Experiment 2: In-Lab Data CollectionName Partner(s) ONYEN Experiment 2: Aqueous Reactions Experiment 2: In-Lab Data Collection Record your general measurements, recorded data and observations directly into this section during the lab. Data can be transcribed directly into the tables provided below. Add titles and captions to all tables and figures for full credit. Remove and replace any highlighted text. • Present your data in the tables below. • Summarize your observations during the progress of the experiment. Observations should not include numbers (measurements). • Always fill in units in tables - in parentheses below. To avoid confusion, do not add units to numbers,but instead to data headers or labels (such as what was done in the Excel tutorial) • Add observations between data tables to log what you see during the experiment (1-2 sentences is usually sufficient for any major steps - i.e. the volume increased noticeably when...) • Be sure to download and save the Vernier data as a .csv so it can be used to generate Excel data in the post-lab. A. HEAT OF SOLUTION DATA COLLECTION Observations -distilled water is clear before adding in the salt -Bubbles forming in the center where the spinning pill is -Salt appears to be completely dissolved after adding it to distilled water -No color changes throughout the mix -For Sodium Carbonate, there were lesser bubbles Table 1. Recorded & calculated mass and mole of NH4Cl and Na2CO3 Ammonium Chloride Sodium Carbonate Mass (grams) 1.010 1.000 Moles (moles) 0.01888 0.009435 1CHEM 101L In-Lab 2 Fall 2021 The initial temperature of the distilled water is 22.6 C. Immideately after adding the solute, the temperature dropped to 21.1 C. Because there was a decrease in temperature of the distilled water, the reactionis endothermic, as the heat from the water enters the reaction. The initial temperature is 22.4 C, and when we added the solute/Na2CO3, the temperature increased to a maximum of 24.1 C. The increase in temperature started at the 13.5 seconds mark and increased until the 85.5 second mark.There is an increase in temperature, so the reaction is exothermic. 2CHEM 101L In-Lab 2 Fall 2021 B. HEAT OF REACTION: SODIUM BICARBONATE WITH CITRIC ACID Observations -The citric acid without the sodium bicarbonate solute looks like an off white color -right after adding in the solute, the solution started to fizzle like soda -couldn't see color change due to the foam/bubbles -After the bubbles died down, no clear color change, but sizzling sound can still be heard with small bubbles -Reminded us of carbonated water Table 2. Calculated mass and mole of NaHCO3 with written molecular equation of NaHCO3 and C6H8O7 Equations 3NaHCO3 (aq) + H3C6H8O7 (aq) → Na3C6H8O7 (aq) + 3CO2 (g) + 3H2O (l) 3HCO3 -(aq) + H3C6H8O7 (aq) --> C6H8O7 3-(aq) + CO2(g) + H2O(l) Mass (grams) 3.52 Moles (moles) 0.0419 The initial temperature is 21.3 C. Before adding in the solute, the solvent increased temperature alittle, going to 21.9 C at 53 seconds. When the solute was added, it decreased, with the steepest slope between the 90.5 second mark (16.2 C) and 53 second mark (21.9 C).The slope then leveled out, and reached a constant of 14.2 at the end. The reaction is endothermic, taking heat from the solvent. HEAT OF REACTION: HYDROCHLORIC ACID AND MAGNESIUM 3CHEM 101L In-Lab 2 Fall 2021 Observations -before adding Mg(s), HCl looks clear, after Mg(s) added, Mg swirled around in shape of the stirring vortex; changes on the Mg(s) could not be seen as it was moving too fast; no clear bubbles were createdin the solvent like the last solution -after turning off the stir, dissolvation of Mg metal can be seen. Tiny bubbles were escaping out of the metal piece in a straight vertical line to the top. No visible bubbles were formed at the surface of the solvent, however. The Mg metal was also still as the stir was turned off Table 3. Calculated mass and mole of Mg(s) with written molecular equation of Mg and HCl Equations Mg(s) + 2HCl (aq) →MgCl2 (aq) + H2 (g) Mg(s) + 2H +(aq) --> Mg 2+(aq) + H2 (g) Mass (grams) 0.0230 Moles (mole) 9.46*10^-4 The initial temperature is 21.3 C. After the addition of the Mg(s) metal piece, the temperature slowly but constantly rose throughout the whole time. After turning the stir off, the temperature started to decrease, which was at the 368 second mark. The highest temperatureit rose to during the given time was 21.8 C. The reaction is exothermic, as there is an increase in temp of the solvent. Observations 4CHEM 101L In-Lab 2 Fall 2021 -The two out of the four solutions that had an increase in temperature for their solvent was Sodium Carbonate + distilled water and Magnesium ribbon + Hydrochloric acid -The only solution that had the biggest change in physical apperance that could be seen was Sodium Carbonate,as the addition of the solute created many fizzling bubbles TA ONLY (Grade last): Formatting Late Penalty