Forming an Ionic Chrystal Procedure: 1. In groups, obtain the following ilems: safety glasses/goggles, graduated cylinder, triple beam baiance, 250mL beaker, 37%HCl, and NaOH. 2. Wearing safety glasses, measure 4.7gNaOH using the triple beam balance. Place the 4.7gNaOH into the 250mL beaker. 3. Next, under the fume hood, measure 10mL of 37%HCl using the graduated cylinder. Keep this under the fame hood. 4. Again, under the fume hood, slonly pour the 10mL37%HCl into the beaker containing the 4.7gNaOH. After the chemical reaction slows down carefully swill the beaker to completely mix the HCl and NaOH together. Write down all of your observations from this step. 5. Place the beaker containing tho HCl and tho NaOH onto the hot plate under the fume hood to allow the water to evaporate from the mi iture. 6. Once all the water has evaporated, we tongs to remove the beaker from the hot plate. BE CAREFULL. AS THE BEAKER WILL BE VERY HOT. Set it aside and allow it to cool. 7. Once the beaker has cooled, scrape some of the white residue from the bottom of the beaker and view the residue under the microscope using low and high power. Draw what you see under the microscope and show the sketch as part of yeur tab report. Discussion: HCl+NaOHNaCl+H2O The above chemical equation shows what happened during the chenical reaction you just perfonned. We say that one molecule of HCl ieacted with ene molecule of NaOH to produce one molecule of NaCl and one molecule of H2O. Or course there were many molecules of each but the basic combination is cutliped by the chemical equation above. Because you evaporated off the water, only salt (NaCl) was len behind. This is the ionic erystal you observed under the microscope. Answer Questions: a) Explain how you could tell a chemical reaction occurred during step 14. b) Explain how you determined a crystal was produced. c) Tell the type of chemical reaction that was performed and the salt produced