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Using Table 2.1, calculate the required amount (in g) of ammonium sulfate to bring the solution from 40% to 60% saturation.
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- 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.Concentration of AR Stock Solution (ppmppm) 21.22 Unrounded Rounded Concentration of AR Stock Solution (μMμM) 42.7461 42.7Stock iron(II) solution (200Ug mL-1 Fe) ferrous ammonium sulfate hexahydrate mass= 0.1437g, transfer it to a 100 ml beaker. add 15 ml approx of water and 15m1 'approx of dilute sulphuric acid (2M H2SO.). then transfer FeII to 100 ml flask makeup to the mark with water. calculate the moles of ferrous ammonium sulfate hexahydrate solution in unit ug/mL.
- Read the Limit Test for salicylic acid in aspirin below then answer the question below. Remember: Aspirin = acetyl salicylic acid (ASA), and salicylic acid = SA Limit Test for salicylic acid: Extract powdered Aspirin tablets (i.e., active + excipient) containing 0.4g acetylsalicylic acid (i.e., active) with 4 mL of 95% ethanol. Add water to give a final volume of 100.0 mL and mix. Transfer 50.0 mL of the filtrate to a Nessler Cylinder and add 1.0 mL of acidified ferric ammonium sulfate solution. Mix and allow to stand. Prepare the standard solution used for comparison as follows: To another Nessler Cylinder add 3.0 mL of freshly prepared 0.01% (wt/vol) salicylic acid, 2.0 mL of ethanol, 1.0 mL of acidified ferric ammonium sulfate solution and sufficient water to give a total volume of 51.0 mL. Mix. A violet colour produced by the sample should not be more intense than that of the standard, used for comparison. Example of "Limit" calculations: Based on the above limit test, the…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).I'm trying to calculate the amount of sucrose in Cola. volume=50mL mass = 54.2060 g Density= 1.0841 g/mL 1) Based on this information, how do I calculate the concentration of the cola solution? 2) The actual concentration of sucrose (given) in cola = 0.638613 M (moles/L). How do I calculate the molarity of sucrose in the solution based on the concentration from #1? What would be the percent error?
- To prepare the solution you would place the solute in a 50.0 ml volumetric flask, and then fill to the mark with water while mixing. This would give a total solution volume of 50.0 ml. The 5.0 solution needs to be diluted to make 10.0 ml of a 2.0% solution. What volume of 5.0% solution should be used? Please answer fast i give you upvote.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 Q5. If Ana determines the absorbance of an unknown tartrazine sample to be 0.662, what is the concentration of the sample in µM?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.
- 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.1. Which of the following is not a step in preparing a water sample container?a. All sample containers must be dark in colorb. The type of sample container and the level of cleaning required depend on the type of sample to be takenc. All sample containers must be thoroughly cleaned in the laboratory before sampling is carried outd. The number of containers prepared must always be in excess of what is needed, for quality assurance, quality control and reserves 2. The purpose of environmental sample analysis is..a. To determine the origin and concentration of chemicals in the environmentb. To determine the origin, concentration of chemicals and/or pollutants in the environmentc. To determine the concentration of a chemical in the environmentd. To determine the cause and concentration of pollutants in the environmentA student must prepare 5.000 L of 0.2500 M Na2CO3 (105.99 g/mol). Which is the bestprocedure for preparing this solution?a. Measure 132.5 g Na2CO3 and add 5.000 kg of H2O.b. Measure 5.300 g Na2CO3 and add 5.000 kg of H2O.c. Measure 5.300 g Na2CO3 and add H2O until the final homogeneous solution has a volumeof 7.00 L.d. Measure 132.5 g Na2CO3 and add H2O until the final homogeneous solution has avolume of 5.000 L.e. Measure 132.5 g Na2CO3 and add 7.000 L of H2O.