Hydrochloric Acid And Double Displacement Reaction Lab Report

Four test tubes were filled with 9 mL of a solution of baker’s yeast. Of the four test tubes, one of them was placed in a beaker filled with water at room temperature, another in a beaker of water at 37 degrees Celsius, one at 65 degrees Celsius, and the last one was placed in a Styrofoam container with ice at 0 degrees Celsius. Once the test tubes reached their desired temperature, they were pulled out of their beakers. Four pieces of filter paper were cut and soaked in a hydrogen peroxide enzyme solution. Once soaked, each of the filter papers was dropped into the test tubes. When the papers reached the bottom of the tubes, they were placed back into the different temperature beakers. The clock was then started to see how long it would take for the filter paper to reach the surface of the tube. The reaction rate (dependent variable) was measured in seconds that it took for the filter paper to reach

Ultimately, the purpose of this experiment is to determine the unknown concentration of hydrochloric acid, by performing a series of titrations between sodium hydroxide and potassium phthalate in order to standardized the sodium hydroxide to be used to identify the concentration of the hydrochloric acid.During each of the titrations, sodium hydroxide (NaOH) was used to titrate potassium hydrogen phthalate (KHP); during each of the trials, sodium hydroxide was gradually added to the KHP from the burette to the beaker. After each addition of sodium hydroxide, the pH was recorded in order to form the titration curve, which can be seen in Graphs 1 and

This trend can be observed in the graph above. The lowest concentration of hydrochloric acid was 1 mole and produced an average temperature increase of 18.4°c. This value sat above the line of best fit and it can be concluded that this is due to the difference between the averages collected from the groups. There was a range of 4°c which was the greatest difference recorded. The next concentration tested was 1.5 moles, recording a temperature change of 23.8°c. The temperature change increased by 6.5°c as the concentration increased by 0.5 of a

Introduction: The rate expression for this reaction is of the form: rate = K(CV+)M(OH-)N Where k = re constant, m is the order of the reaction with respect to the concentration of CV+, and n is the order of the reaction with respect of OH-. In the experiment the concentration of OH- is purposely made 1000 times larger then Concentration of CV+. Thus, the concentration of OH- changes so little during the

To start off the experiment 25mL of water was placed into a labeled beaker and tested for the pH using pH test strips. Next the antacid tablet was placed in the solution and timed for how long it took to dissolve the tablet. Finally the temperature was measured. This same process was repeated for the acidic solution, and finally for the basic solution. After each experiment the pH, the reaction time, and the temperature of the beaker were recorded into a table. For this experiment the independent variable was the substance used (acid, neutral or base), and the dependent variable was the reaction time of each substance. The constant conditions of this experiment included the amount of substance being used, and the placing of one antacid tablet into each beaker. The experimental group was the acidic and basic solution, and the control group was the neutral

By adding acid to the baking soda, it caused the substance to form bubbles and release gas. More drops of HCl were added until the bubbling

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

In this experiment we tested the effects that enzymes and substrate have on chemical reaction rates, which is the rate at which chemical reactions occur.. This experiment tested how different concentrations of enzyme and substrate affected the light absorption measurements on a spectrophotometer. The experiment also tested how temperature affected the light absorption, and in a separate test, the effect of the enzyme inhibitor hydroxylamine was also tested. In the first test conducted, 3 different concentrations of enzyme, and three different concentrations of substrate were measured in a spectrophotometer. For the enzyme and the substrate, the measurements got higher as the concentrations were higher, but the over measurements of the substrate were smaller than those of the enzyme. In the second test conducted, the medium concentration enzyme was tested under the temperatures; 4°C, 23°C, 37°C, and 60°C. The measurements in this test got higher as the temperature got higher, but did the measurements under 4°C were overall significantly higher than the other temperature measurements. Lastly, the last test conducted showed that the measurements of the substance with 0 and 1 drop of hydroxylamine inhibitor went up, but the measurements of the enzyme with 5 drops of hydroxylamine inhibitor stayed rather low and did not change much. In conclusion, these experiments showed that chemical reaction rates are sped up with higher concentrations of enzyme, substrate,

ii. The second part of the titration series involves titration of NaOH with Hydrochloric acid (HCL). Again, three reps of titration and a blank titration have to be completed. A volumetric pipet is used to measure 10.00mL of HCL into three labeled conical flasks. Then the flasks are filled with deionized water until about the 50mL mark. A buret is

to compare the results, and neither solution was expected to produce an observable chemical reaction. The procedure was the same as used for the test with 6M HNO3 and 0.1M AgNO3 solution and the test with 6M HCl and 0.1M BaCl2 solution. A third experiment used was the flame test. First, a scoopula was used to place 0.1 grams of the unknown compound in a test tube, and a wash bottle was used to add approximately 2 mL of deionized water to create a solution.

The type of reaction that occurs through reaction A through E is a chemical reaction. InReaction A, a redox reaction (oxidation-reduction) occurred. Copper metal reacted withnitric acid to produce copper (II) nitrate. It also created nitrogen dioxide, and water (which isdecomposed from nitric acid). In reaction B, a double displacement reaction occurred forthe reasons that when copper (II) nitrate reacts with sodium hydroxide, copper and sodiumdisplace each other to create copper (II) hydroxide and sodium nitrate.

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.

One milliliter of 6.00-M phosphoric acid was placed into a 125-mL Erlenmeyer flask using a volumetric pipette. Using a slightly larger pipette, six milliliters of 3.00-M sodium hydroxide was transferred into a 50-mL beaker. Then a disposable pipette was used to slowly mix the sodium hydroxide into the phosphoric acid while the solution was swirled around. Then both the beaker and flask were rinsed with 2-mL of deionized water and set aside. A clean and dry evaporating dish was weighed with watch glass on a scale. Then the solution was poured into the dish and the watch glass was placed on top. The solution was then heated with a Bunsen burner to allow for the water to boil off to reveal a dry white solid. After the dish cooled to room temperature it was once again weighed and the new mass was recorded.

For Table 1 the difference between the reactants and the product was zero grams. One possible explanation as to why the mass stayed the same, was that there was a rubber stopper covering the top of the Erlenmeyer flask. This resulted in the mass to staying the same because it stopped the gas that was formed from

In this lab a acid-base indicator phenolphthalein was used to determine endpoint of a reaction HCl(aq) and KOH(aq). At the end point all of the HCl(aq) would have reacted with KOH(aq), and the pH becomes 7. The phenolphthalein would changed colours from colourless to pink indication when enough KOH(aq) was added. The purpose of numerous trials was to use the average volume of the 3 trials with similar measurements.