Nahco3 Powder Experiment

An automatic pipet was used to measure 0.450 mL water and 0.165 mL acetic anhydride and was added to the conical vial. A spin vane was placed into the vial and an air condenser was attached.

mL cylinder to the beaker on the stir plate and empty it into the beaker. Place the pH probe in the beaker and record the pH in the data table. Drag the beaker to the red disposal bucket. Double-click the bottle of NaHCO3 to move it to the Stockroom counter. Repeat steps 5 and 6 for KNO3.

The mass of the small beaker/flask and solution for each trial was found and recorded by using 50 mL graduated cylinders to add increasing 5 mL increments of vinegar, from 0 to 35 mL, and decreasing 5 mL increments of water, from 35 to 0 mL to the eight small beakers or flasks and weighed on an analytical balance. Accordingly, the mass of each of the eight Alka-Seltzer Tablets was determined and recorded. Moreover, the tablets were each dropped in their respective beakers/flasks, and allowed to fizz, without spilling over. The loss of mass of CO2 was furthermore ascertained by finding change in mass of each of the solutions after the fizzing stopped from the value of the mass of the Alka-Seltzer tablet plus the mass of the solution and beaker/flask. Further, using the loss of mass of CO2 for each trial and the balanced equation, the amount of NaHCO3 reacted and percent by mass in the tablet were identified. After determining the class average and the standard deviation for each trial, and plugging it into a scatter plot, the change of slope showed the true percent by mass of NaHCO3 in Alka-Seltzer tablets.

First, a 100 mL graduated cylinder was obtained and filled with 35 mL of water. A pipet was used to attain a more accurate amount of liquid. The water was then poured into a beaker, which was weighed on an analytical balance. Next, an Alka-Seltzer tablet was obtained and the weight measured using the same balance the weight of the beaker was measured on. When both masses were recorded, the tablet was dropped into the water. The liquid was swirled to allow for the tablet to dissolve completely. After the fizzing had stopped, the beaker was once again weighed and the mass was recorded. Each step was repeated seven more times for a total of eight trials. However, with each trial the liquids added to the beaker changed. In each new trial, an additional 5 mL of vinegar was added and 5 mL of water was taken away. Thus, beaker one had 0 mL of vinegar and 35 mL of water; beaker 2 had 5 mL of vinegar and 30 mL of water; beaker 3 had 10 mL of vinegar and 25 mL

The smaller the pieces of a solid is, the quicker the reactant react. It is normal that a powdered solid will develop a faster reaction than the mass being the same amount but is presented as a large chunk. The solid that was in a powder form has a greater surface than the solid that was presented as a large chunk. An example of this theory is with the powder reacting to gas, it would be easier for the gas to penetrate its way through the little particles of the powder. If the object was in a chunk, it would take a really long time for gas to penetrate through the object or it may not even penetrate it. As predicted, the powdered solution dissolved faster than the rest as there was less surface area for it to react on. Having a small surface

A 100 ml beaker is placed on cross mark drawn on a white cardboard. 6. 25 ml of sodium thiosulfate solution and 20 ml of distilled water is measured using measuring cylinder and poured into the beaker. 7. 5 ml of hydrochloric acid is added to the beaker and the stopwatch is started immediately.

The solution with the unknown concentration but known volume (vinegar) is called an analyte and a solution with a known concentration (sodium hydroxide) is called the titrant. In titration, the titrant is added to the analyte to achieve the equivalence point and determine the concentration of the analyte. In this experiment, the ethanoic acid was combined with sodium hydroxide to produce a neutralisation reaction. This can be seen in equation 2.

The accompanying materials utilized as a part of these experiments were a 50 mL container, a hot plate, a plastic funnel, aspirator, rubber tubing, a ring stand, a clasp, an iron ring, measuring boat, magnetic stir bar, a 10 mL graduated barrel, few expendable pipettes, a filter flask, a Buchner pipe, filter paper, refined water, a mixing pole, lastly litmus paper. Six chemicals were utilized as a part of the investigations are copper (wire), 6M HNO3, 6M NaOH, 3M H2SO4, Zinc, and 6M HCl. Toward the start of the lab, the 50 mL was connected to the ring stand on top of the hot plate. The iron ring was incorporated into the lab, so it can keep the measuring glass enduring set up. Soon after, a fume hood was amassed utilizing a pipe, elastic tubing, and the suction apparatus. The tube was appended to the ring stand on top of the measuring

· Measure out 10ml of acid and add it to the conical flask and start

First, you make sure all of the liquid (water) is emptied out of the buret. Next, you fill the buret with sodium hydroxide

Although this experiment was not an aquatic plant, it can be support for predictions made. The net formula for photosynthesis is CO2 +H2O -> CH2O +O2. Therefore, by increasing the levels of NaHCO3 (or CO2) available to an aquatic plant, the amount of oxygen produced will increase with it. To approach this experiment, an isolated testing environment will be used. The form of this being a sealed 75 ml glass tube in a 250 ml Erlenmeyer flask filled with water to stabilize any temperature changes. The aquatic plants will be evenly cut and submerged in varying concentrations of NaHCO3 solutions and placed at equal distances from an uncoloured light source. A 1 ml pipette will measure the oxygen output of the system and many trials will be made to ensure accuracy. The null hypothesis in this case will be that a higher NaHCO3 concentration will not increase/influence the oxygen production of an aquatic plant. The prediction for this lab is, if the reactants of photosynthesis are increased, namely NaHCO3, then the oxygen output of an aquatic plant (Elodea densa) will also increase with it.

Fill the beaker with 500 mL of water and 2 drops of detergent. Add 5 grams of baking soda using the spoon. Using the stirrer, stir gently; there should be no bubbles when finished.

Begin by weighing a 125-mL Erlenmeyer flask and recording the result. Next, add approximately 2 g of salicylic acid to the Erlenmeyer flask. Then, record the new mass of the Erlenmeyer and the salicylic acid. Next, inside of the hood add 5 mL of acetic anhydride and 10 drops of 85% phosphoric acid. Stir the mixture with a stirring rod. Next, place the flask in a boiling water bath and stir until the solid dissolves. Next, remove the flask from the water bath and let it cool to room temperature. Then, add 20 drops of water to the flask. Next, add 25-mL of cold water to the flask and place it in an ice bath for 10 minutes. After 10 minutes, to collect the Aspirin crystals, add a piece of filter paper to a Büchner filtration apparatus. Then, fit the funnel snuggly in the rubber washer of the filter flask. Next, turn on the water aspirator and pour the aspirin product slowly onto the center of the filter paper. Then, push down gently on the funnel to suction out the water from the aspirin product. After the crystals have formed on the filter paper, obtain a weight boat. Record the mass of the weight boat. Next, use a spatula to transfer the crystals onto the weigh boat. Then, after the crystals have dried, record the mass of the weight boat and aspirin product.

Using the tape cover the drainage wholes of the pot, fill container with water and using take the initial weight. Empty the container and properly wet, mix and fill pot with soilless media. Slowly fill the pot with a measured amount of water to be level with media. Once full remove tape over a beaker and measure amount of water once the container stops dripping, this will be representative volume of the aeration porosity. Once fully drained weigh the

This experiment was conducted to learn the relationship of 3 different types of pipettes and how to be accurate at measuring volumes of substances very accurately in quantitative analysis lab work. The accuracy of the measurement is the degree of closeness of measurements of a quantity’s actual volumes and the precision is the degree to which that are repeated measurements that are not changed show the same results.