REAGENTS 0.10 M KI 3% H₂O₂ H₂O MIXTURE #1 15.0 mL 10.0 mL 35.0 mL MIXTURE #2 15.0 mL 20.0 mL 25.0 mL MIXTURE #3 30.0 mL 10.0 mL 20.0 mL In each trial the total volume of reagents used is 60.0 mL
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- TITRIMETRIC DATA SAMPLE: CANE VINEGAR % acidity in label: 4.5% %purity of KHP: 99.80% FORMULA WEIGHT of KHP: 204.22 g/mol STANDARDIZATION OF NaOH SOLUTION TRIAL 1 TRIAL 2 TRIAL 3 Weight of KHP, g 0.1012 0.1004 0.09987 Initial volume of NaOH, mL 5.00 10.01 Final volume of NaOH, mL 4.95 9.99 14.93 Molarity of NaOH Average Molarity of NaOH ANALYSIS OF ACETIC ACID IN A VINEGAR SAMPLE TRIAL 1 TRIAL 2 TRIAL 3 Volume of vinegar, mL Initial volume of NaOH, mL 1.00 1.00 1.00 14.98 22.90 30.87 Final volume of NaOH, mL 22.84 30.77 38.75 Molarity of acetic acid Average molarity of acetic acid ANALYSIS OF CARBONIC ACID IN A SODA SAMPLE TRIAL 1 TRIAL 2 TRIAL 3 Volume of soda, mL 20.0 20.0 20.0 Initial volume of NaOH, mL 20.20 22.05 23.93 Final volume of NaOH, mL 22.03 23.89 25.8 Molarity of carbonic acid Average molarity of carbonic acid1. 500.0 mL 0.2 M KI2. 500.0 mL 0.2 M KCl3. 500.0 mL 0.1 M K2S2O84. 500.0 mL 0.1 M K2SO45. 500.0 mL 4.0 mM Na2S2O3 (from Na2S2O3∙5H2O)pls compelete the 2nd table given the dataA sample is analyzed for chloride using the Volhard method. What is the percentage chloride as NaCl using the following data? Weight of sample: 303.0 mg AgNO3 used: 40.00 mL of 0.1234 M KSCN used: 12.20 mL of 0.0930 M
- 1. A 50.00 mL stock CaCl2 solution was diluted with water in a 250.0-mL volumetric flask. A 25.00 mL aliquot of this was further diluted to a final volume of 100.0 mL. Finally, 20.00-mL aliquot of the resulting solution was analyzed and found to contain 0.1500 M CaCh2 Solve for the concentration of the stock solution in M. 2. A 50.00 mL stock CaCl2 solution was diluted with water in a 250.0-mL volumetric flask. A 25.00 mL aliquot of this was further diluted to a final volume of 100.0 mL. Finally, 20.00-mL aliquot of the resulting solution was analyzed and found to contain 0.1200 g CaCl2 Solve for %w/v CaCl2 in the stock solution.4. The Ksp for MgCO3 = 1.1 x 101º. CIRCLE the solubility of MgCO3 in pure water. a) 1.1 x 10-10 M b) 1.1 x 108 M c) 1.1 x 107 M d) 1.1 x 106 M e) 1.1 x 10$ MTable 1: Temp vs. solubility data of ammonium chloride. Test tube g NH4Cl/10 mL H2O Crystallization temp. (ºC) 1 1.0 g/10 mL H2O 10 oC 2 1.8 g/10 mL H2O 20 oC 3 2.9 g/10 mL H2O 40 oC 4 3.8 g/10 mL H2O 65 oC 5 4.4 g/10 mL H2O 95 oC Use the table to plot a solubility curve for ammonium chloride on the graph provided below. For the best fit line, use a smooth curve. "Mass of Solute per 100 mL of H2O," should be written on the y-axis (use increments of 2g for every box). "Temperature (°C)" should be written on the x-axis (use increments of 10 °C for every 2 boxes).
- TITRIMETRIC DATA SAMPLE: CANE VINEGAR % acidity in label: 4.5% %purity of KHP: 99.80% FORMULA WEIGHT of KHP: 204.22 g/mol Average Molarity of NaOH: 0.09934 M ANALYSIS OF CARBONIC ACID IN A SODA SAMPLE TRIAL 1 TRIAL 2 TRIAL 3 Volume of soda, mL 20.0 20.0 20.0 Initial volume of NaOH, mL 20.20 22.05 23.93 Final volume of NaOH, mL 22.03 23.89 25.8 Molarity of carbonic acid Average molarity of carbonic acidAverage mass of the precipitate MgNH4PO4·6H2O (s) / g Average phosphate concentration in water sample (mass/volume %) % difference of 2 trialsAs part of this experiment you will need to determine the concentrations of Fe* and SCN ions present in test tubes 1-9. These values can be calculated using the volumes and concentrations provided in Tables 1 and 2 of the Equilibrium Lab - Procedure and the dilution equation (M,V1 = M2V2). Note: the solutions provided in the lab, and therefore the tables in the lab document, are the compounds used to prepare the solution. You must determine the concentration of the ions based on how these compounds díssociate in solution Complete the following table by filling the the calculated initial concentrations of each substance. Be sure to: Pay attention to significant figures • Round appropriately Use decimal notation (not scientific) Do not include units Test Initial [Fe3*] (M) Initial [SCN'] (M) Tube 1 3 4. 6. 7 8. 2.
- The following data were collected for the reaction 2A + 2B + C 3G+ 4 F Experiment 2 3 4 5 [A] Units of Molarity .00125 .00250 .00125 .00125 .00301 [B] Units of Molarity 00125 .00125 00302 00302 .00100 [C] Units of Molarity 00125 .00125 .00125 00375 .00115 Rate Units M/s 00870 .0174 .0508 .457 a. What is the order with respect to each reactant and what is the overall order for the reaction? Answer this question within the answer box and show your work clearly labeled on the scratch paper. b. Write the rate law for the reaction. Answer this question within the answer box and show your work clearly labeled on the scratch paper. c. What is the value and units for k? Answer this question within the answer box and show your work clearly labeled on the scratch paper. d. Predict the rate for experiment 5, you should give a value and units. Answer this question in the answer box and show your work on the scratch paper labeled clearly.Concentration of the KSCN stock solution, M Volume of the KSCN stock solution, mL Initial molar concentration of SCN in a 50-ml flask, M PART A. Establishing the Beer's Law Coefficient: blank 0 0 solution 2 1.00×10-³ 2.00 solution 3 1.00×10-3 5.00 solution 4 1.00×10-³ 10.00 solution 5 1.00-10-3 15.00Standardization of 0.10 M HCl1. Take three (3) clean and properly labeled 250-mL Erlenmeyer flasks. Into the three flasks, weigh 0.1 g of the primary standard Na2CO3 to the nearest 0.1 mg. Record the weights of the primary standard.2. Add about 75.0 mL of boiled distilled water and swirl to dissolve the solids.3. Add 2 to 3 drops of phenolphthalein indicator. Record the initial burette reading and titrate with the prepared 0.10 M HCl solution until phenolphthalein endpoint.4. Record the final burette reading for each titration in your data sheetDetermination of Ksp and Molar Solubility1. Add Ca(OH)2 to 250.0 mL distilled water with stirring until equilibrium is achieved. 2. Filter the undissolved precipitate. Measure out 50.0 mL of the supernate into a 250-mL Erlenmeyer flask using a pipette.3. Add a few drops of phenolphthalein indicator and titrate with standardized HCl solution until endpoint is achieved.4. Record the volume the HCl solution used. Perform two more trials.…