Nahco3

The experiment is to observe a variety of chemical reactions and to identify patterns in

In this experiment, we learned about stoichiometry, empirical formula, molecular formula, polyprotic acids and bases, metathesis reactions, and moles.

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.

Throughout the course of the experiment, the weight of the beaker and liquid, the weight of the Alka-Seltzer tablet, the weight of the beaker with liquid plus the weight of the tablet, and the weight of the beaker with all of the contents after the bubbling ceased remained roughly constant and did not vary widely. However, a trend is able to be seen in Figure 1. It is clear that as the mL of vinegar used in each experiment run increased, the mass percent of NaHCO3 increased as well. During the construction of Figure 1, experiment runs four and six were deleted to create the expected graph which consists of a gradual increase and eventually leveling off into a plateau.

After the amount of carbon dioxide lost was found, stoichiometry lets the loss of carbon dioxide to help find the amount of sodium bicarbonate reacted. Moreover, the mass of sodium bicarbonate and the mass of the original tablet help calculate the percent by mass of sodium bicarbonate. An observation made is that the changing amounts in each trial according to Table 1.1 show that, with changing amounts of starting material, the mass of carbon dioxide and the mass of sodium bicarbonate are inevitably affected. However, looking closely at Figure 1.1, the amounts of vinegar added increased in the experiment consequently making it the excess reactant to the sodium bicarbonate causing the graph in Figure 1.1 to level out. The tables should then show a steady increase in the percent by mass in the tablet and the amount of carbon dioxide

In conclusion, the more baking that was added in the reaction the more gas that was produced. When there was only one scoop of baking soda, the least amount of gas was produced, when three scoops of baking soda were used, the most amount of gas was produced. The number of bubbles roughly stayed the same, so the number of bubbles created was not affected by the amount of baking soda. With increments of 1 scoop of baking soda, small amounts of gas are produced each trial. We compared each trial by identifying the firmness of the bag due to the gas. Since gas takes up space of the bag, the more firm the bag is, the more gas is produced. Therefore, our hypothesis of having more baking soda will make more gas is correct.

The purpose of this lab is to become more familiar with the products of different types of chemical reactions by conducting several chemical reactions and observing the changes that occurred. In addition, by performing various experiments, the observations will help in writing chemical equations, which represent the process involved in a chemical reaction. Overall, the chemical changes observed throughout can determine the products that are formed from the reactants. In chemical reactions, substances that are referred to as reactants produce other substances called products. There are several ways to determine that a chemical reaction has occurred, and which type of reaction has taken place, exothermic or endothermic, which will help predict

Then with a pipet, place slowly with hydrochloric acid, 10 ml, into the sodium hydrogen carbonate until the bubbles stop. Then with the product, heat until it seems as if all the water in the dish is evaporated. Originally the product was supposed to be 2.09g of hydrochloric acid, however there was a miscalculation of the mass of the sodium hydrogen carbonate, and that mass turned out to be 3.07g. The final mass for the product was supposed to be 2.14g as a mass of the product. After all the procedures were completed, the mass that was received from the lab calculations was 2.45g. This was a 114.55 percent error to the lab. The large error could have lead to many different things. One of the things that the error could have been caused was miss calculating the mass. While measuring the sodium hydrogen carbonate, the mass of the evaporating dish mass, 46.50g, had altered when it was zeroed and put the 3.00g of the sodium hydrogen carbonate. Then it was massed again together and it was 49.57g. Another possible way that the mass was altered the way it was, it that all the water wasn’t evaporated. There was also a little splatter outside the dish. That helped lessening the mass that was already too big. Finally an important error that happened was not letting the evaporating dish cool after it was heated. Those are some ways that the lab error could

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

This experiment is an experiment because of the reactants, and it is has to do with a process called

Our failure was induced by ignorance and failure to apply and incorporate the law of conservation of mass as we were performing our first lab. On our second attempt, we incorporated the “closed system”. Similar to our first attempt, we individually measured the mass of each material while ensuring that the weighing scale was precisely put on zero each time it was measured. Then, we combined the Vinegar and baking soda in a plastic bag while tightly securing the plastic bag with a twist tie.

This paper is about chemical reactions and chemical reaction types. All the data gathered was from conducting multiple experiments. Each experiment was performed carefully and analyzed to obtain the necessary information for the paper. That information included the four signs of a chemical change, the rnx type, and more.

Vinegar was used in this experiment to mimic the stomach acid that reacts with the sodium bicarbonate in the Alka-Seltzer tablet. Limiting reactants relate to this lab by the sodium bicarbonate reacting with the stomach acid. Once the stomach acid, vinegar in this lab, was reacted, the sodium bicarbonate no longer was secreted. Increasing amounts of vinegar was added to the tablet to determine a point at which the sodium bicarbonate becomes the limiting

In this lab, a 95.43% yield resulted from the chemical reaction between a base and an acid. Sodium bicarbonate, a base, and sodium chloride, an acid, are a 1:1 mole proportion. The balancing coefficients in the reaction indicate that there is a 1:1 mole ratio between reactant sodium bicarbonate and product sodium chloride. This means that for every 1 mole of sodium bicarbonate that reacts, 1 mole of sodium chloride should be produced. A chemical reaction occurred when hydrochloric acid was added to sodium bicarbonate because there was a formation of bubbles.

The purpose of this experiment was to determine what happens to baking Soda when it is heated. It was hypothesized that the baking soda would bubble and turn into a gas. It is concluded that the data partially supports the hypothesis. The baking soda did not bubble, but it did create some form of gas. A test tube was placed in a position where a rubber tube connected the test tube to a soda bottle. In part 1 of this experiment as the water exited the bottle, some form of gas replaced the missing water. Towards the middle of this experiment condensation appeared in the test tube and the baking soda formed a clump like structure unlike its original form. At the end of this experiment the bottle squashed and was estimated to have loss 14% of its