p1g3+mp4

__Tanner, Nick, Chris, Liam, Dave __ = = = Chemical Reactions Lab =

__ Bakground Information: __

 * 1) ===Calcium Cloride(CaCl2): Used in pickle flavoring, used in electrolites, drying pipes, salting roads.===
 * 2) ===Sodium Bicarbinate(NaHCO3): Baking soda, sports supplement, toxic if to much consumed.===
 * 3) === Bromothymole Blue: Used as a weak acid in solutions, used in managing pH in pools and fish tanks. ===

=== __Summary:__ From doing the chemical mixing lab, w e found that when we added more chemicals to the mix they reacted faster. We also noticed that if Calcium Chloride or Sodium Bicarbonate was added it would usually bubble or fizz if water was added. From our temperature readings most of the reactions were endothermic because the temperature of the mixture was higher after the reaction had taken place.=== 2 || 22.3 ͦC || No temp change || 14.8 ͦC || 20.5 ͦC || 20.5 ͦC || 21.3 ͦC || === __Conclusion:__ When we did this lab we learned that when different chemicals are combined they can create different substances and be endothermic or exothermic. We found that two of the chemical we used, Calcium Chloride and Sodium Bicarbonate, were added, it would usually bubble or fizz. This happened every time we mixed chemicals. We also found that Bromethymal Blue would create a precipitate when it was mixed with both Calcium Chloride and Sodium Bicarbonate. We found that the reactions that occurred were always Exothermic and gave off energy. We also learned that when chemicals are mixed they can react and create new substances, like when Sodium Bicarbonate was mixed with water it created CO2.===
 * Combination || Prediction || Observation ||
 * CaCl₂+ H₂O || Absorbing || Fizzing/ dissolving
 * CaCl₂+ BB+ H₂O || Absorbing/ fizzing || Bubbled
 * CaCl₂+ NaHCO₃ || Nothing || Nothing
 * NaHCO₃+ H₂O || Fizzing || No color change
 * NaHCO₃+ BB+ H₂O || Change in color || No color change
 * NaHCO₃+ CaCl₂+ H₂O || Absorbing || Extreme bubbling opaque
 * NaHCO₃+ CaCl₂+ BB || Absorbing/ color change || Extreme bubbling yellow/ green

= The conservation of mass Lab =

Question: How does the mass of the reactants compare to the products in a chemical reaction when a precipitate is formed?
== Hypothesis: As a group, we hypothesized the mass of the reactants and the mass of the products will remain the same. The reason for this is the conservation of mass. This states that the mass of the reactants and the mass of the products will stay the same. ==

__Background Information:__

 * 1) === Lead Nitrate (PbN): This can cause lead poisoning if swallowed. This is toxic and is linked to lung,renal, and brain cancer. ===
 * 2) === Sodium Iodide (NaI): This is harmful if injestided. It is an iritant if exsposed to skin. ===

===__ Summary: __ We hypothesized that the mass would remain the same throughout, from the reactants to the products, because of the law of conservation of energy. Our hypothesis has shown to be correct, with a mass of 4.3 for both the reactants and the products. The reactant compounds of Sodium Iodide and Lead Nitrate created an opaque substance that turned yellow right on contact. The mass gained was .1, but was canceled out by other group’s -.1.===

__ Data (Results/Observations): __
===__ Observations: __ Once the Sodium Iodide and Lead Nitrate were combined a yellow precipitate formed immediately. After the mass was measured a one-tenth difference in the mass. This difference was cancelled out because, when looking at all the data, one group had a increase of one-tenth and we had a decrease of one-tenth. This cancelled out creating a change of zero, matching much of the other groups. In the end, when this solution was filtered, the filtrate was a clear liquid and the residue left in the filter was a bright yellow. This could be used in coloring paint, however, is not used today because lead is toxic.===
 * Lab Group ||  Mass of the Glassware  ||  Mass of the Reactants & Glassware  ||  Mass of the Reactants Alone  ||  Mass of the Products & Glassware  ||  Mass of Products Alone  ||  Change in Mass  ||
 * 1. ||  94.2  ||  99.2  ||  5.0  ||  99.1  ||  4.9  ||  -.1  ||
 * 2. ||  95.5  ||  99.5  ||  4.0  ||  99.5  ||  4.0  ||  0  ||
 * 3. ||  80.1  ||  84.4  ||  4.25  ||  84.5  ||  4.35  ||  +.1  ||
 * 4. ||  82.2  ||  86.4  ||  4.2  ||  86.4  ||  4.2  ||  0  ||
 * 5. ||  74.4  ||  79.0  ||  4.6  ||  79.0  ||  4.6  ||  0  ||
 * 6. ||  92.9  ||  96.9  ||  4.0  ||  96.7  ||  3.8  ||  -.2  ||
 * 7. ||  88.3  ||  92.0  ||  3.7  ||  92.0  ||  3.7  ||  0  ||

===__ Conclusion: __ We learned that when a chemical reaction takes place the mass will stay the same after the reaction because of the law of conservation of mass. The mass of the reactants stayed the same but some of the mass was a liquid and some of it was a precipitate. When we measured that mass it was the same so it shows that no mass was created or destroyed. This proved our hypothesis true because the mass stayed that same.===