Volumetric Analysis Lab

If the NaOH managed to absorb water before measured, then the measured mass of the NaOH

1. Objective: My objective for this experiment is to find the mass, volume, and density of a variety of objects. After this, I will record my data and place a select few of the items on a graph. My hypothesis for this experiment is, "If I measure the mass of every object, the wooden ball will have the least because it seems to be the smallest and most lightweight. " 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

The volume of a small test tube and a thin-stemmed pipet were determined in this section of the lab. Water was poured into a small test tube until the water reached the very top edge of the test tube. The test tube was then emptied into a plastic 25 mL graduated cylinder and volume was measured and recorded into data table 3. A think-stemmed pipet was completely filled with water. Drops were carefully counted and emptied into the empty plastic 25 mL graduated cylinder until the water level reached 1 mL. The number of drops in 1 mL was recorded into data table 3. The thin-stemmed pipet had a total volume of 4 mL and that was also recorded into data table 3.

The purpose of this lab was for my group, which was just Wendy Say and I, to use a graph to help measure density. We had to measure the mass and volume of several samples of pennies, and then create a graph to determine the pennies’ average density. We used seven materials, which were used in two different parts. In the first part we used a graduated cylinder, a scale, paper towels, a pencil and twenty-four pennies. The graduated cylinder was used to measure the volume of the pennies by water displacement, the scale was used to measure the mass of the pennies, the paper towel was used to dry pennies because we couldn’t reuse them, and the pennies were needed because we were getting their average density.

Methods: First, a burette, ring stand, clamp, and an empty flask were obtained. The burette, with the valve closed, was attached to the ring stand with a clamp, and the empty flask was placed below the burette. Next, 50mL of the NaOH solution were poured into the burette, and a small bit was drained into the empty flask to ensure that the tip of the burette was also full of NaOH solution. The volume of the NaOH in the burette was recorded. Next, approximately 0.6 grams of KHP were massed poured into an empty 125mL flask. Two drops of an indicator solution were added to the KHP

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.

The 100 mL graduated cylinder is the most precise piece of glassware to measure volume.

By using acid-base titration, we determined the suitability of phenolphthalein and methyl red as acid base indicators. We found that the equivalence point of the titration of hydrochloric acid with sodium hydroxide was not within the ph range of phenolphthalein's color range. The titration of acetic acid with sodium hydroxide resulted in an equivalence point out of the range of methyl red. And the titration of ammonia with hydrochloric acid had an equivalence point that was also out of the range of phenolphthalein.. The methyl red indicator and the phenolphthalein indicator were unsuitable because their pH ranges for their color changes did not cover the equivalence points of the trials in which they were used. However, the

The carboxylic acid was mixed with enough HCl to precipitate and was put on a vacuum filtration apparatus. The weight of the residue was recorded. 6. They then mixed the original solution with 10mL of sodium hydroxide.

This is an experimental lab that tested how well an antacid acid tablet will dissolve in excess stomach acid. The lab can help the creators and consumers of the drug with know how efficient the drug is. Each group got a certain antacid acid tablet to test. The lab utilizes back titration to help with figuring out the amount of hydrochloric acid(HCl) that is dissolved by an antacid acid by introducing a base with a known molar concentration. The tablet effectiveness was tested by seeing how much strong base (Sodium Hydroxide-NaOH) is needed to be added to a strong acid solution (HCl and antacid acid tablet) for a color change. A color change means that the acid solution became basic, so enough base was added to neutralize the acid. The results

Background: Acids are known to chemistry as the chemical substances that are below seven on the pH scale and they cause litmus paper to turn red. They are also known to have a sour taste but not all acids should be tasted due to some of them being extremely dangerous and should not be in contact with human body parts. In this lab, we worked with an acid known Hydrochloric Acid (HCl). HCl is a clear liquid that visibly looks no different from water. HCl is known to be very dangerous when in contact with skin, eyes, ETC, and should be dealt with caution.

After all the solid NaOH has dissolved a beaker, pour the beaker into the 250ml volumetric flask until almost reaching the mark on the neck of the flask and using a dropper, add distilled water until the meniscus reaches sits on the mark on the neck of the flask. To mix thoroughly, put a stopper at the mouth of the glass and then shake the volumetric flask. For part B, KHP is used to standardize NaOH solution. We started the experiment by cleaning the burette with distilled water and rinsing the burette with NaOH solution to prevent any changes of the concentration of NaOH.

The purpose of this lab was to use process titration to find concentration of an aqueous solution of Hcl(aq) , using KOH(aq) as the titrant.

For this experiment, a pH meter was used so this part of the experiment began with the calibration of the pH meter with specified buffers. The buret was then filled with the standard HCl solution and a set-up for titration was prepared. 200g of the carbonate-bicarbonate solid sample was weighed and dissolved in 100 mL of distilled water. The sample solution was then transferred into a 250-ml volumetric flask and was diluted to the 250-mL mark. The flask was inverted several times for uniform mixing. A 50-mL aliquot of the sample solution was measured and placed unto a beaker. 3 drops of the phenolphthalein indicator was added to the solution in the beaker. The electrode of the pH meter was then immersed in the beaker and the solution containing the carbonate-bicarbonate mixture was titrated with the standard HCl solution to the phenolphthalein endpoint. Readings of the pH were taken at an interval of 0.5 mL addition of the titrant. After the first endpoint is obtained, 3 drops of the methyl orange was added to the same solution and was titrated with the standard acid until the formation of an orange-colored solution. Readings of the pH were also taken at 0.5 mL addition of the titrant.