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= __I Can Count to Potato!!! Lab Page__ = __The Chemical Reaction Lab__ __Lab Summary__ This is the Background Information on the Chemicals used in the Chemical Reactions experiment. Press the full screen button near the bottom for the best view.
 * In this lab, we mixed various chemicals together to see the different signs of a chemical reaction. Some of the different chemicals that we used were as follows: calcium chloride, sodium bicarbonate, bromothymal blue, and water. We mixed these chemicals together in 7 different ways, finding signs of chemical reactions of all kinds, including a solid precipitate, a change in color, and even gas evolution. In our experiment Calcium Carbonate was formed. Calcium Carbonate formed as a result of the reaction between the water and carbon dioxide formed. Sodium Chloride or salt was also formed in the reaction, and this is soluble in water. **

media type="custom" key="16980052" (After) || + Sodium Bicarbonate || Nothing will happen. || -Both white -Calcium Chloride: .1g -Sodium Bicarbonate:.4g -Solids -Powder || No reaction || + Calcium Chloride || The Bromothymol Blue will change color. || -Calcium Chloride: .8g - 15 mL of Bromothymol Blue - Bromothymol Blue: 20.4 degrees Celsius - Bromothymol Blue is a dark blue || -Bromothymol Blue changed into a greenish-yellow color -Temperature: 23.5 degrees Celsius -Exothermic change || + Sodium Bicarbonate || The Bromothymol Blue will change color. || - Sodium Bicarbonate: .9g - Bromothymol Blue: 15mL - Temperature: 20.9 degrees Celsius || - Temperature: 19.8 degrees Celsius - Suspension formed || + Water || The Sodium Bicarbonate will dissolve. || - Sodium Bicarbonate: .7g - Water: 15mL - Water temp: 20.2 degrees Celsius || - Temperature: 18.6 degrees Celsius - suspension formed - exothermic reaction || + Sodium Bicarbonate + Water || They will both dissolve into the water. || - Water temp: 20.8 degrees Celsius - Water: 15mL - Calcium Chloride: .1g - Sodium Bicarbonate: .4g || - Temp: 19.5 degrees Celsius - Fizzed -Bubbled up - Endothermic change -White || + Water || The Calcium Chloride will dissolve. || - Calcium Chloride: .3g - Water: 15mL - Temp: 18.8 degrees Celsius || - Temp: 21.5 degrees Celsius - Dissolved - Suspension || + Calcium Chloride + Bromothymol Blue || The Bromothymol Blue will change color. || - Temp: 20.4 degrees Celsius - Calcium Chloride: .8g - Sodium Bicarbonate: .7g - Bromothymol Blue: 15mL || - Temp: 21.6 degrees Celsius - Fizzed - Bubbles - Turned white ||
 * Combination || Prediction || Observations (Before) || Observations
 * Calcium Chloride
 * Bromothymol Blue
 * Bromothymol Blue
 * Sodium Bicarbonate
 * Calcium Chloride
 * Calcium Chloride
 * Sodium Bicarbonate



media type="youtube" key="OExoruUXNHw?version=3" height="360" width="640" When we mixed calcium chloride and sodium bicarbonate together dry, no reaction took place. But when we added water to that mixture, the calcium chloride dissolved with the sodium bicarbonate and a new unknown substance formed. Since bubbles were coming up from the water, this showed that there was gas evolution taking place. We found that most of these chemical reactions needed water to take place. When we mixed calcium chloride and bromothymal blue, the bromothymal blue changed to a yellowish green color. This indicated that the mix between calcium chloride and bromothymal blue is an acid. When we mixed bromothymal blue and sodium bicarbonate, the sodium bicarbonate formed a suspension and the temperature of the water dropped from 20.2 to 18.6 degrees, meaning that it was an endothermic reaction. When we mixed sodium bicarbonate and water, the sodium bicarbonate dissolves. We concluded many things from this experiment, such as that a lot of reactions need water to happen. Also, we learned some signs that a chemical reaction has taken place, such as a solid precipitate.

= Chemical Reaction Lab II =

__ Lab Summary and Procedure __ By Dana Getty

In this lab, we took two compounds, Pb(NO3), which is lead nitrate, and NaI, which is sodium iodide. Our materials included a beaker with two miniature test tubes, all sitting on a triple beam balance. Then, we had lab glasses that we wore to protect our eyes from the chemicals. We also had 5 other test tubes. 2 of those test tubes held the chemicals, lead nitrate and sodium iodide. 2 of the other test tubes had pipettes in them. The remaining test tube had a funnel in it and filter paper next to it. My hypothesis was that the mass of the reactants and the products are the same. Adam had the same hypothesis, but Sean thought that the mass would decrease. First we zeroed the balance, and then we measured the mass of the beaker and the two mini test tubes that were inside of it. Next, we took the lead nitrate and the sodium iodide and filled the mini test tubes inside of the beaker with the pipette. Then we measured the mass of the components without a reaction. Then we mixed the two chemicals and then a precipitate formed but the mass stays the same. This makes me conclude that even though a precipitate forms, there is no change in mass. media type="custom" key="16980194"

Chemical Equation: By Adam
Lead Nitrate Sodium Iodide Sodium Nitrate Lead Iodide Pb (NO3)2 + 2NaI yields 2NaNO3 + PbI 2

Lead Nitrate:

Sodium Iodide: Sodium Nitrate:

Lead Iodide:

in Mass ||
 * Lab Group || Mass of the Glassware || Mass of the Reactants and Glassware || Mass of the Reactants Alone || Mass of the Products and Glassware || Mass of the Products Alone || Change
 * 1 || 90.5 || 95.1 || 4.6 || 95.1 || 4.6 || 0 ||
 * 2 || 96.1 || 98.2 || 2.1 || 98.2 || 2.1 || 0 ||
 * 3 || 80.2 || 87.2 || 7 || 87.2 || 7 || 0 ||
 * 4 || 81.7 || 86.8 || 5.1 || 86.8 || 5.1 || 0 ||
 * 5 || 74.2 || 76.4 || 2.2 || 76.4 || 2.2 || 0 ||
 * 6 || 92.9 || 96.8 || 3.9 || 96.8 || 3.9 || 0 ||
 * 7 || 88.5 || 93.1 || 4.6 || 93.1 || 4.6 || 0 ||