* 3. 3.0 ppm standard: * 3.00 mL of 10.0 ppm phosphate solution was placed in a 25 mL graduated cylinder and diluted to exactly the 10 mL mark with distilled water then poured into a plastic cup labeled 3. Cylinder was rinsed with distilled water. * * 4. Zero standard: 10 mL of distilled water was poured into a plastic cup labeled 0.
We found the mass of our pure alcohol to be 10.23g. The volume of our pure alcohol was 10.97mL. With these numbers, we used the formula mass/volume to find the density of our pure alcohol to be .9325g/mL. The percent error of our experiment was found to be 18.19% with an absolute error of .1435%. Conclusion:The purpose of this lab is to prepare and purify a fuel, ethanol C2H5OH.
For every 20 drops of solution you will add 0.1g of zinc to the new test tube. Repeat steps 3 and four until the solution is clear. If there ever exists too little of the solution to get enough drops, add up to 1mL of distilled water to the solution. 4. Once the solution is clear, retrieve at least ten drops of the solution and place them in a new test tube.
Materials and Methods Part 1 For the cation elimination test first 10 drops of potassium, iron (III), zinc (II), copper (II), and cobalt (II) were added to 5 centrifuge tubes and the color was recorded. Then for the metal hydroxide test, 6 M NaOH was added drop wise till a precipitate was formed. Each solution except potassium formed a precipitate, so then 10 additional drops of NaOH were added to the remaining solutions. Tubes were cleaned with distilled water and 6 M HCL. Next was the ammonia test 10 drops of each metal solution were added to new centrifuge tubes and 15 M NH4OH was added until the solution changed color or a precipitate was formed.
A) How many mosm solute will 1 gram of NaCl yield? Show your calculations. (1gNaCl/1)*(1000mg/1gNaCl)(2/58mg)=34.5mOsm. 3. Mixed Solutions: If 1 mmole of glucose (180mg=1mOsm) and 1 mmole of NaCl (58mg=2mmOsm) are put into a beaker and distilled water added to make 1 liter, the osmolarity is 3 mOSm/L.
From your three trials, calculate the average volume of Na2S2O3 needed for the titration of 25.00mL of diluted bleach. 3. Use the average volume and the molarity of Na2S2O3 to determine the molarity of the diluted bleach. (Find moles of Na2S2O3, convert to moles of NaClO, and divide by volume of dilute bleach that was titrated in each trial to get M). 4.
The solubility of the solution containing Ca(OH)2 in NaOH had a smaller solubility of 4.15 g/L than the solution containing Ca(OH)2 in water, which had a solubility of 4.45 g/L. This experiment successfully showed the relationship between the concentration of the Ca2+ ions in solution. Introduction: Many ionic compounds are considered to be “insoluble” in water, but no compound 8placed in water. When the slightly soluble compound stops dissolving the ions in the solution and the undissolved solid are in equilibrium.  A saturated solution is one that holds as much dissolved solute as possible at a given temperature, therefore only a small amount of a slightly soluble ionic compound is needed to produce a saturated solution of that compound.
Kobs is the slope on the graph plotting Vol of NaaS2O3 against time. Specific hydrogen ion catalysis Kobs = KH+[H+] This is used when a strong acid is being used in the reaction as it acid fully dissociated and there is no A- value. This is the equation used for reactions (i), (ii) and (iv) as they used HCl as the acid. General acid catalysis Kobs = KH+[H+] + KHA[HA]. This is used when a weak acid is being used in the reaction as it acid does not fully dissociated and there is an A- value.