Soda Ash Lab Report

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.

1.5mL of phosphoric acid including 3-4 boiling chips were also added to the 25mL flask. The short path distillation apparatus was set up as shown in Figure 1. A heating mantle was used to heat up the 25mL flask. The solution was distilled to the receiving flask until a small amount of liquid remained in the initial RBF flask. At this point the presence of thick grey smoke pulling over into the entire apparatus was observed. The apparatus was then left to cool down. Through the use of pasture pipette, the aqueous layer from the distilled solution was drawn out. Sodium carbonate was then added to the remaining organic solution in order to check the pH and to verify the basicity of the solution. The aqueous layer was again drawn out from the solution. Next, 0.5g of sodium sulfate was added to the remaining organic layer and was swirled until the liquid appeared to be dry and clear. The alkenes were transferred into a clean 10mL flaks using another clean pasture pipe. The apparatus from the first distillation was rinsed off with

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:

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.

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

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

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.

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 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.

The purpose of this experiment is to show how an acid (Coke) can react together with potassium to create a charger for an iPhone. Potassium and acid formed together makes bubbles. With both potassium and acid working together, they will give off energy to the iPhone. Why Coke? Every liquid will be either acidic or basic traits. An acid-base reaction is a chemical reaction that happens between an acid and a base. There are multiple definitions when considering the reaction mechanism when solving problems. Regardless of what the problem is, it’s always a known fact that when using liquid or gaseous reactions, they become less apparent. You want to use Coke because its pH is the acidity of the substance. For an acidity to be

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.

Overall, the data I collected while doing the experiment proves that my hypothesis was correct, in stating that the more baking soda we add, the colder the temperature gets because of the chemical reaction between the two materials. This is shown multiple times, for an example, in our experiment we adding the baking soda to the vinegar, and as the vinegar disperse into the chemical reaction, and the gas form took place. Another example that our hypothesis was correct is we didn’t change any materials but the amount of baking soda and the baking soda in self-caused the temperature to decrease. These pieces of evidence prove my hypothesis is correct, is because in the chemical reaction, where we only changed our independent variable,

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

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.

The research work is on determination of optimum dosage of soda ash or lime in treating underground water in Makurdi metropolis. In the course of carrying out the work, samples of borehole and well water from five different locations of the study area (Makurdi) were obtained and analyzed in Benue State water works. The sample were analyzed to ascertain the level of hardness in samples and to determine the optimum values of soda ash (Na2CO3) and lime (Ca(OH)2) that will be used in reducing hardness and treating the sample in the study area. The locations were, North Bank, Wurukum, Wadata, High Level and Kanshio. The hardness level in the study area was found to range from 200mg/L to 80mg/L averagely; this was found to lay outside the WHO (1993) drinking water standards of 75mg/L to 100mg/L. On analysis, the hardness was found to range from 76mg/L to 100mg/L (borehole) at optimal level. Which was found to range within the WHO (1993) drinking water standard. While for well, range from 20mg/L to 80mg/L at optimal level. Which was