Soda Ash Lab Report

The solution of the formed ash and the water is basic, which was shown using the pH paper where its color became blue. A chemical change occurred. It is described using the following chemical reaction:

We were assigned mystery powder convertible which contained calcium carbonate, baking soda, and sucrose. We found out that the mystery powder had calcium carbonate because when it reacted with iodine it turned orange/brown. When calcium carbonate reacted with vinegar it had a fizzy-like reaction. It also reacted with hydrochloric acid and that caused it to bubble. When we tested the mystery powder it also turned orange/brown when we added iodine. Also when we added vinegar and it also fizzed like the calcium carbonate. Again when we added the hydrochloric acid it reacted exactly like calcium carbonate, lots of bubbles were made. We know that the calcium carbonate was in the mystery powder because it had similar reactions.

The pre-test helped us decide the exact details of our experiment. We started off with testing 25cm³ of 3-molar hydrochloric acid to 2g of calcium carbonate medium size chips (we decided a medium size chips before we started our pre-test as we had a choice of 3, small, medium, large). We saw that this reacted too quickly as we used 10 second intervals and we couldn't get 6 results this is because our burette could only hold 100cm³ of water, which would make our results reliable. We then decreased the amount of Calcium Carbonate to 1g and kept the same 25cm³ of 3 molar hydrochloric acid and 10 second intervals. We could get the right amount of results of this, so we then tested the other extreme - the lowest molarity.

The goal of this lab was to determine the amount of grams of sodium bicarbonate (NaHCO3) required to produce enough CO2 gas to completely fill the lab and also how many Alka-Seltzer tablets that would equate to. This was done by collecting CO2 gas by inverting a buret and submerging it under water in order to calculate the volume of CO2 released from a fragment of Alka-Seltzer tablet. The main component of Alka-Seltzer is sodium bicarbonate, used to neutralize excess stomach acid during illness through the following reaction that generates CO2:

In this experiment, the precision of percent by mass of sodium carbonate was decent. It seemed to be consistent, although we seemed to have an outlier in our fifth trial. I believe this was due to human error of adding too much vinegar to this graduated cylinder. The accuracy of our results was decent in comparison to the rest of the class’s data, but our results were on the higher end compared to the averages of the class data, though not too high to be considered

Measure 500ml of tap water in the 500cm3 beaker, then measure 5g of sodium hydrogen carbonate using the 50cm3 beaker and weight scale and place in the beaker of water, using the glass rod to dissolve it into the mixture.

2. In Part I of this experiment, acetic acid is titrated with NaOH. The net ionic equation for acetic acid reacting with NaOH is CH3COOH+ NaOH =NaC2H3O2+H2O. The equivalence point is when the moles of the titrant and other solution are equal.. You detect the equivalence point by obtaining the point on the graph where the steep pH occurs. In titrating acetic acid with NaOH, the pH is greater than 7 at the equivalence point because NaOH is a strong base so it results in a higher pH, due to the OH- ions in the solution.

From the results that were acquired from mixing the liquid reagents with each powder, it was determined that Unknown Mixture #1 consisted of baking soda and cornstarch. When individually testing the substances from Unknown Mixture #1 with the liquid reagents, a few noticeable reactions occurred. Mixing baking soda with vinegar caused bubbling to occur. This is because a neutralization reaction took place between the two reactants. In this reaction, sodium bicarbonate(baking soda) reacts with vinegar and produces sodium acetate, water, and carbon dioxide(HC2H3O2(aq) + NaHCO3(aq) NaC2H3O2(aq) + H2O(l) + CO2(g) ). The gaseous carbon dioxide most likely tried to escape into the atmosphere and caused the bubbling to occur. Another noticeable reaction

Procedure: In the first experiment (Synthesis Reaction) 5g of Mg was heated with a Bunson burner to perform a reaction. In the second experiment (Decomposition Reaction) 5g of Cu2Co3 was heated with a Bunson burner to perform a chemical reaction with visible physical properties. In experiment 3 (Single Displacement Reaction) 15 mL of 6 M hydrochloric acid (HCl) was put into a Erlenmeyer flask and was stopped with an airtight stopper to record the temperature and pressure when .25g of Zinc was added. In Experiment 4 (Double Displacement Reaction) two separate beakers were used. In the first one there was 15mL of NaOH and the second contained NiCl2. These were poured into each other to watch what reaction would take place.

The volume of carbon dioxide gas produced from a reaction was measured in order to determine what carbonate sample was used. A gas assembly apparatus was used to capture the gas from a reaction between an unknown carbonate and 6M hydrochloric acid; three trials were performed. The mass of the unknown carbonate was determined, and the reaction occurred in a test tube. The volume of gas produced by the reaction was measured, and the partial pressure of carbon dioxide was calculated after the partial pressure of water vapor was determined using Dalton’s Law of Partial Pressures. The percent mass of carbon dioxide gas was then calculated, and the average mass percent was compared to the table of known carbonates. It was concluded that the unknown carbonate sample used in the reaction was magnesium carbonate.

This lab included determining our PTC (a chemical substance causing bitter tastes) phenotype and genotypes through taste-tests and DNA-analysis. After performing my taste-test, I was unable to taste the bitterness of the PTC, so I concluded that no movement would take place in the gel electrophoresis wells.

Fly ash inspection included examination of the results of chemical tests with the X- ray fluorescence (XRF) method in order to find out the chemical and mineral composition of the fly ash. Moreover the particle size analysis (PSA) was used to determine the grain size of the fly ash, and X-ray diffraction (XRD) testing to determine the mineral elements and relative composition of the fly ash. The chemical composition of zone-0 and zone-4 fly ash are given in Table

In reaction eleven, 0.2 grams of solid sodium bicarbonate was placed in a 13 x 100 mm test tube. Using a beral-type pipet, one milliliter of the hydrochloric acid solution was added to the test tube and when the substance reacted, observations were made. Later, in a 13 x 100 mm test tube, one milliliter of sodium bicarbonate solution was mixed with one milliliter of the hydrochloric acid solution and the reaction between the two substances was studied and observed. Again, a 13 x 100 test tube was used and about one milliliter of the silver nitrate solution and one milliliter of the hydrochloric acid were mixed together to create a reaction. Observations were then made and written down.

Results and Discussion: The first process of the experiment was when 1.0545 grams of the pieces of aluminum cans were mixed with potassium hydroxide to form the products potassium aluminum sulfate and water. The equation shown below is the unbalanced version Al(s)+KOH(aq)+H2O(l)KAl(OH)4(aq)+H2(g) .The new balanced equation was 2Al(s)+2KOH(aq)+6H2O(l)2KAl(OH)4(aq)+3H2(g). The reaction shown above is a redox reaction due to the transfer of electrons from one element to another.The aluminum was oxidized from 0 to 3+ and the hydrogen in potassium hydroxide was reduced from 1+ to 0. As the reaction was being completed a gas was formed as well as a color change in the liquids used. In order to speed up the reaction a hot plate was used. All of this was done under a fume hood to make sure none of the gases formed was in the air. The next chemical process in the experiment was when the 20 mL of sulfuric acid was added to the solution. The balanced equation is 2KAl(OH)4(aq)+H2SO4(aq)2Al(OH)3(s)+K2SO4(aq)+2H2O(l) but the total ionic equation is what was used which was Al(OH)4-(aq)+H+(aq)Al(OH)3(s)+H2O(l). The reaction shown was an acid-base

The mass of the empty, capped plastic bottle was determined using the analytical balance. Afterwards, 25.00 mL of Light Coke® solution was measured in the burette by filling it completely (50.00 mL), then draining it carefully until 25.00 mL was left. This amount was added to the plastic bottle. The mass of the bottle was measured again and recorded. This procedure was repeated once more for Trial II by draining the remaining 25.00 mL of solution in the burette. The results of these trials are recorded in Table. 2 below.