Experiment 1 E Data Table 1 EData Table 2 Exercise 1 Data Table 1: NaOH Titration Volume Initial NaOH Volume (mL) Final NaOH Volume (mL) Total Volume of NaOH Used (mL) Trial 8.9 0.1 8.8 Trial 9.1 0.1 9 Trial 6.9 6.9 Average Volume of NaOH Used (mL):
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- BSA for concentration measurements is often prepared as a 10 mg/mL stock solution. Suppose you wish to prepare a series of 10 mL solutions of BSA at 1.0, 0.8, 0.6, 0.4, and 0.2 mg/mL. Using the dilution equation C1 × V1 = C2 × V2, you plan to do this by transferring a calculated volume (V1) of the 10 mg/mL (C1) into a clean test tube, then adding water in sufficient volume to produce 10 mL (V2) at the desired concentration (C2). Complete the table below, showing the volume of stock 10 mg/mL solution you need to add to each tube, and the volume of water you need to add to each. Also, convert the desired mg/mL concentration values to their equivalent in μM (micromolar; 10-6 M).A solution of HNO3HNO3 is standardized by reaction with pure sodium carbonate. 2H++Na2CO3⟶2Na++H2O+CO22H++Na2CO3⟶2Na++H2O+CO2 A volume of 24.78±0.06 mL24.78±0.06 mL of HNO3HNO3 solution was required for complete reaction with 0.8272±0.0007 g0.8272±0.0007 g of Na2CO3Na2CO3, (FM 105.988±0.001 g/mol105.988±0.001 g/mol). Find the molarity of the HNO3HNO3 solution and its absolute uncertainty.Sucrose solution for experiment 1: (Question a-c)Prepare a solution of sucrose by accurately weighing 9.0 – 9.25 g of sucrose into a 100mLbeaker / conical flask. Record the mass of the sample. Add 25 mL distilled water. Mix until allcrystals dissolve.NaCl solution for experiment 2: (Question d-f)Prepare a solution of NaCl by accurately weighing approximately 1.5 g of NaCl into a 100 mLbeaker / conical flask. Record the mass of the sample. Add 25 mL distilled water. Mix until allcrystals dissolve.MgCl2٠6H2O solution for experiment 2: (Question d-f)Prepare a solution of magnesium chloride by accurately weighing approximately 3.6 g ofMgCl2٠6H20 into a 100 mL beaker / conical flask. Record the mass of the sample. Add 25 mLdistilled water. Mix until all the crystals dissolve
- A sample consisting entirely of pure Li2CO3 and pure BaCO3 weighs 1.000 g and requires 30.00 mL of 0.5000 N HCl for neutralization. Calculate the number of grams of Li2CO3 in the sample. (Note: Use the least significant digits in your answer.)An environmental scientist obtained the following replicate concentration measurements of methane (CH4) gas at a landfill site: Replicate Measurements CH4 Concentration (mg/m3) 1.0 0.1571 2.2 0.2031 3.0 0.1914 4.0 0.2103 Calculate % error when the scientific community accepts 0.2102 as true value.If 25.0 mL of a 3.00 M HCl stock solution are diluted with water to a final volume of 5.00 L, what will be the final concentration of HCl in the dilute solution? Report your result in decimal notation and to the proper number of significant figures. All numbers are measured. a) 0.600 M b) 0.120 M c) 1.50 M d) 0.0150 M e) 0.300 M
- I have 6 tubes with the contents labeled. How can I make a 20% concentration serial dilution? Please show the steps and the final dilutions for the tubes as a fraction.As part of the aspirin synthesis lab the orgo students also had to perform the following calculation to demonstrate their knowledge. Are you able to help them work this out? Saponification is a process in which soap is produced from the chemical reaction between animal fat (triglycerides) and a strong base such as KOH. An example of such balanced chemical reaction is shown here: C51H98O6 + 3KOH → C3H5(OH)3 + 3C16H31O2K (Triglyceride) (Soap) if during the saponification reaction 231.5 g of C51H98O6 is mixed with 231.5 g of KOH and 160 g of soap is produced. Calculate the theoretical yield of soap C16H31O2K and indicate who is the limiting reactant. (Provide your answer to 2 decimal places) Calculate the percent yield for this reaction (Provide your answer to 1 decimal place) *Show ALL steps and mathematical equations involved in your calculations to help the orgo students. Remember to label all…For the following questions (Q1-Q5), consider the compound tartrazine (Yellow 5 food dye) that has a chemical formula of C16H9N4Na3O9S2. Ana weighs out 0.1328 g of tartrazine powder on the balance for her experiment and makes a stock solution by dissolving her powder in 500.0 mL of solution. Concentration (µM or µmol/L) Absorbance 0.00 0.001 9.94 0.252 19.9 0.506 29.8 0.738 39.8 1.018 slope (m): 0.02534 1/(µM) y-intercept (b): -0.0009147 Q4. Calculate the molar extinction coefficient (molar absorptivity) of tartrazine in units of 1/(M·cm). Assume a cuvette path length of 1.00 cm.
- Obtain values from the pictures found in the procedure to complete the data table below.Remember to include units!A. Data:1 Mass empty beaker2 Mass beaker + Na2CO33 Mass Na2CO3 used4 Mass graduated cylinder + HCl(aq)5 Mass empty graduated cylinder6 Mass HCl(aq) used7 Total mass before rxn: beaker + Na2CO3 + HCl(aq)8 Mass beaker + salt solution after reaction9 Mass of CO2 generated by the reaction10 Mass of beaker + NaCl (after drying)11 Mass of NaCl GeneratedK2CO3 (aq)+ CaCl2 (aq)→ CaCO3 (s) + 2KCl (aq) Data Sheet Table 1: Data and Observations Material Mass CaCl2 2.0g K2CO3 2.5g Filter Paper 1.6g Watch Glass 35.8g Filter Paper + Watch Glass + Precipitate 38.9 Precipitate 1.5g Table 2: Mass of CaCl2 after 24 Hours Initial Observations 24 hour Observation Weigh Boat Mass of Weigh Boat 0.5g Mass of Weigh Boat 0.5g CaCl2 2.0g Mass of CaCl2 2.4g Mass of CaCl2 Calculate the theoretical yield of the solid precipitate. Then use that to calculate the percent yield of the solid precipitate.For questions 48-55, please refer to the following: In order to form Ba(IO3)2, 500 mL of 0.5000 M Ba(NO3)2 was mixed with 500 mL of 0.0500 M NaIO3. Ksp= 1.57x10^-9 1. How many millimoles of Ba(NO3)2 are there in the solution? 2. How many millimoles of NaIO3 are there in the solution?