Ionic Reaction Lab Report
CHEM111AC, Experiment#9 - Ionic Reactions
Discussion/Error Analysis In the first part of this experiment, the student was presented with 7 unique and unidentified bottles of solutions labeled A-G and was expected to be able to analyze the 7 solutions through trial and error and mixing them with one another.
For solution A: mixing A + B formed a precipitate, A + C generated heat, A + D gave no reaction, A + E gave no reaction, A + F gave no reaction, A + G formed a precipitate.
For solution B: mixing B + C, B + D, B + E and B + F formed precipitates, and mixing
B + G gave no reaction. For solution C: mixing C + D led to the formation of gas, C + E gave no reaction, C + F led to the formation of heat and C + G gave no reaction. For solution …show more content…
It was suspected that E + F would form lithium phosphate, which forms a precipitate extremely slowly, and needs to be heated to react faster. As expected, heating the mixture of E + F did indeed reveal the formation of a precipitate, confirming the student’s initial suspicions. This accounts for one of the two possible major errors that the student could have made in this part of the experiment, the other one being accidentally mixing up two solutions up due to carelessness. Smaller errors include not watching the reaction long enough or carefully enough to see that it could be an entirely different …show more content…
One student in particular, given the table that the professor had given them as a guideline, decided that he would first mix the given mixtures with potassium sulfate, potassium carbonate and potassium phosphate in that exact order while centrifuging the formed solutions in between mixing. If the mixture, when reacted with potassium sulfate, forms a precipitate, it would be confirmed to have strontium ions, which were just separated from the mixture after centrifugation. The ions formed are certainly strontium ions due to the fact that among the 4 given cations present in the mixture that strontium is the only one that would form a precipitate when mixed with potassium sulfate. Likewise, if the mixture forms a precipitate when mixed with potassium carbonate, it would be confirmed to have magnesium ions, and if the mixture forms a precipitate when mixed with potassium phosphate, it would be confirmed to contain lithium cations. To confirm the presence of the sodium cation, which never forms a precipitate, a flame test is utilized to confirm its presence. Sodium’s flame color, which is yellow-orange, is unique to sodium, and is its single most distinguishable trait, at least in this experiment in particular, when compared to the other three cations. There can be as little as 0% error in this part of
Discussion/Error Analysis In the first part of this experiment, the student was presented with 7 unique and unidentified bottles of solutions labeled A-G and was expected to be able to analyze the 7 solutions through trial and error and mixing them with one another.
For solution A: mixing A + B formed a precipitate, A + C generated heat, A + D gave no reaction, A + E gave no reaction, A + F gave no reaction, A + G formed a precipitate.
For solution B: mixing B + C, B + D, B + E and B + F formed precipitates, and mixing
B + G gave no reaction. For solution C: mixing C + D led to the formation of gas, C + E gave no reaction, C + F led to the formation of heat and C + G gave no reaction. For solution …show more content…
It was suspected that E + F would form lithium phosphate, which forms a precipitate extremely slowly, and needs to be heated to react faster. As expected, heating the mixture of E + F did indeed reveal the formation of a precipitate, confirming the student’s initial suspicions. This accounts for one of the two possible major errors that the student could have made in this part of the experiment, the other one being accidentally mixing up two solutions up due to carelessness. Smaller errors include not watching the reaction long enough or carefully enough to see that it could be an entirely different …show more content…
One student in particular, given the table that the professor had given them as a guideline, decided that he would first mix the given mixtures with potassium sulfate, potassium carbonate and potassium phosphate in that exact order while centrifuging the formed solutions in between mixing. If the mixture, when reacted with potassium sulfate, forms a precipitate, it would be confirmed to have strontium ions, which were just separated from the mixture after centrifugation. The ions formed are certainly strontium ions due to the fact that among the 4 given cations present in the mixture that strontium is the only one that would form a precipitate when mixed with potassium sulfate. Likewise, if the mixture forms a precipitate when mixed with potassium carbonate, it would be confirmed to have magnesium ions, and if the mixture forms a precipitate when mixed with potassium phosphate, it would be confirmed to contain lithium cations. To confirm the presence of the sodium cation, which never forms a precipitate, a flame test is utilized to confirm its presence. Sodium’s flame color, which is yellow-orange, is unique to sodium, and is its single most distinguishable trait, at least in this experiment in particular, when compared to the other three cations. There can be as little as 0% error in this part of