Formation of a Salt Lab Essay Example
Title: Formation of a Salt
Objective: Students will observe the reaction of NaHCO3 and HCl.
Students will draw the Lewis Electron Dot Diagrams of Na+ and Cl-.
Students will site examples of how to identify an ionic compound.
Materials: Materials include 6M of HCl and NaHCO3 , a 100 milliliter (mL) beaker, a 10 mL graduated cylinder, a dropper, phenol red indicator, distilled water, a hot plate, a balance, a magnifying glass, and beaker tongs.
Procedure: First, measure the mass of a 100 mL beaker. Then, add 0.5 grams of NaHCO3 and 15 mL of distilled water to the beaker. Once the NaHCO3 is dissolved, add about 2 to 3 drops of phenol red indicator. While swirling the beaker, add drops of HCl, until the solution turns yellow. Next, heat the beaker on the hot plate, until the water evaporates. Then, allow the beaker to cool, and mass the beaker and the crystals. Observe the contents of the beaker, record the data, and clean up.
Data: The mass of the empty beaker is 69.24 grams. The mass of the beaker and the NaHCO3 is 70.19 grams. The mass of the NaHCO3 is 0.95 grams. The mass of the NaCl is 0.04 grams.
Observations: When the phenol red indicator was added, the color of the solution changed from clear to a pinkish color. When the beaker was heated, the solution began to bubble, then the color changed to orange, then back to the original pinkish color. Eventually the solution began steaming, and the water started to evaporate. After the solution was finished heating, the contents of the beaker turned to a solid crystal. There were some pink remains on the walls of the beaker. Analysis and Conclusion: 1.) As you added the hydrochloric acid, what did you observe? The solution bubbled and turned yellow. 2.) What gas was released during the chemical reaction? CO2 was released. 3.) The NaHCO3 underwent a chemical change. What evidence do you have of this change? The solution bubbled and had a change in heat. 1.) Write the electron
Objective: Students will observe the reaction of NaHCO3 and HCl.
Students will draw the Lewis Electron Dot Diagrams of Na+ and Cl-.
Students will site examples of how to identify an ionic compound.
Materials: Materials include 6M of HCl and NaHCO3 , a 100 milliliter (mL) beaker, a 10 mL graduated cylinder, a dropper, phenol red indicator, distilled water, a hot plate, a balance, a magnifying glass, and beaker tongs.
Procedure: First, measure the mass of a 100 mL beaker. Then, add 0.5 grams of NaHCO3 and 15 mL of distilled water to the beaker. Once the NaHCO3 is dissolved, add about 2 to 3 drops of phenol red indicator. While swirling the beaker, add drops of HCl, until the solution turns yellow. Next, heat the beaker on the hot plate, until the water evaporates. Then, allow the beaker to cool, and mass the beaker and the crystals. Observe the contents of the beaker, record the data, and clean up.
Data: The mass of the empty beaker is 69.24 grams. The mass of the beaker and the NaHCO3 is 70.19 grams. The mass of the NaHCO3 is 0.95 grams. The mass of the NaCl is 0.04 grams.
Observations: When the phenol red indicator was added, the color of the solution changed from clear to a pinkish color. When the beaker was heated, the solution began to bubble, then the color changed to orange, then back to the original pinkish color. Eventually the solution began steaming, and the water started to evaporate. After the solution was finished heating, the contents of the beaker turned to a solid crystal. There were some pink remains on the walls of the beaker. Analysis and Conclusion: 1.) As you added the hydrochloric acid, what did you observe? The solution bubbled and turned yellow. 2.) What gas was released during the chemical reaction? CO2 was released. 3.) The NaHCO3 underwent a chemical change. What evidence do you have of this change? The solution bubbled and had a change in heat. 1.) Write the electron