2. Purpose- Will different compounds form solutions in water? Independent variable- Type of compound Dependent variable- Ability to dissolve in water Copper sulfate Zinc oxide sulfurSodium chloride Sucrose 44444

3. Procedures 1.Measure 20 ml of water. 2.Place a small amount (tip of lab scoop) of each compound in a separate test tube. 3.Add the water to the test tube and record observations. 4.Mix the test tube 5 times and record observations.

4. CompoundObservationsDissolved Copper Sulfate Before: Crystals are staying at the bottom After: Dissolved 1. yes 2. Yes 3. Yes 4. Yes Zinc Oxide Before: Cloudy; White After: Cloudy; Opaque; White 1. Yes 2. No 3. No 4. No Sulfur Before: Floating on sides, top, bottom After: Stayed the same 1. No 2. No 3. No 4. No Sodium Chloride Before: Transparent, particles spread out After: Transparent, dissolved 1. Yes 2. Yes 3. Yes 4. Yes Sucrose Before: Transparent, particles at bottom After: Same 1. Yes 2. Yes 3. Yes 4.Yes

5. Conclusion In this lab, the copper sulfate, sodium chloride, and sucrose all formed solutions in water. Sulfur and zinc oxide did not form solutions. The results from each group were very consistent and were all pretty much the same. We know the first three chemicals were solutions because when they were added to the water, they were uniform and transparent. The zinic oxide was opaque or not see through, and the sulfer was clumpy so we knew they coulld not be solutions. Our hypothesis that all of the chemicals would be solutions except copper sulfate was not supported. Since the chemicals formed solutions were transparent, they were see through. They were also uniform, or the same through out. Observing the characteristics of the chemicals help us to determine whether it was a solution or not. We used solvents and solutes to find the solutions the solvent was the water and the solutes were the different substances being added to the solvent.

6. Temperature & Solution Lab Purpose: What happens to the temperature when a solute is dissolved in a solvent. IV: Amount of sodium chloride DV: Temperature of solution 0g1g2g3g4g5g 4 trials 44444

7. Procedures Measure 50 (ml) of water, pour in cup. Record starting temperature Measure 1 (g) of sodium or calcium chloride. Record the temperature after 1 min. Calculate the change in temperature. Repeat the steps using 2 (g) 3 (g) 4 (g) 5 (g)

8. TABLES

9. Conclusion When we mixed the water and the sodium chloride together, the temperature decreased and when we added calcium chloride to the water, the temperature increased. As we added more sodium chloride to the water, the result of the decreasing temperature did not change by much. The results for the calcium chloride also did not change by a lot. The temperature of the water depended on the amount of solute we added. We added 1 gram of sodium chloride every minute up to 5 grams and then we took a new cup of water and added.2 grams every minute up to 1 gram. Our hypothesis that sodium chloride would increase the temperature and calcium chloride would decrease the temperature was not supported. Instead, it was the opposite, with the sodium chloride decreasing the temperature and the calcium chloride increasing the temperature. The sodium chloride decreased the temperature because the salt and water break away from each other and combine. Since the sodium chloride is endothermic, it absorbed the heat, lowering the temperature of the solution. The calcium chloride went through the same process, but it is exothermic so it released the heat, increasing the temperature. As we added the salt to the water, chemical bonds were broken and they were formed.