0.00079 moles EDTA4- c. 0.00079 moles ZnI2 d. 0.0517 grams of ZnI2 are in the sample e. 0.0517/0.237= 21.8% f. Error Is 6.34% Lab Report: Part 1: In this lab we used the following supplies: * Zinc Iodide * Na2H2EDTA(s) * Calmagite indicator solution * pH 10 buffer solution * 6M Acetic Acid * Unknown Zinc Compound The main purpose for this part of the lab was to determine the amount of zinc ion in a sample of ZnI2 by titration. The two types of zinc: * Zinc iodide made by zinc and iodine * Commercially purchased zinc iodide (the
Zing Substances. For ionizing substances, such as NaCl , 1mosm is 1mmole times the number of ions formed when each molecule dissociates. One mmole of NaCl is 58 mg, but when it dissociates, it yields 1 mmole of Na+ (23mg) and 1mmole of Cl ( 35mg). Therefore , 58 mg of NaCl is 2 mOsm of NaCl is put into a beaker and distilled water added to make 1 liter, the osmolarity is 2mOsm/l. A) How many mosm solute will 1 gram of NaCl yield?
29.4 atm B. 4.89 atm C. 25.1 atm D. 36.0 atm _____ 5. The vapor pressure of pure ethanol at 60 °C is 349 mm Hg. Calculate the vapor pressure at 60 °C of a solution prepared by dissolving 10.0 mol of naphthalene (nonvolatile) in 90.0 mol of ethanol. A.
6. How many moles of NaCl are in 250. mL of a 0.200 M solution? 1. 15.8 g of KCl is dissolved in 225 mL of water. Calculate the molarity.
Ally Emerson Lab Report H. Chem. Period 3 1-11-15 How does mixing distilled water, iron, and copper (II) sulfate and then boiling the mixture help us determine the theoretical and percent yield of copper after the chemical reaction? Partner: Naomi Purpose: To determine the theoretical and percent yield of copper after a chemical reaction between distilled water, iron, and copper (II) sulfate. Hypothesis: There will be around 2 grams of copper left, which will equal a 89% yield. Materials: scale, filter paper, weighing paper, distilled water, copper (II) sulfate, iron, beaker, tongs, drip, and a funnel.
Part C: Density of Sodium Chloride (NaCl) Solution, a sample of NaCl was obtained and measured using a 100mL beaker and a 10mL pipet to determine the concentration of the solution. In order to obtain the appropriate result, a calibration graph and density measurement was used to determine the concentration of the sodium chloride solution. In conclusion, based on the water temperature of 21.8°C in part A’s graduated cylinder experiment obtained, it was determined that the average density was .0973g/mL with a percentage error of 2.5%. When graphed the measurement was equal to Y=0.988x. Part B: The graduated pipet’s average density at 22.3 °C was determined to be 0.9785g/mL with a percentage error of 1.89% shows the graduated pipet to be more accurate and precise.
Part 1- Description of Substances: - Mossy Zinc: Shiny and small solid - Magnesium Ribbon: Shiny and long metallic solid - HCl: Clear liquid Description of Zinc and Mg reaction with HCl: - Observations of Mossy Zinc: It stays on the bottom after the addition of the HCl and there is only light bubbling. - Magnesium Ribbon: The ribbon moves around after the addition of the HCl and there is a large amount of fizzing. Dilution Data: - 1.5 M: Add 18.75 mL of the 2M HCl and mix with distilled water until the entire solution is measured to be 25 mL - 1.0 M: Add 12.5 mL of the 2M HCl and mix with distilled water until the entire solution is measured to be 25 mL - 0.75 M: Add 9.375 mL of the 2M HCl and mix with distilled water until the entire solution is measured to be about 25 mL -
What amounts of stock solution and water do you need to use? (Remember that you will need enough solution to more than cover the egg.) p. Write up your new dilution procedure in your lab notebook, including the calculated salt concentrations for each cup. q. Make the new dilution series.
How many kilograms of pure HCl would be used to make this hydrochloric acid? (Assume that 30% has two significant figures. There are 2000 lb/ton.) (Obj 15) 30 ton HCl 2000 lb 1 kg ? kg HCl = 6.0 × 105 ton HCl soln 100 ton HCl soln 1 ton 2.205 lb 30 ton HCl 2000 lb 453.6 g 1 kg ?
Calculate the value of Ke for this system. 2 H2S (g) === 2 H2 (g) + S2 (g) [1.1(10-4] 7. At a given temperature, the following system has an equilibrium constant, Ke, of 0.27. C(g) + B(g) === 2 E(g) The system was established by placing 8.00 moles of C and 5.0 moles of B in a 4.0 L vessel. Calculate the concentration of all substances at equilibrium.