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- You have a MASTER STOCK solution containing 1.000g of caffeine in 100mL of mobile phase solvent mixture (20% methanol / 80% water with a formic acid sodium formate buffer @ pH 3.4) You have a diluted STUDENT STOCK solution that contains 0.01g of caffeine in 100mL of mobile phase solvent mixture. You are asked to prepare 3 diluted concentrations: 1. 15 mL of student stock in 25 mL of mobile phase solvent. 2. 10 mL of student stock in 25 mL of mobile phase solvent. 3. 5 mL of student stock in 25 mL of mobile phase solvent. Calculate the concentration of caffeine (in mg/mL) for each dilution.What is the percentage purity of acetic acid if 2.6 grams required 32.5 ml of 0.994 N NaOH solution to reach the endpoint? Does it conform to USP requirements for acetic acid 3%-6%?Find the Ksp of distilled water with Mg(OH)2 as its salt (solubility:1.51121E-05 M) MgCO3 as its salt (solubility: 1.78E-06 M)
- What is the Qsp of a solution mixture Al(OH)3 formed from 10 mL 1.00M C6H5NH2 and 15 mL 0.10M Al(NO3)3?What is the minimum distribution constant that permits removal of 99% of a solute from 50.0 mL of water with two 25.0-mL extractions with toluene? five 10.0-mL extractions with toluene?bottle of Na2EDTA.2H2O is labeled with an assay of 100.5%, what is this implied? What is the result of heating to 100 ºC? How does the Eriochrome Black T indicator function?
- A 20.00-mL sample of a saturated Sr(OH)₂ solution requires 24.36 mL of a 0.0550 M HCl solution to reach the endpoint. What is the Ksp of Sr(OH)₂?Full acid, HOOC = CH-COOH is a biphatic acid and we will label it as H2M. Acid constant data for the two protonation phases of the acid: K H.M+H2O = H, 0++HM- HM +H2O = H, 0++M2– a1 = 1.3x10-2 K.2 = 5.9 x 10-7 Measure 0.1 ml of 0.100 M of malic acid with 0.100M NaOH and measure the H variability as a function of the added base volume. A. Calculate the PH value at the beginning of the titration. B. Calculate the pH value at the first equivalent point. C. Calculate the pH value at the second equivalent point. D. Draw the titration curve in the graph. Indicate in the graph titles and units for the axes.In how much volume of diluted sulfuric acid should you dissolve a multivitamin tablet of approximately 1700 mg of Vitamin C to back analyze 10.00 mL of that solution, with 25.00 mL of 0.01 M KIO3 and 0.04 M thiosulfate to use approximately 8-10 mL of titrant ? You have 25, 50, 150, 250 and 500 mL flasks.
- Transfer 3-4 drops or a pinch of the test compound (Acetanilide) to 3 ml of the solvents, 5% NaOH and 5% NaHCO3 Shake the mixture thoroughly. The time required for the solute to dissolve in the solvent should not be more than 2 minutes. Indicate with (+) or (-) if the test compound is soluble or insoluble in the solvent. What is the theoretical solubility of Acetanilide in 5% NaOH? _______ What is the theoretical solubility of Acetanilide in 5% NaHCO3? _______PLEASE SHOW STEP BY STEP HOW TO SOLVE You have a MASTER STOCK solution containing 1.000g of caffeine in 100mL of mobile phase solvent mixture (20% methanol / 80% water with a formic acid sodium formate buffer @ pH 3.4) You have a diluted STUDENT STOCK solution that contains 0.01g of caffeine in 100mL of mobile phase solvent mixture. You are asked to prepare 3 diluted concentrations: 1. 15 mL of student stock in 25 mL of mobile phase solvent. 2. 10 mL of student stock in 25 mL of mobile phase solvent. 3. 5 mL of student stock in 25 mL of mobile phase solvent. Calculate the concentration of caffeine (in mg/mL) for each dilution.The standardization of same titrant during the determination of BOD5 of water sample was done separately for Day 1 and Day 5. Upon standardization, it turned out that the concentration of the titrant in Day 1 is higher than the concentration of the same batch of titrant in Day 5. How would you explain this discrepancy? The water used to prepare the Na2S2O3 solution was not boiled resulting to proliferation of bacteria. Too much starch indicator was added in the conical flask. Sulfuric acid was added first before potassium iodide. There were bubbles at the tip of the burette during titration.