Results Sheet, Experiment 13 Brand of Vinegar used:________________ Acetic Acid % from bottle label_____________ | Initial NaOH Reading(estimate to 0.1 mL) | Final NaOH Reading(estimate to 0.1 mL) | Volume NaOH used(Final – Initial) | Trial 1 | 9.5 | 1.3 | 8.2 | Trial 2 | 9.6 | 1.4 | 8.2 | Trial 3 | 9.7 | 1.4 | 8.3 | Average Volume of NaOH used | 8.2 | Calculations: Normality of the acetic acid: .82 Mass of acetic acid: 49.2 % acetic acid (divide the grams, above, by the volume you used to get g/L): 4.92 Answer questions A-G in the lab manual: A. What is the average % acetic acid in your vinegar sample? Standard vinegar is 5% acetic acid. How does your result compare with the standard? The average was 4.92 which is pretty close comparably to the standard.
With renal compensation for respiratory acidosis, the pH of the urine You correctly answered: b. decreased because [H+ ] increased. 07/18/13 page 3 Review Sheet Results 1. Describe what happened to the concentration of ions in the urine when the
With the use of this technique we placed chlorine, bromine, and iodine into solutions containing chloride, bromide, and iodide. In the reaction the free halogen (X2) oxidizes the other halide ion (Y-) and gets reduced by gaining electron(s). In table 3, chlorine was the strongest oxidizing agent and iodine was the weakest oxidizing agent. Since chlorine was the strongest oxidizing agent it will react more and the weak agent will react less. This explanation can be demonstrated in table 3 also because the results of the reactions demonstrates that chloride reacted more by the color of the product compared to the color of chloride in the mineral oil.
Laboratory Report/ Marlinda Saintil/ Influence of Fluid Intake on Urine Formation/ Florence Vicil/ 05.04.2015/ Page [1] of [3] L/day 7.4 6.8 7.5 7.3 2. Does water loading increase, decrease, or not affect average urine production rate (L/day). Table 4. Osmolarity (mosm/L) Subj. 1 Subj.
Therefore each compound has similar solubility in water. The hydrogen bonds in butanol are stronger that the dipole interactions in diethyl ether. Butanol has a higher boiling point because of the stronger hydrogen bonds. The intermolecular forces holding the butanol molecules together are stronger than those holding the diethyl ether molecules together. 2) Predict which of the following in each set of compounds will have the highest water solubility.
Then you put the remaining liquid (neutral component mixture) through the suction filtration funnel to isolate the crystals. After 10-15 minutes, the crystals will be dry and you can weigh them and find their melting point. How is the neutral component of your 3-compound mixture isolated from the final methylene chloride solution? 16 of 22 4/16/12 9:15 PM StudyBlue Flashcard Printing of Lab Final 2211L UGA http://www.studyblue.com/servlet/printFlashcardDeck?deckId=... Name the four active ingredients that we will be testing for in the TLC of Analgesics lab: Ibuprophen Caffeine Acetaminophen Acetylsalicylic acid What solvent system will you be using to dissolve the common analgesics (power) in preparation for TLC spotting? Methylene chloride: ethanol (1:1 solution) What solvent system will you be using to "develop" your TLC plates in the TLC of Analgesics lab?
Next the freezing point which didn’t eliminate either of them. Next we look at the mass which was 7.465g/ml. This make me lean toward ethyl ether but the masses were still pretty close. Next we move to the solubility of the substances. They are both very soluble in alcohol and hexane so that doesn’t help, but in water ethyl ether is semi soluble and pentane is in soluble.
The reason I believe they were the most effective am because they both caused the inks to spread out the furthest amount. While vegetable oil, and alcohol did not do all that much. (5 points) Score 3. Which solvent caused the ink from the dots to move the most? Which solvent caused the ink from the dots to move the least?
Calculate the molarity of the original vinegar solution and its concentration in gdm-3, given that it reacts with NaOH in a 1:1 ratio. 7. 2.5 g of a sample of ethanedioic acid, H2C2O4.nH2O, was dissolved in water and the solution made up to 250 cm3. This solution was placed in a burette and 15.8 cm3 were required to neutralise 25 cm3 of 0.1 moldm-3 NaOH. Given that ethanedioic acid reacts with NaOH
Among four types of surfactants, partially hydrolyzed PVA is most frequent used because it gives the smallest microsheres (Jeffrey et al, 1991). The amount of PVA used may affect microparticles properties. Freitas and coworkers have added 1.3% and 8% of PVA into an aqueous solution and found that both lower and higher concentrations of surfactant results in coagulation of the particles. Hence, these authors suggested to use 3% of PVA as it the most optimum concentration. (Freitas and Marchetti,