Testing And Analyzing The Quality Of Water

Procedure- The procedure for this lab includes many simple steps and a few different things we are testing. Our first Procedure was to combine water and salt to see what kind of reaction it would make. First we fill the graduated cylinder with 100 ml of water. We then measured 1.0 grams of table salt on a balance to get an accurate amount. After, we took the measured amount of salt and poured it into the water filled beaker. Lastly, we watched and recorded the reaction.

In the Chemistry of Natural Waters Lab we were to collect a sample of water, ranging from a fountain, stream, bottle, or tap water. After we collected the samples we all did many tests to see what the hardness was for each one. Water hardness is determined by the amount of Calcium and Magnesium in the water.(2) Water that has more Calcium or Magnesium is considered to be harder than water with less of those two elements. When you use soap and detergent, this is where you see water hardness coming into play in everyday life when you are washing things.

The materials that were used to carry out the experiments on the water samples were ten testing kits. We ran 10 tests on all

19. Stir the solution with a toothpick and observe any changes. Measure the pH of the new solution and record into Table 2.

ii. The second part of the titration series involves titration of NaOH with Hydrochloric acid (HCL). Again, three reps of titration and a blank titration have to be completed. A volumetric pipet is used to measure 10.00mL of HCL into three labeled conical flasks. Then the flasks are filled with deionized water until about the 50mL mark. A buret is

iii. Materials: Distilled water, beverages (juice, soda, sport drinks), Sugar reference solutions (0, 5, 15, ad 20%) 25ml each, Balance, centigram(0.01g precision), Beaker (100-mL), Erlenmeyer flask (125-mL to collect rinse solutions), Pipet(10-mL), Pipet bulb or pipet filler

In the experiment we were determining the chemical formulas for the hydrated, and dehydrated samples. The purpose of this was to asses our knowledge of chemical formulas, and how they relate to each other.

In experiment 3 drinking water quality, I will test the quality of two different types of bottled water and tap water using materials such as: Dansani bottled water, Fiji bottled water, ammonia test strips, chloride test strips, 4 in 1 test strips, phosphate test strips, iron test strips, (3) 250ml. beakers, parafilm, pipettes, (3) foil packets of reducing powder, stopwatch, permanent marker and water. First you must label the (3) 250ml. beakers with Tap water, Dasani, and Fiji, and pour 100ml of each type of water into the beakers name. Next place an ammonia test strip with the pads down into the tap water and move it up and down for 30 seconds. Next remove the test strip shaking off excess water and then hold level with pad side up for 30 seconds. Read the results of the strip pads by

The third experiment I did was to see the quality of tap water, Dasani water and Fuji water. I first labeled 250ml beakers Tap, Dasani and Fuji. I then poured 100ml of each water type into there specific beaker. The first strip test I did was the ammonia test. I placed the strip in each of the 3 beakers for 30 seconds to see the test strip level. Then compared to the strip color to the colored charts that were given. I repeated the same steps for chloride except for putting the test strip in for 1 second. Next, I did the 4 in 1 test repeating the same steps besides placing the test strip in the beaker for 5

This study concentrated specifically on eight potential indicators of poor water quality, including color, turbidity, chloride, total hardness iron, phosphate, nitrate, and pH. Of these parameters, nitrate is the only MCL substance, the remaining seven are considered SMCL's, and were measured strictly for aesthetic purposes. The composition of two water samples, yielding from sources of different regulation, was studied to develop a better understanding of contamination prevalence. The first sample was collected from a drinking water fountain found inside the Natural and Environmental Sciences (NES) building. This water is treated and cleaned after being extracted from the Floridian Aquifer. The second was taken from the edge of a pond in Simmons Park, found on campus. This water source intercepts significant surface runoff and works as a retention basin for the surrounding area. Before conducting the experiment, it was expected that the NES water fountain would provide a sample more in compliance to the MCL and SMCL standards set by the EPA when compared to the Simmons Park Pond water. It is likely that the color and turbidity of the pond water will yield higher measurements than the NES drinking water. This was predicted to be the result, as the NES drinking water comes from a source of

Sixth, the stopper for the test tube was put into the test tube, and the test tube was placed into the test tube rack. Seventh, the procedure of measuring the water, testing the pH and labeling the test tube was repeated until all the different brands/types of water were in a test tube and were placed in a test tube rack that was labeled “Warm/Room Environment” by ripping off a piece of tape and writing “Warm/Room Environment” using a pen/pencil and placing it on the test tube rack. Each time a different type/brand of water was measured, the graduated cylinder was wiped dry using a paper towel. Eighth, this process was repeated for the cooler environment. However, these test tubes were instead placed in a rack that was labeled “Cooler Environment.” Ninth, the test tubes that were placed in the test tube rack labeled “Cooler Environment” were placed into a refrigerator, and the test tube rack labeled “Warm/Room Environment” were placed in a room on a table. Tenth, for eight days, the pH of the different waters were tested twice daily to ensure accuracy and to check for any changes in pH in both environments and observations were made

The significance of titration is to find out the concentration of unknown substances. There are different kinds of titration and this experiment consists of two kinds of titration. The traditional titration uses the phenolphthalein indicator dye to determine the concentration by color change. The modern titration uses pH electrodes. The chemical reaction “H3C6H6O7(aq)+3OH-(aq)→3H2O(l)+C6H5O7(aq)” is used to determine the moles of citric acid from the moles of NaOH. The main scientific objective of the experiment is to determine the molarity of two different sodas by traditional titration and modern titration respectively.

Part 1: First, all materials was gathered: metal sample (aluminum), empty jar, electronic scale with 0.01 accuracy, calculator, thermometer, paper towels and lab worksheet. A sink was also needed for tap water. The mass of the empty jar was weighted and recorded in the lab worksheet. The mass of dry metal was weighted and recorded in the lab worksheet. About 1/8 of the jar was filled with tap water. The temperature of the water was measured and recorded in the lab worksheet. It was made sure that the thermometer did not touch the walls of the jar. The mass of the jar filled with water was then weighted and recorded in the lab worksheet. The metal was placed inside the jar filled with water. It was made sure that the water did not splash out of the jar during the placement. The mass of the jar filled with water and metal was then measured and recorded in the lab worksheet. All the material was returned to the teacher and in their original conditions- clean and dry.

Part 1 of the experiment was the standardization of the Iodine solution. First, three ascorbic acid samples were weighed out to 0.10 grams each and then placed into a 250mL Erlenmeyer flask. Each flask containing the sample was then filled with 100mL of distilled water and the ascorbic acid dissolved. Next, 100 mL of the stock I2 solution was measured into a 400mL beaker and 150 mL of water was added and thoroughly stirred. A buret was obtained, washed thoroughly, and then rinsed three times with the I2 solution. Then the buret was filled with the I2 solution. 1 mL of starch indicator was added to the first ascorbic acid sample. An initial reading on the buret was recorded and then the titration began. The flask was gently swirled to mix the solution as the titration was

Step 1 and 2 was repeated by using distilled water by replacing the test solution.