60 Ml Of Soda Lab Report

Students will place a potato cube into a test tube and add 3 ml of H202 into each tube. Then students will wait one minute and record the height in cm of the bubbles and rate how rapidly the solution bubbles on a scale of 0-5. (0=no reaction, 1=slow,……. 5= very fast.)

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:

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 research question for the Alka Seltzer Lab is, “What is the effect of different surface areas of an Alka Seltzer tablets reaction time?’. Inside of an Alka Seltzer tablet there are two key ingredients; which are citric acid and baking soda. When a tablet is dropped into a liquid, the acid and baking soda show a physical reaction of fizzing and eventually dissolving. Materials needed for this lab was goggles, aprons, beakers, water of the same temperature, mortar pestle, and three alka seltzer tablets. In each beaker there was 150 mL of water. The first tablet was a full tablet, the second was broken into quarters, and the last tablet was crushed in a mortar pestle. The dependent variable of the lab was the rate of reaction, and the independent

The mass of the CO2 in the Alka-Seltzer tablet could be found by subtracting the mass of the solution after the bubbles escaped from the cup form the mass of the all substance before the reaction. In each trial the amount of Acetic Acid (vinegar) was increased by 5 mL while still maintaining 35 mL of solution. Theoretical,the mass of the CO2 initially increases with the amount of vinegar used and then reaches a steady value at trial 5. This is because when the volume of vinegar exceeds 20 mL, sodium bicarbonate, which produces the CO2, became the limiting reactant and the same amount of CO2 is produced each time.

Alka Seltzer is a medical drug used for pain relief and used for relieving indigestion. For example, if you have a stomachache or some indigestion problems, Alka Seltzer may help neutralize the stomach acidity. Not only that, Alka Seltzer is also used for cleaning household items, such as vases or jewelry. Alka Seltzer contains citric acid and sodium bicarbonate, which makes it dissolve and release carbon dioxide gas when dropped in water. In this experiment, my lab partner, Rebecca, and I are trying to find a way to make Alka Seltzer dissolve faster in water. Rebecca and I both decide that if we increase the temperature of the water or make the water hotter, then the Alka Seltzer will dissolve faster because I know when salt and sugar dissolve in hot water, they dissolve faster. I predict that this same result would apply to this experiment.

The cup with the second greatest change in mass of the rock was number 2. Cup 2 had the solution of 10% vinegar and resulted in the change of -0.3g. Lastly, Cup 3 with distilled water had the lowest change in the mass of the rock, of 0g. It was hypothesized at the beginning that Cup 3 with distilled water would have the least amount of change, if any. This hypothesis was correct. Water is not acidic, so there would be no reason for the rock to change. When the hypothesis was conducted, it was based on the pH level. Instead, the actual solution should have been taken into consideration. The fact that the soda water would eventually lose its carbonation and become flat within a few days. Therefore, taking the acidity away. The experiment was done correctly, and there did not need to be any changes. Just the hypothesis could have been more thoroughly

The liquid (vinegar) and solid (baking soda) formed into a gas. A: Chemical reaction procedure 2: The evidence that a chemical reaction was occurring was there was a bit of fizzing with the bubbles. The liquid and solid formed into a gas which also inflated the balloon and you cannot reverse that. 3. Q: How did the final mass of the system compare with the initial mass of the system for each procedure?

The hypothesis stated the higher temperature the water is, the faster the sugar cube will dissolve. The reference tables and graph show that the warmer the water is, the faster the sugar cube will dissolve. The reference tables and graph also show that the colder the water is the bigger the difference between the rates of dissolving are. For example the sugar dissolving in the 5.0 (℃) water took almost 8 minutes longer to dissolve compared to the sugar in the 88 (℃) water. The warmer the water became, the smaller the difference between the rates of dissolving were. Figure 1 shows the average dissolving rate at different temps.

The soda ash form experiment 3 was obtained. A 250 ml beaker was obtained and rinsed.

This experiment was started by having one regular sized tub, filled up with water. Next a 100mL graduated cylinder was filled up to the top with the water that was inside the tub. The top of the cylinder was held shut with one hand while carefully at the same time the graduated cylinder was inverted, facing upside down in the water tub. This was done, so that the water that was captured didn’t leak out into the tub. One group member held the inverted cylinder inside the tub the whole time so that it wouldn’t tip over.

The materials we used for this experiment were two aluminum soda cans, water, ice, a graduated cylinder, a metal saucepan, a hot plate, and a

Dilute 2.7 mL 37% aqueous formalin solution to 1 L with distilled, deionized water. This solution is stable for at least three months. Standardize by placing 5.0 mL of freshly prepared 1.13 M sodium sulfite solution in a 50-mL beaker and stir magnetically. Adjust pH to between 8.5 and 10 with base or acid. Record the pH. Add 10.0 mL formaldehyde stock solution. The pH should now be greater than11. Titrate the solution back to its original pH with 0.02 N sulfuric acid (1 mL acid = 0.600 mg HCHO; about 17 mL acid needed). If the endpoint pH is overrun, back-titrate to the endpoint with 0.01N sodium hydroxide. Calculate the concentration, C s (mg/mL), of the formaldehyde stock solution:

The goal of this lab was to determine the effects of different amounts of Vinegar on the temperature in the reaction NaHCO3 + HC2H3O2 → NaC2H3O2 + H2O + CO2.

Eight Styrofoam ball calorimeters were calibrated. Five milliliters of 1M hydrochloric acid (HCl) was reacted with 10 ml of 1M sodium hydroxide (NaOH) in each calorimeter. The temperature before and after the reaction were recorded; the change in temperature (∆T) was calculated by subtracting the initial temperature from the final temperature. The reaction was performed twice for every calorimeter.