Name: 6.03: Calorimetry Data and Observations: Part I: Insert a complete data table, including appropriate significant figures and units, in the space below. Also include any observations that you made over the course of part I. (4 points) I observed that when the metal is placed inside the calorimeter, it transfers heat to the water making the water increase temperature while the metal will decrease temperature. I also noticed that the system was the metal and the surroundings is the water, this is because the water is taking in the heat from the metal making the water warm. Metal Name Mass of Metal Volume of water Initial temp.
After that, dissolve the sample in 2 mL of deionized water and shake the test tube for 1 to 1 ½ minutes to dissolve the solid. Place another dry test tube in a 50mL beaker and weigh it. Find a bottle of barium iodide and record the name and molar mass. Then, weight out either anhydrous barium iodide or barium iodide dehydrate into this test tube and dissolve is it in 2 mL of deionized water. Pour the contents of one of the test tubes into the other and a reaction should occur and you should see a white precipitate of barium sulfate form.
The following data were obtained when a sample of barium chloride hydrate was analyzed as described in the Procedure section. Calculate (a) the mass of the hydrate, (b) the mass of water lost during heating, and (c) the percent water in the hydrate. Mass of empty test tube 18.42 g Mass of test tube and hydrate (before heating) 20.75 g Mass of test tube and anhydrous salt (after heating) 20.41 g. Mass of the Hydrate is 2.33g. Loss (H2O) is 0.34g. Percent H2O in Hydrate is equal 0.34/2.33=14.6% 3.
The chemical equation to be used is : 2NaHCO3(s) Na2CO3(s) + CO2(g) + H2O(g) In the second part, 1.0 M HCl will be titrated into a solution with a known amount of sodium carbonate (Na2CO3), the pH will be measured as it becomes more acidic and the equivalence point (the point at which HCL and Na2CO3 reach equilibrium) determined. We will calculate the moles of Na2CO3 by dividing the grams used by the molar mass of sodium carbonate. Then, the moles of HCl required to neutralize Na2CO3 will be determined by using the mole to mole ratio in the chemical equation. Finally, the molarity
Record your hypothesis on page 123. -My hypothesis is we can determine the different between each chemical reaction by the temperature change.To descide which one is exothermic and endothermic. 4. Summarize the procedures you will follow to test your hypothesis. -We measured in each chemical and added water besides, HCl we added NaOH.
BE READY WITH THE STOPWATCH. Record the time in the data table. Room Temperature Water: Fill beaker with 80mL of water. Use thermometer to record the temperature Drop Alka-Seltzer tablet in water. Measure the time it takes to completely dissolve.
In another flask 50-mL of ice water was deposited with three-drop phenolphthalein. Using a volumetric pipet 50-mL of the 1-bromopropane was added into the empty flask in the bath. By the same method 50-mL of potassium hydroxide was delivered to the same flask while swirling the contents and remaining in the water bath. A 10-mL aliquot was immediately removed from the mixture and added to the ice water containing the phenolphthalein. When the pipet was half emptied into the ice water a timer was started.
To the second, add 10% NaOH dropwise until the pH is 14. (To do this, add a couple of drops of NaOH to the tube; stir thoroughly with a stirring rod; then touch the stirring rod to a piece of pH paper to check your pH.) To the third, add 0.5% sodium bicarbonate solution to pH 9, and to the fourth, add 2% HCl to pH 2. Record your observations on the data sheet. Repeat the above tests using 2% casein solution.
Part C: Density of Sodium Chloride (NaCl) Solution, a sample of NaCl was obtained and measured using a 100mL beaker and a 10mL pipet to determine the concentration of the solution. In order to obtain the appropriate result, a calibration graph and density measurement was used to determine the concentration of the sodium chloride solution. In conclusion, based on the water temperature of 21.8°C in part A’s graduated cylinder experiment obtained, it was determined that the average density was .0973g/mL with a percentage error of 2.5%. When graphed the measurement was equal to Y=0.988x. Part B: The graduated pipet’s average density at 22.3 °C was determined to be 0.9785g/mL with a percentage error of 1.89% shows the graduated pipet to be more accurate and precise.
Lab 2 Measurements: Accuracy and Precision A. Data Tables (36 points) Place your completed data tables into your report here: Data Table 1 Measurement | Data | Length of aluminum plastic packet | 4.50cm | Height of aluminum plastic packet | 7.50 cm | Temperature of faucet water | 26.0 degrees Celsius | Temperature of ice water | 10.0 degrees Celsius | Volume of water in 10-mL graduated cylinder | 10.0ml | Volume of water in 50-mL graduated cylinder | 9.0ml | Data Table 2 Measurement | Data | Inside diameter of 50-mL graduated cylinder | 2.50 cm | Height of 50-mL graduated cylinder | 10.0 cm | Water temperature | 25.0 degrees Celsius | Initial volume of water in 50-mL graduated cylinder | 10.0 mL | Mass of water in the 50-mL graduated cylinder (remember, 1 g of water weights 1 mL since its density is 1 g/mL) | 10.0gm | Volume of water and aluminum shot in 50-mL graduated cylinder | 18.0ml | Mass of aluminum shot (given on outside of packet) | 20.0gm | B. Follow-Up Questions (Show all calculations) Part I (Each question is worth 10 points.) 1. Convert the length and height measurements for the packet that contains the aluminum shot from units of cm to units of mm using the unit-factor method.