In the first part, five 100 mL flasks of 5 mL ligand solution, 5 mL 2 M sodium acetate, 4 mL 3 M NH2OH, and 1-5 mL Fe2+ solution are diluted with water. The absorption spectrum for varying concentrations of Fe2+ are measured using a spectrophotometer and the data is graphed in Excel. The slope of the line is ε in the Beer-Lambart equation A = εcl. In the second part of the experiment, eleven flasks containing diluted stock solutions of Fe2+ and ligand are mixed with 5 mL 2 M sodium acetate and 4 mL 3 M NH2OH and diluted with water. The absorption spectrum is measured using a spectrophotometer and the data is graphed in Excel.
Mix. k. Measure out 3/4 cup of the solution from cup 3 and add it to cup 4. Mix. l. What are the relative salt concentrations of cups 1–4? Example: Cup 2 is made up of half stock solution and half tap water, which is a 50 percent relative salt concentration.
Attempt to get as close to your calculated amount as possible. Record this amount in your data table. 3. Weigh a clean 500 mL Erlenmeyer flask. Record this amount in your data table.
Calculate the volume of 0.250 M H2SO4 that contains 0.250 g H2SO4. 0.250 g H2SO4 x 1 mole x 1 L = 0.0102 L 98.12 g 0.250 mole 5. 1.50 g of NaCl is dissolved in 100.0 mL of water. Calculate the concentration. 6.
Calculate the equilibrium constant, Ke. [0.85] 4. If the equilibrium concentration of F2(g) is 1.50 mol/L and H2(g) is 2.5 mol/L, determine the concentration of HF(g) at equilibrium. [1.92 mol/L] F2 (g) + H2 (g) === 2 HF(g) Ke = 0.98 5. If 0.100 mol of hydrogen iodide is placed in a 1.0 L container and allowed to reach equilibrium, find the concentrations of all reactants and products at equilibrium.
Also include any observations that you made over the course of part II. (4 points) Unknown (A,B,C,D) Mass of Metal Volume of water Initial temp. in calorimeter Initial temp. in beaker Final temp. of mixture Metal C 25.605g 24.6mL 25.2°C 100.5°C 28.7°C Calculations: Show your work and write a short explanation with each calculation.
(0.125)(0.1) = 0.0125 moles of solute b. Pour 50 mL of the stock solution to get the number of moles needed. 6. Exercise 6: a. (0.02) (1) = x/ 372.24 x=7.4 grams of sodium EDTA that is weighted out. b.
Collect 6 grams of copper (II) sulfate on weighing paper. Weigh and record. 5. Collect 50 mL of distilled water into the beaker. 6.
Record the actual mass (1.01 grams weighed) in the results table. 2. Transfer the sample of NaOH to the 250 ml volumetric flask. 3. Put approximately 50 ml of deionized water into the flask and dissolve all of the NaOH.
Research Question: Will samples of water obtained from drinking water points have a concentration of TDS which is suitable for drinking purposes? Aim: To determine and prove that the concentration of TDS in the drinking water samples will be suitable for drinking purposes. Hypothesis: The samples of water which were obtained from the drinking water sources will be under the threshold of 500 mg/l of TDS. Background information: Drinking water will tend to be between 25-500 mg/l of TDS concentration and the maximum concentration threshold for drinking water is 500 mg/l of TDS Dependent Variable-Quality of water sample Independent Variable – TDS concentration in water sample Controlled Variable- Temperature of the sample, Volume of the sample Materials Required: 1. Vernier Conductivity probe 2.