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.
* 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.
Obtain beaker filled with 250 mL of HCl and 5 pennies. 2. Get a pipette and remove 10 mL of that solution (HCl + Zn) and place it in a 100 mL beaker. 3. Add color indicator 4.
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.
Section 3: The titration of an unknown concentration of HCl with the standard solution of NaOH. Section 4: Use the HCl solution titrate a commercial basic product and determine the quantity of active ingredient. -Section1: Preparation of a Standard Sodium Hydroxide Solution Materials 250-mL volumetric flask Weigh scale Weighing bottle, or watch glass for NaOH sample, Glass funnel Dropper pipette 100 ml beaker Deionized water NaOH solid Procedure 1. Weigh approximately 1 gram of NaOH in a weighing bottle. Record the actual mass (1.01 grams weighed) in the results table.
Twenty drops of bromothymol blue was also added to the 150mL beaker. The pH was then obtained using the Vernier pH probe and it read 6.68. The 5mL pipet was then used to transfer 5mL of the green solution to the three 50 mL beakers. A 100mL beaker was obtained and filled with 1.0 M HCl solution and the pipet was used to acquire 1mL of the 1.0 M HCl solution. The 1mL of HCl was then transferred to one of the 50mL beakers turning the color of the solution to yellow.
Part C: Density of an Irregular Shaped Solid 1) Obtain a sample of metal and determine the mass. 2) Fill a 100 mL or 50 mL graduated cylinder with water, recording its volume. 3) Using the water displacement method, determine the volume of the object. 4) Determine the density and percent error. Part D: Density of Methanol 1) Find the mass of an empty 10 mL graduated cylinder, and then fill approximately 9 mL of methanol and record volume.
Solution Stoichiometry and Gas Law Problems Problem 1 In flask A, 1.500g of silver nitrate solid is dissolved in 50.0mL of water, while in flask B, 0.500g of potassium carbonate is dissolved in 25.0mL of water. The two solutions are then mixed together. a) Before mixing, what is the molarity of each solution? b) Write the balanced molecular equation, the complete ionic equation, and the net ionic equation for the reaction. c) If the percentage yield is 85.0%, what mass of precipitate is actually produced?
5. Potassium hydroxide solution: Use 0.01 M potassium hydroxide, 0.56 g/L. 6. Ammonium hydroxide solution: Add water to 10 mL of concentrated ammonium hydroxide solution to make 82 mL of a stock solution. Use 10 mL of the stock and dilute to 1 L with distilled water.
The mechanism for the reduction of a ketone by sodium borohydride: (1) Method (Based on Chemistry Laboratory Manual): 1. 0.4510g of benzophenone was dissolved in 5 cm3 of ethanol in boiling tube containing a magnetic stirrer bar. 2. O.1249g of sodium borohydride was added and left for 30 minutes. 3.