# 6.03 Calorimetry Lab Report Chemistry

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In order to safely dispose of a solution with a pH of 12, the solution needs to be diluted with an acid to neutralize the basic solution. The pH range should be between 5 to 8 to be ready for disposal.
2. A graduated cylinder, Erlenmeyer flask, and beaker were used to measure a 60-mL volume. Which of these devices seems to be the most accurate for measuring a 60-mL volume? Be sure to explain what the term ‘accurate’ means. How did you determine this during lab? State some reasons why this device might be most accurate compared to the others.
The graduate cylinder seemed to be the most accurate for measuring a 6-mL volume, as one is able to approximately reach the true value better than using an Erlenmeyer flask or beaker. When looking
While he wanted to achieve a solution of 400 mL, he ended up with a solution of 420 mL because he did not take into account the volume that the solute (sucrose) would take up within the solution. This additional volume would thus also change the concentration; however, even if the actual concentration amounted to 400 mL, he would still have not obtained the 4M he assumed he was creating. This may be due to guessing, but he may have also assumed that by adding 400 mL of water, that would make the solution 4 M, regardless of the amount of solute he added into the mixture (If he wanted a 3M solution, he may have thought he could add 300 mL of deionized water). Because of his error, he ended up with a solution with a much smaller concentration. Therefore, when the student wants to create a solution of certain concentration, he needs to know either how much solution or solute he wants and then calculate for the other component in order to achieve the desired concentration.

4. Define the term pH. What is the H+ concentration of a solution with a pH of 1? What is the H+ concentration of a solution with a pH of 10? Of these two solutions, which of these solutions is more acidic? What is the difference in acidity between the two solutions? pH is defined as the negative log of the hydronium concentration (often stated as the concentration of hydrogen): pH=-log⁡([〖H_3 O〗^+ ]) or pH=-log⁡([H^+
This can be due to the creation of too much acid, buildup of acid, or lack of base in the blood to balance the acid in the system. There are several causes/types of metabolic acidosis. The first one is diabetic ketoacidosis, which is brought on by long periods of hyperglycemia, or high blood glucose. The body doesn’t have enough insulin to allow the cells to use the glucose in the blood to create energy, and thus turns to burning fat, which has a byproduct of ketones, which are acidic. If the process continues for a long period of time, it can throw off the pH of the blood and cause the blood to become very acidic (O’keefe). Another cause of metabolic acidosis is lactic acid buildup due to anaerobic respiration. Dysfunctional kidneys can also cause metabolic acidosis as they are unable to filter out acid from the blood when fluids are excreted. Lastly hyperchloremic acidosis can also cause high levels of acid in the blood as problems within the body cause a lack of bicarbonate production. Bicarbonate therapy may be used to treat metabolic acidosis because bicarbonate can serve as a buffer in the blood system. Bicarbonate is an anion in solution and has the ability to pick up a hydrogen cation or act as a proton acceptor. This thus prevents dramatic rates of pH change in the blood as well as can lower the pH of the solution (“Metabolic

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