Rate of reaction between Hydrochloric Acid and Calcium Carbonate

In Experiment B the limiting reactant was determined to be CaCl2 when two drops of the test reagent 0.5 M CaCl2 was added to the supernatant liquid in test tube 1, and a precipitate formed. Since there was a reaction, there was C2O42- in excess and Ca2+ is the limiting reactant in the original salt mixture present in test tube 1 . This was further confirmed when two drops of the test reagent .05M K2C2O4 was added to the supernatant liquid in test tube 2. There was no precipitate because Ca2+ was not present since it was the limiting reactant and instead C2O42- was in excess.

In this experiment, you have been asked by your teacher, to investigate the design of a small-scale airbag system they want to produce as a child safety device to put into baby strollers. Because of sodium azide’s toxicity (which is used in many vehicular airbags), it is suggested you use the reaction of NaHCO₃ (sodium bicarbonate or baking soda) with an aqueous solution of HCL (stomach acid) to produce CO₂ gas to test your engineering design. The reaction of hydrochloric acid and sodium bicarbonate is: HCL + NaHCO₃, one mole of CO₂ gas is produced. Regarding the other products, NaCl dissolves in the water to create a salt solution which occupies only a small portion of the volume inside the bag.

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:

* By using the dropper and measuring cylinder, 7 ml sodium carbonate solution was added to the test tube

The purpose of this experiment was to mix Alka-Seltzer with Hydrochloric acid in order to analyze Sodium Bicarbonate as an active ingredient in the Alka-Seltzer. The mixture will contain hydrochloric acid to only see the composition of Sodium Bicarbonate in the tablet once it reacts. The amount that reacted allowed us to determine how much of it is present in the tablet. The amount of sodium bicarbonate will be measure by using the ideal gas law PV=nRT. The experiment will be conducted in the lab, therefore we are going to use room temperature which ranges from 15 to 26 degrees celsius. At room temperature pressure ranges from 12.8 to 25.0 millimeters mercury according to its corresponding room temperature.In the ideal gas equation R is 0.08206latm/mol k which is a constant. Once we have those values we can calculates the number of moles that reacted in the mixture by solving for the missing value. With the number of moles we are able to find the mass in grams which is what will potentially tell us the composition of Sodium Bicarbonate in a tablet of Alka-Seltzer.

The limiting reactant lab was performed in order to determine the ratio of two reactants that will yield the maximum amount of product. By keeping the amount of vinegar at 40 mL, 630 mL CO2, the maximum amount that was actually produced, were obtained when 3.008 g of baking soda were added. The amount of baking soda added to the vinegar to obtain the most efficient reaction theoretically should have been 2.81 g, but the experimental result of 3.008 g was the closest value obtained that was higher than the theoretical amount. After adding more than 3.008 g of baking soda, the amount of CO2 released should have been close to 630 mL, but at 5.004 g and 7.021 g the amounts were not close to the range due to errors. One of the potential errors

Stoichiometry and Determining the Limiting Reagent Abstract: Four chemical reactions will be done using different ratios of mixture between calcium chloride and sodium carbonate. The mixture of these two substances produces the precipitate calcium carbonate, which will be separated using filtration. After observing the tubes and collecting data, the limiting reagents were deduced from observing which amount of substance had the least amount of moles. It was found that in trials one through three, the limiting reagent was calcium chloride and in trial four, the limiting reagent was sodium carbonate.

Bubbles slowly started to form as the acid was poured into the test tube. At 6:30 minutes the bubbles start to rise to the top. At 11 minutes the bubbles started to slow down until only a few bubbles are rising to the top. At 20 minutes the bubbles almost stop rising to the top for the rest of the time

The experiment was a success because all of the ultimate goals were completed. The volume of CO2 released from the pop rock reaction was calculated and found at 58 mL. The moles of CO2 was calculated at .00233 mol. The experiment was also a success because it was found that the heat released from combining and eating pop rocks with soda would not kill the consumer unless it was consumed in very high doses. The combination is not dangerous because it doesn't release a large amount of heat. The simulation of stomach acid, pop rocks, and soda reviled that the temperature increase during the reaction is minimal. Some possible errors of this experiment was missing some of the CO2 when the tube escapes the graduated cylinder. To avoid this in the future the tube could be held during the apparatus processes. Another possible error is miscalculation of LD50. In the future calculations could be done more precisely and

An unknown sample was massed and put into three test tubes for three different trials. A gas transfer assembly was put together and hydrochloric acid was added to each sample in each test tube. A reaction between the carbonate sample and the acid occurred and the volume of carbon dioxide gas produced was recorded. This process was repeated three times. The mass

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Experiment to investigate factors affecting the rate of reaction between magnesium ribbon and hydrochloric acid