Chemical Reaction Lab

The purpose of this lab was to determine the limiting reactant in a mixture of to soluble salts and the percent composition of each substance in a salt mixture.

A chemical reaction is when substances (reactants) change into other substances (products). The five general types of chemical reactions are synthesis (also known as direct combination), decomposition, single replacement (also known as single displacement), double replacement (also known as double displacement), and combustion. In this lab, the five general types of chemical reactions were conducted and observations were taken before, during, and after the reaction. Then the reactants and observations were used to determine the products to form a balanced chemical equation. The purpose of this lab was to learn and answer the question: How can observations be used to determine the identity of substances produced in a chemical reaction?

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

When the volumes of NaOH and CH3COOH were equal, the temperature increased by 5 degrees celsius. When we performed a second trial and added 15 mL of NaOH and 5 mL of CH3COOH, the temperature only showed an increase

After the twenty minutes elapsed, the flask was cooled to room temperature and then titrated with the remaining NaOH until the colorless solution remained pink. The final volume was then recorded. While solution #1 was heating the same process was repeated with solution#2 and the second burette

Purpose: The purpose of this experiment is to observe a variety of chemical reactions and to identify patterns in the conversion of reactants into products.

In our experiment, you controlled one of the factors. Which one (temperature or NaCl concentration) was it? i controlled the NaCI concentration.

For our lab, we have six beakers of water. Three of the beakers contain high temperature water that range from 46 ℃ to 55 ℃, while the other three beakers contain room temperature water that range from 22 ℃ to 23 ℃. Then, we take six different colored Alka Seltzer tablets, and place them into the beakers one at a time. We record the length of time it takes for each Alka Seltzer to dissolve

Purpose: The purpose of this experiment was to observe the many physical and chemical properties of copper as it undergoes a series of chemical reactions. Throughout this process, one would also need to acknowledge that even though the law of conservation of matter/mass suggests that one should expect to recover the same amount of copper as one started with, inevitable sources of error alter the results and produce different outcomes. The possible sources of error that led to a gain or loss in copper are demonstrated in the calculation of percent yield (percent yield= (actual yield/theoretical yield) x 100.

The mean temperature of substance 2 for room temperature was 20°C. Substance 2 dissolved easily in the water. The mean temperature for substance 2 in colder water was 6.25°C, and most of the powder dissolved. However, some of it sank, leaving us to think both substance 1 and 2 were supersaturated in the cold water. The average temperature of substance 3 for room temperature was 23.5°C.

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.

Procedure: A beaker was filled up with water to about 90% of the beaker’s capacity was placed on a hot plate and was continuously heated throughout the entire experiment. 90 mL of potassium iodate and sodium bicarbonate were combined into a large beaker. The initial temperature of each solution was recorded.

Study the graph below: It shows the number of grams (g) of sodium nitrate (NaNO3) dissolved in 100 grams of water (H2O) at different Celsius temperatures (0 C).

The styrofoam cups were used to store the acid (cup was labeled A) and base (cup was labeled B) prepare for them to be mixed. A lid was put on cup A and then the temperature probe was inserted to begin to measure the temperature

3. Calculate the total heat released in each reaction, assuming that the specific heat of the solution is the same as for pure water (4.18J/gK). Use q=mcΔT. Show work here and record your answer in Data Table 2.