6.03 Calorimetry Lab

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For Part A of the experiment, acetic acid was titrated with NaOH. First, the 0.05M acetic acid solution was prepared. A 50-milliliter graduated cylinder was obtained and used to add 45 milliliters of deionized water was added to a labeled 150-milliliter beaker. A ten-milliliter graduated cylinder was used to add five milliliters of acetic acid to the beaker and the solution was placed on the stir plate and stirred with a magnetic stir bar. Next, a 0.05M NaOH solution was prepared. A 50-milliliter graduated cylinder was obtained and used to add 90 milliliters of deionized water to a labelled 250-milliliter beaker and the solution was placed on the stir plate and stirred with a magnetic stir bar. After the solutions were prepared, the LabQuest was prepared for data collection. …show more content…
Before the titration began, the burette was conditioned. Ten milliliters of deionized water were added to the burette (with the stopcock closed) and the burette was inverted several times. The water was drained and the process was repeated a second time. Next, the burette was conditioned twice with five to ten-milliliter portions of 0.05M NaOH using the process described above. Next, the burette was attached to the ring stand with the burette clamp. A plastic funnel was used to fill the burette to the zero-milliliter mark with the 0.05M NaOH solution and the initial volume was recorded. A stir bar and 50 milliliters of deionized water were added to a 250-milliliter beaker. A ten-milliliter volumetric pipette was used to transfer ten milliliters of the 0.05M acetic acid solution to the

6.03 Calorimetry Lab

Calculate the mass of potassium nitrate and the mass of water in each solution Calculate the ratio of the mass of potassium nitrate to the mass of water for each solution. Multiply the mass ratio by 100 to determine the concentration of each saturated solution in grams of potassium nitrate per 100 grams of water. Plot a graph of solubility of potassium nitrate (in g of solute/100 g of water) on the y-axis versus temperature on the x-axis. Scale each axis as necessary. Draw a smooth…

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6.03 Calorimetry Lab

The average enthalpy of neutralization for HNO3 and NaOH is -55.95 kJ/mol H2O. Post Lab Questions: 1. The temperature change of water will increase because the heat in hot water will transfer to cold water in the calorimeter. 2. Part A.5. His decision will decrease the specific heat of the unknown metal. The highest measured temperature…

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6.03 Calorimetry Lab

In a chemical reaction, matter is neither created nor destroyed. This is the law of conservation of mass, which begs the question, does this linearity also apply to volume? One of the goals of this experiment was to see if two pure liquid substances are together, will the volume of the solution be the total sum of each individual substance? Three characteristics must be known about the solution: the mass, volume, and density. Mass can be accurately measured out by a digital scale, volume can be measured…

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6.03 Calorimetry Lab

Get a piece of copper wire, proceed to clean it with steel wool and clean it until the surface is shiny. Using the electronic balance given, mass the copper wire and record it in the data table. Put the copper into a 150 mL beaker. When placed in the beaker, the Copper needs to be smashed down flat. Place the beaker with the Copper in it, in the fume hood. Proceed to carefully add 12 mL of concentrated Nitric acid ( HNO3 ) into the beaker. Let all the copper dissolve, slowly add 100 mL of distilled…

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6.03 Calorimetry Lab

For the first reaction, which is NaOH(s) → NaOH(aq), I would first need to measure out the required .041 moles of NaOH, which would weigh 1.65 grams. I would then measure out 41 milliliters, so that when I mixed the two, my concentration of NaOH in my aqueous solution will be 1M. In all, this should weigh about 41.8 grams when mixed together; however, prior to pouring the NaOH, I will first need to measure the temperature of the water itself with the calorimeter; I will do this at least five times…

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6.03 Calorimetry Lab

sulfate(II) sulfate and adding iron sulfate and copper will be used in a single replacement action. Also it should be able to find the ratio of moles of a reactant to moles of a product in the chemical reaction. Thus, it should answer another purpose for the lab which is to find is to be able to relate this ratio to the coefficients of these substances in the balanced equation for the reaction. Hypothesis: Both of coefficient off iron Variables: Procedure Find the mass of a clean, dry 100 ml beaker. Record…

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6.03 Calorimetry Lab

Before beginning this experiment make sure to write down observations of all the chemicals that are going to be used. To begin, 25 mL of .05 M lead nitrate into a clean 50 mL graduated cylinder and add to a clean Erlenmeyer flask. Measure out 1.4 mL of .025 M sodium carbonate and also add it to the Erlenmeyer flask. After adding mix both chemicals for 15 seconds or so. After mixing set up vacuum filtration flask using deionized water. In order for the apparatus to work it needs to be set up correctly…

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6.03 Calorimetry Lab

This is because copper cations (Cu2+) in copper(II) gluconate produce a green flame. The cation is the part of the compound responsible for color. You know that the copper ions is responsible for color because for example in lab when we measured K+ which was actually KCl, it was found that KCl produces a purple flame. K+ was the part of the compound that is responsible for color thus it would also make sense that Potassium gluconate produces a light purple flame because it…

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