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Experimental Section In the following two experiments, you are going to react variable amounts (volumes) of 1.0 M NaOH, with the corresponding amounts (volumes) of 1.0 M acid (as shown in each row of the table below) Example (NaOH and HCI): 1. Using a graduated cylinder, measure out 45.0 ml of 1.0 M HCl into the Styrofoam cup. 2. Using a thermometer, record the initial temperature. 3. Measure out 5.0 ml of 1.0 M NaOH, and add them to the HCl in the Styrofoam cup. 4. Stir the reactants together and monitor the temperature change. Record the final temperature 5. Repeat the above steps with the remaining volume combinations of HCl and NaOH Experiment I: Reaction of Sodium Hydroxide NaOH and Hydrochloric Acid HC. NaOH + HCl → NaCl + H20 (unbalanced) 1. Fill out the rest of the following table. (12 points) / Volume or Volume of 1.0 MHCI Moles HCI (ml) 1.0 M Non Moles Now Initial Temp. Final Temp. AT (°C) CC) (ml) 45.0 DOUS 5.0 0.009 22 23 40.0 0.04 10.0 ooo 22 25 3 350 0.85 150 OS 92 96 30.0 wolo 200 090 02. 27 Is 25.0 Jo.o 25 25.0 025 22 29 20.0 b. 20 30.0 020 22 21 5 15.0 cols 35.0 22 24 2 10.0 0.00 40.0 0.046 222 2.3 5.0 0.00 45.0 0.045 02 22 Lol 0.625 Show a sample of your calculations (2 points) 5. Select (highlight) the rows from the table that represent chemical reactions where HCI was the excess reactant. (2 points) 6. Draw a graph of the moles of NaOH (x-axis) against AT (y-axis), that would demonstrate your answers to question 2 (it has to be a manual graph on graph paper-attach it with your lab report) (2 points). 7. The corresponding number of moles of HCl at this point is (1 point).