Baking Soda Lab Report

Sodium Bicarbonate (also known as baking soda) is something used everyday. Baking soda is a very common ingredient in cooking- one of its main uses is to make cakes "risk" due to the compounds produced. (Summer Chemistry Workshop). The lab was to use decomposition, the chemical change in which a single compound breaks down into two or more simpler products (Pearson Chemistry, 358), listed below are the possible reactions.

When given similar looking substances, they can be distinguished by their chemical reactions. Baking soda can be noticed when it is contained in acidic ingredients and starts to bubble. Its chemical formula is NaHCO3. Baking powder is a combination of baking soda, calcium acid phosphate (a weak acid), and cornstarch; used in bing to generate bubbles. Its chemical formula is NaHCO3. When baking soda is reacted with red cabbage indicator, a color change usually occurs from pink to green. The chemical equation between vinegar and baking soda is NaHCO3(s) + CH3COOH(l) → CO2(g) + H2O(l) + Na+(aq) + CH3COO-(aq).

After about an hour of reaction time, the mixture was isolated via vacuum filtration and was then acidified with 6 M HCl during the work up step. The reaction mixture was initially basic because of the sodium bicarbonate added during the beginning of the reaction. This was confirmed by a litmus paper test, with the reaction mixture spot showing up green which correlates to a pH of 8. However, the incorporation of HCl into the reaction mixture greatly acidified the solution. The litmus paper was spotted with the resulting reaction mixture and appeared red, which suggests a pH of about 2.

An example of synthesis is water. The equation for this is 2H2 + O2 ---> 2H2O.

This is done by adding sodium bicarbonate to the water, raising the total concentration of bicarbonate ions in the water as in the process

Then, place 5 drops of each aqueous solution into the right wells according to the table that is constructed for taking notes of observations. Mix in ten drops of each solution in a clean test tube, for the following aqueous combinations: barium nitrate Ba (NO3)2 (aq) and sodium hydroxide NaOH (aq), nitric acid HNO3 (aq) and sodium hydroxide NaOH (aq), and nitric acid HNO3 (aq) and sodium carbonate Na2CO3 (aq). Finally, record any observations of the reactions taken place in the test tubes. When completed, all of the contents in each of the test tube were discarded into the waste jar located in the fume hood. Test tubes were then washed with soap and rinsed with water and placed onto the test tube rack when

CO2 and H2O are two molecules present in all soda, CO2 is what gives pop that tingly flavor that makes it irresistible. However, there is one problem with this combination: CO2 is nonpolar while, H2O is polar, a conflicting pair, because of the rule that “like dissolves like;” nonpolar molecules and polar molecules do not mix. Manufacturers force CO2 and H2O into soda at high pressures–up to 1.200 points per square inch. CO2 is forced to be a liquid in the form of carbonic acid inside a can of soda (The Regents University of California). When you open the can, the sound you hear is CO2 gas escaping from the “watery prison” (Bryner).

For the points describing the results of 0g and 1g of sodium bicarbon, the points remained at 0. The points for 1g of sodium bicarbonate increased, and the slope of the trend line is 0.24x. This means 0.24 leaves floated per minute. Conclusion

Vinegar is a non-toxic chemical made from acetic acid, water, salt and other chemicals. Sodium Bicarbonate also known as baking soda is a salt composed of sodium ions and bicarbonate ions. Vinegar and sodium bicarbonate cannot be mixed with each other which causes a chemical reaction. There are two chemical reactions that take place in the whole process. Firstly, a double displacement reaction occurs where acetic acid in the vinegar reacts with the sodium bicarbonate to form sodium acetate and carbonic acid: NaHCO3 + HC2H3O2 → NaC2H3O2 + H2CO3.

This experiment will demonstrate a double-replacement action, as the two different compounds will trade elements to form two new compounds e.g NaHCO3 + HC2H3O2 → NaC2H3O2 + H2O + CO2. However, this experiment will also involve a neutralisation reaction, when the same amount of acid and base are combined together, as it will neutralize the compound and produce salt, water (see equation) and an extra product of carbon dioxide. According to the hypothesis, as the concentration/amount of acid increases, the rate of reaction will also increase this is because as the reactant particles in the compounds will get more crowded in the compound, leading to a greater chance of particles colliding, therefore this means there is a higher chance that the molecules will complete the reaction quicker, which means the rate of reaction would be faster. But, this reaction occurs baking soda (sodium bicarbonate) has a sodium atom, a hydrogen atom, an oxygen atom and a carbon trioxide molecule, whereas vinegar (acetic acid) contains a hydrogen atom and an acetate ion. And when these compounds are combined the hydrogen atom in the vinegar accumulate with the hydrogen and oxygen atoms in the baking soda to form water (H2O), but while the acetate ion in the vinegar takes the sodium atoms and forms salt/sodium acetate. And now the carbon dioxide molecule is not connected with other chemical bonds, therefore comes forth as a

The main purpose of this lab was to use stoichiometry to determine the yield of NaCl based on a given amount of reactants. Stoichiometry is a method used in chemistry which utilizes the amounts of reactants, products and the coefficients of the balanced chemical equation, to determine measurements such as the excess and limiting reactants. The chemical equation for this lab was NaHCO3(s) + HCl(ag) NaCl(s) + H2O(l) + CO2(g) and in the end of the lab the H2O and CO2 were evaporated. The chemical equation was used to predict the amount of NaCl that should be produced from the the combination of NaHCO3(s) and HCl(ag). We observed two different chemical changes when the solution became cold in the beaker of NaHCO3(s) and HCl(ag) and when the solution began to bubble due to the production of CO2 gas. The limiting reactant was NaHCO3(s) because a set amount was used and the excess reactant was HCl(ag) because we were able to add the necessary amount needed to completely consume the amount of NaHCO3(s). After the bubbling stopped, we added 5 drops of HCl(ag) to prove that the reaction between the HCl and NaHCO3(s) had

NaHCO3 and HCH3COO are reacting together to make CO2. How much baking soda, added to 10ml of vinegar, will cause a film canister rocket to shoot the farthest? I think 10 ml of baking soda will shoot the farthest because I think having the same amount of each will be the best. The independent variable is the amount of baking soda and the dependent variable is how far the lid shoots.

Additionally, if tap water were used in place of distilled water to dissolve the dried alkali metal carbonate, there would be an increase in the apparent molar mass. Tap water has other ions in it which would have reacted partially with the alkali metal carbonate, making it seems as though there was less alkali metal carbonate than there actually was. Again, this would decrease the moles of alkali metal carbonate and thus increase the molar mass (4). One precaution taken to get the most accurate measurements possible was heating the calcium carbonate for 15 minutes,

Next, spatula tips of sodium bicarbonate were added to the solution until CO2 was no longer being produced. This was observed by when the solution stopped bubbling after the addition of the sodium bicarbonate. Once the sodium bicarbonate was no longer reacting with the

The purpose of this lab was accomplished by following the procedure. Our first step was to use the beaker to find the mass of two grams of Calcium Chloride and two grams of Sodium Carboante. After finding the mass, we added 40 ml of distilled water and stir it until it starts dissolving the mixture. In the third step, we waited until the mixtures was completely dissolved and then we poured the Sodium Carbonate solution