Ph Measurer Lab Report
Throughout the experiment, there were 3 significant error I made. Firstly, at first when I conduct my experiment, I measured 10g of ascorbic acid powder and mix it within 1 litre of water. I believed that by having the solution prepared before putting in the d-block elements would save time overall. Unfortunately, the data was all over the place, this is because the later I conduct the experiment, there is a higher chance of oxidation occur in the ascorbic acid solution as it have a direct contact with oxygen in the atmosphere. In order to keep constancy, I had to reduce the amount of ascorbic acid by ratio to 0.2g with 10ml of water. By measuring element for each trial, it is easier to control the rate of oxidation to have a data with higher precision.
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Secondly, when I measure the pH level of each solution, I did not calibrate the pH measurer every time after I use it.
The reason why I think this could be a limitation is because each solution has an extreme acidic pH level like 1 or 2. As a result, I speculate the supreme acidity of the solution could negatively affect the pH measurer that could make it lose the originality to measure the right pH level for later product. Hence, it is crucial to have the pH measurer calibrated in a buffer solution so that the measurement can have a high accuracy overall. Thirdly, when measuring the enthalpy change for the solution, it is suggested to measure the temperature of the ascorbic acid solution for 30 seconds before putting in the d-block element in order to have a plateau temperature of the original solution in order to compare with the product temperature later. In my experiment, I waited 30 seconds for the ascorbic acid power to dissolve in water, I should have measured the temperature then put in the element to have more data to support the enthalpy change
result.
On the other hand, there were 3 parts of the experiment which should be improved upon. Firstly, the result from measuring the product with pH and conclude from then leads to a great variation. This is because the pH level of element itself is very low, for example copper (II) chloride dihydrate has the pH level of 2. Therefore, the result pH of the product has the average of 1 or even lower. Hence, it comes to a conclusion that the pH of the reactant could have a significant effect towards the overall result. Therefore, it is suggested to consider the pH of the ascorbic acid with the reactant and take the average of the two in order to have a data with higher accuracy. Secondly, oxidation for ascorbic acid occurs when there is a change in temperature and contact of light. When I did my experiment, I planned to conduct trials by each element. As a result, the environmental error could lead to different oxidization rate. Therefore, it is suggested to conduct experiment by each trial, which is to finish all the first trial for different variables in order to minimize the error. Thirdly, as mentioned in conclusion, it is suggested to create extreme environmental condition as a catalyst for other d-block ions to oxidize than ascorbic acid. This is because element with low valence level like manganese, chromium are easy to be oxidized only at high temperature in order to transform into higher valence level. Hence, the experiment could further to be build to discover how extreme temperature could affect d-block ions to stabilize ascorbic acid.
Secondly, when I measure the pH level of each solution, I did not calibrate the pH measurer every time after I use it.
The reason why I think this could be a limitation is because each solution has an extreme acidic pH level like 1 or 2. As a result, I speculate the supreme acidity of the solution could negatively affect the pH measurer that could make it lose the originality to measure the right pH level for later product. Hence, it is crucial to have the pH measurer calibrated in a buffer solution so that the measurement can have a high accuracy overall. Thirdly, when measuring the enthalpy change for the solution, it is suggested to measure the temperature of the ascorbic acid solution for 30 seconds before putting in the d-block element in order to have a plateau temperature of the original solution in order to compare with the product temperature later. In my experiment, I waited 30 seconds for the ascorbic acid power to dissolve in water, I should have measured the temperature then put in the element to have more data to support the enthalpy change
result.
On the other hand, there were 3 parts of the experiment which should be improved upon. Firstly, the result from measuring the product with pH and conclude from then leads to a great variation. This is because the pH level of element itself is very low, for example copper (II) chloride dihydrate has the pH level of 2. Therefore, the result pH of the product has the average of 1 or even lower. Hence, it comes to a conclusion that the pH of the reactant could have a significant effect towards the overall result. Therefore, it is suggested to consider the pH of the ascorbic acid with the reactant and take the average of the two in order to have a data with higher accuracy. Secondly, oxidation for ascorbic acid occurs when there is a change in temperature and contact of light. When I did my experiment, I planned to conduct trials by each element. As a result, the environmental error could lead to different oxidization rate. Therefore, it is suggested to conduct experiment by each trial, which is to finish all the first trial for different variables in order to minimize the error. Thirdly, as mentioned in conclusion, it is suggested to create extreme environmental condition as a catalyst for other d-block ions to oxidize than ascorbic acid. This is because element with low valence level like manganese, chromium are easy to be oxidized only at high temperature in order to transform into higher valence level. Hence, the experiment could further to be build to discover how extreme temperature could affect d-block ions to stabilize ascorbic acid.