Laboratory Report December 6‚ 2010 Title: Combining Vinegar and Baking Soda Statement of Problem: We wanted to observe what kind of reaction would take place when combining white vinegar and sodium bicarbonate (baking soda). Equipment or Apparatus: Sodium Bicarbonate (baking soda)‚ white vinegar‚ 13 oz. vessel‚ cork‚ household measuring devices (for lack of a scale) such as glass measuring cup and metal measuring spoons‚ and safety goggles. Procedure: We selected a vessel and a cork
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soda? The proper chemical name for sodium bicarbonate or baking soda is sodium hydrogen carbonate.{Source 1} What does baking powder contain? It is made from an alkali‚ bicarbonate of soda‚ and an acid‚ cream of tartar‚ plus a filler like corn flour or rice flour which absorbs moisture. {Source 2} How
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the plant.  The CO2 levels: Increased CO2 levels also increase the rate of photosynthesis. The variable I am going to investigate is the level of CO2‚ however‚ the addition of NaHCO3 (sodium bicarbonate) to the water may affect the osmotic ability of the water. Just 2g of sodium bicarbonate in 1000ml of water gives the equivalent salinity of seawater‚ and as Elodea is a fresh water plant‚ it cannot survive in salt water. I will need to take this into account when measuring the NaHCO3
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phenolphthalein HCI and phenolphthalein NaOH and AgNO3 AgNO3 and NH3 NH3 and CuSO4 Data Tables: Data Table 1: ReactionsReaction Question/WellNumberA/H12 Chemicals NaHCO3 and HCI - CO2 When I added the hydrochloric acid to the sodium bicarbonate it began to bubble and fizz almostimmediately. This solution continued to bubble forseveral minutes. There was no color change and I didnot detect any noticeable odors.When I added the BTB to the hydrochloric acid itturned a yellow-orange
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In the experiment‚ we tested a sodium chloride solution. Along with the tested solution‚ control groups (water and sodium phosphate) were used to be help understand whether or not NaCl was a buffer. Water was the negative control group and sodium phosphate was the positive control group. If NaCl was a buffer than the pH would be stabled as the sodium phosphate buffer. If NaCl was not a buffer than the pH would fluctuate like the negative control‚ water. During the first trial and prior to the drops
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Observations of Chemical Changes Date: 02/11/015 Pre Lab Questions: Use what you learned in this lab to answer the following questions. A. Suppose a household product label says it contains sodium hydrogen carbonate (sodium bicarbonate). How would you test this material for the presence of sodium bicarbonate? I would add hydrochloric acid (HCl) with carbon dioxide with NaHCO3‚ and it should bubble and form gas. B. You know what color phenolphthalein and bromothymol blue turn when testing
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(acetylsalicylic acid)‚ citric acid‚ and sodium bicarbonate (NaHCO3). As soon as the tablet dissolves in water‚ the NaHCO3 dissociates to form a bicarbonate ion (HCO3-) and a sodium ion (Na+) 1. NaHCO3(s) Na+(aq) + HCO3-(aq) Acetic acid‚ which will ‘donate’ H+ to water to create H3O+(aq) is then added to the mixture. With the addition of acetic acid the following acid-base reaction then takes place: 2. HCO3-(aq) + H3O+(aq) 2H2O(l) + CO2 (g) (The sodium ion does not take part in
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acid molecules. Further‚ more molecules can bind to the remaining free substituents on these molecules to create a macromolecule‚ or polymer. The polymer is formed as a by-product. Acetylsalicylic acid will react with sodium bicarbonate to form a water-soluble sodium salt‚ whereas the polymer remains insoluble. This difference can be used to purify the aspirin product. The most likely impurity in the final product is salicylic acid‚ which can be either unconsumed reactant‚ or the result
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Experiment 5B: Ketone Reduction Objective: Using sodium borohydride as a reducing agent‚ the ketone 4-tert-butylcyclohexane is reduced to its corresponding alcohol. It is purified through extraction techniques to give the cis and trans diasteromer products. Procedure: The procedure was followed as outlined in Mayo’s book for Experiment 5B with the following modifications: 1. Reagents and Equipment – The reaction will be on a scale of 2X what is described in the text. 2. Reagents and Equipment
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put the ester in a clean test tube. Materials Citric acid‚ 20 mL Cornstarch‚ 20 mL Sodium bicarbonate‚ 65 mL Ester (fragrance)‚ several drops Vegetable oil‚ 30 mL 400 mL beaker Stirring rod 250 mL beaker 250 mL graduated cylinder Procedure – Making the bath bomb 1. In the large beaker‚ 20 mL of citric acid was mixed together with 20 mL of cornstarch‚ and 65 mL of sodium hydrogen carbonate. 2. In the small beaker‚ 30 mL of vegetable oil and a few drops of the
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