was also a color change in the solution when potassium iodide was added and nanoparticles were present. The reason that a color change occurred when KI was added to the solution was because KI is ionic and when it was added to Red #3, the molecules dissociated causing the color to change. Also, due to the fact that when ionic solutions are added to nanoparticles, they clump together and cause a color change, we can conclude that there are nanoparticles in this red solution. In order to determine the identity of this solution, a future experiment will have to be conducted because there is not enough evidence to fully conclude what Red #3 is based off of the four experiments conducted. Due to the strong conductivity of this red solution, it is possible that it is a strong acid or base because those are also ionic compounds. A future experiment that can be performed to try and identify this red solution is to obtain 50 mL of red solution #3, a graduated cylinder, five 50 mL beakers, a scale, a stir bar, deionized water, and all the strong acids and bases. We can then find the conductivity of each of the acids and bases using the same procedure as used for experiment 2 to see which acid or base has a conductivity most similar to Red
#3.
Conclusion
My proposal of the qualitative analysis for three unknown red solutions had a goal to answer questions about the system by conducting four experimental techniques including wavelength, conductivity, nanoparticles, and ionic compounds. The wavelength technique used for this proposal included using a spectrophotometer to measure the maximum wavelength of each solution to determine if they had the same 묬max and if they did then it was concluded that the three red solutions are comprised of the same molecules, and if they did not then they were not comprised of the same molecules. After performing this experiment, it was established that the three red solutions did not consist of the same molecules, so another experiment was proven to determine the conductivity of each of the solutions. A conductivity probe was used to measure the conductivity of each solution to see which one had the highest measurement. It was determined that Red #3 had the highest conductivity, concluding it to be the strongest ionic compound out of the three red solutions. The third experiment used a laser beam to shine through each solution to see if it contained nanoparticles. The laser beam came out as a horizontal line for Red #2 and Red #3, ultimately causing them to be ionic compounds if the color changed when potassium iodide was added. Adding KI to each solution allowed us to observe any color changes that occurred. Red solution #2 and #3 both changed color when KI was added, just as predicted. All of these techniques and goals were used to propose an identity of each of the red solutions. Red solution #1 is anticipated to be Kool-Aid or pink lemonade due to the sweet smell and the fact that it is a molecular compound. Red solution #2 is predicted to be hydrogen sulfate for the reason that it is an ionic compound. Lastly, red solution #3 is expected to be perchloric acid because it is one of the strongest acids. Along with undertaking these future experiments, another experiment involving the absorbance could have also taken place but we are unsure of the concentration so applying a Beer’s Law plot was not applicable to this proposal.
The four experimental techniques used in this proposal was aimed to complete the goal of answering questions about the system of three unknown red solutions. Based on the experiments conducted and the data collected, I am able to conclude information about the three red solutions that will lead to a possible identity of each red solution. Starting with red solution #1, we are able to conclude that there are no nanoparticles in this solution and that is a molecular compound due to the fact that when potassium iodide was added, there was no color change and no precipitate formation to indicate that a chemical reaction had happened. Having no color change occur when an ionic compound is added to a solution means that the solution is …show more content…
not ionic because there is no reaction happening, and no dissociation. We can conclude that there are no nanoparticles in Red #1 because when ionic solutions are added to nanoparticles, they clump together and cause a color change. Now that we know Red #1 is a molecular compound, we can bring in the possibility of Red #1 being water with food dye or some sort of powder causing the color to be light pink. I had also smelled this solution and it smelled very sweet, much like Kool-Aid or pink lemonade. This data could lead to future experiments to try and solidify the hypothesis of Red #1 being Kool-Aid or pink lemonade by obtaining water, a packet of each power, two 50 mL beakers, a graduated cylinder, and 10 mL of red solution #1. Measuring out 10 mL of water into each beaker and adding each powder into the beaker until the color of that solution is extremely similar to that of Red #1 then looking through a microscope to see if the molecular structure is the same, can conclude the hypothesis of whether or not Red #1 is in fact Kool-Aid or pink lemonade. If it is not, then further experiments can be determined afterwards.
Based off of data collected for red solution #2, we concluded that this solution is an ionic compound because there was a color change in the solution when potassium iodide was added and nanoparticles were present.
The reason that a color change occurred when KI was added to the solution was because KI is ionic and when it was added to Red #2, the molecules dissociated causing the color to change. Also, due to the fact that when ionic solutions are added to nanoparticles, they clump together and cause a color change, we can conclude that there are indeed nanoparticles in this red solution. There are a wide variety of ionic compounds to choose from that could potentially match the molecular structure of Red #2. In order to determine the identity of this solution, a future experiment will have to be conducted because there is not enough evidence to fully conclude what Red #2 is based off of the four experiments conducted. Since we know that Red #2 is ionic, we know that a precipitate will form if a certain ion is added to the solution and they are not soluble. A future experiment that can be performed to try and identify this red solution is to obtain 50 mL of red solution #2, a graduated cylinder, ten 50 mL beakers, a scale, a stir bar, and different elements that are known to be insoluble using a common solubility chart such as one found here: http://www.flinnsci.com/store/Scripts/prodView.asp?idproduct=16645. Measure equal amounts of Red #2 into each of the beakers, then …show more content…
add different compounds to each beaker that are insoluble, and stir until a precipitate forms. After recording observations, we will be able to narrow it down to a certain ionic compound that red solution #2 will be.
Based off of data collected for red solution #3, we concluded that this solution is a highly ionic compound because the conductivity of this solution was the highest (31210 µS/cm) out of all the other solutions.
There was also a color change in the solution when potassium iodide was added and nanoparticles were present. The reason that a color change occurred when KI was added to the solution was because KI is ionic and when it was added to Red #3, the molecules dissociated causing the color to change. Also, due to the fact that when ionic solutions are added to nanoparticles, they clump together and cause a color change, we can conclude that there are nanoparticles in this red solution. In order to determine the identity of this solution, a future experiment will have to be conducted because there is not enough evidence to fully conclude what Red #3 is based off of the four experiments conducted. Due to the strong conductivity of this red solution, it is possible that it is a strong acid or base because those are also ionic compounds. A future experiment that can be performed to try and identify this red solution is to obtain 50 mL of red solution #3, a graduated cylinder, five 50 mL beakers, a scale, a stir bar, deionized water, and all the strong acids and bases. We can then find the conductivity of each of the acids and bases using the same procedure as used for experiment 2 to see which acid or base has a conductivity most similar to Red
#3.
Conclusion
My proposal of the qualitative analysis for three unknown red solutions had a goal to answer questions about the system by conducting four experimental techniques including wavelength, conductivity, nanoparticles, and ionic compounds. The wavelength technique used for this proposal included using a spectrophotometer to measure the maximum wavelength of each solution to determine if they had the same 묬max and if they did then it was concluded that the three red solutions are comprised of the same molecules, and if they did not then they were not comprised of the same molecules. After performing this experiment, it was established that the three red solutions did not consist of the same molecules, so another experiment was proven to determine the conductivity of each of the solutions. A conductivity probe was used to measure the conductivity of each solution to see which one had the highest measurement. It was determined that Red #3 had the highest conductivity, concluding it to be the strongest ionic compound out of the three red solutions. The third experiment used a laser beam to shine through each solution to see if it contained nanoparticles. The laser beam came out as a horizontal line for Red #2 and Red #3, ultimately causing them to be ionic compounds if the color changed when potassium iodide was added. Adding KI to each solution allowed us to observe any color changes that occurred. Red solution #2 and #3 both changed color when KI was added, just as predicted. All of these techniques and goals were used to propose an identity of each of the red solutions. Red solution #1 is anticipated to be Kool-Aid or pink lemonade due to the sweet smell and the fact that it is a molecular compound. Red solution #2 is predicted to be hydrogen sulfate for the reason that it is an ionic compound. Lastly, red solution #3 is expected to be perchloric acid because it is one of the strongest acids. Along with undertaking these future experiments, another experiment involving the absorbance could have also taken place but we are unsure of the concentration so applying a Beer’s Law plot was not applicable to this proposal.