You have a test tube containing a mixture of Ag+, Fe3+, and Ba2+ . Make a diagram to separate the given mixture of cations. Include the correct reagents to be used to effectively isolate cations from each other.
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You have a test tube containing a mixture of Ag+, Fe3+, and Ba2+ . Make a diagram to separate the given mixture of cations. Include the correct reagents to be used to effectively isolate cations from each other.
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- You are given a solution that contains a mixture of the following cations: Ag+, Ba2+, Mn2+ and Cu2+. Draw a flow chart to show how these cations are separated and indicate specific reagents used in each separation step.A piece of magnesium metal was reacted with each of the following acids: 3 M HCl, 3 M acetic acid (Ka=1.8 • 10-5) and 3 M HF (Ka=6.8•10-4). Rank this acids in decreasing order of reactivity. Explain as well.You are asked to prepare a buffer for an experiment. You have access to the following dolutions of acid/base pairs: 1. Propanic Acid (CH3CH2COOH) / Sodium Propanoate (NaCH3CH2COO) with Ka = 1.4 x 10^-5 2. Potassium Hydrogensulfite (KHSO3) / Potassium Sulfite (K2SO3) with Ka = 6.2 x 10^-8 3. Chloroacetic acid (CH2ClCOOH) / Sodium Chlocoacetate (NaCH2ClCOOO) with Ka = 1.4 x 10^-2 Your buffer needs to be at a pH of 4.5. Which acid/base pair do you choose and why? Be very specific!
- What weight of sample must be taken so that each 50 mg BaCl2 obtained in a gravimetric silver determination shall correspond to 10% of the Cl in the original sample? BaCl2 (208.23) Cl (35.45)Standard solution : 0.201 grams of acetylsalicylic acid was combined with 10 mL of 0.5 M NaOH, then transfered to a 100 mL flask and filled the rest of the way with water Then 0.500 mLs of the standard solution was transfered to a 10.00 mL flask and diluted to the 10 mL mark with 0.02 M of buffered iron chloride. This step was repeated using 0.400, 0.300, 0.200, 0.100 mLs of the standard solution Questions: A.) determine the concentration of the acetylsalicylic acid in the 100.00 mL volumetric flask containing the solution from which the standards were made. B.)determine the concentration of the acetylsalicylic acid in each of the 10.00 mL calibration solutions. I only need the work for 0.400 mLs C.)Make a scatter plot (on the computer again) of absorbance versus concentration for the calibration samples. On the plot, add a linear trendline, and display the equation and the R2 value on the chart. Take your time to label the axesWhat is the role of Glycerin in the assay of Boric Acid?I. The reagent prevents the formation of pink color earlier than the expected endpoint.II. The reagent allows the reaction of protons from the acid sample with the hydroxyl ions from the titrant.III. It enhances the water solubility of the difficultly soluble boric acid. a. I, II & III b. II & III c. I & II d. I only e. I & III
- All of the following criteria must be met for a titrimetric analysis to be feasible EXCEPT: Select one: a. Reaction between the standard and analyte must be known. b. There should be a substance for endpoint detection c. Reaction must proceed quantitatively to completion. d. Reaction between the reactants must be slow.What is the pH of 0.150M of Na2HPO4? How to determine 1st or 2nd intermediate? ka1 7.11*10-3 ka2 6.34*10-8 ka3 4.22*10-13In the titration of 25.00 mL of a water sample, it took 19.990 mL of 3.480x 10−3 M EDTA solution to reach the endpoint. Calculate the number of moles of EDTA required to titrate the water sample. (enter your answer with 3 significant figures) The total hardness is due to one or a combination of Ca2+, Mg2+, and Fe2+ in your sample. It is convenient to express this hardness as though it was entirely due to Ca2+. Making this assumption, determine the number of moles of Ca2+ present in the bottled water sample titrated. (enter your answer with 3 significant figures) The total hardness is always listed in parts-per-million (ppm) of CaCO3 (or mg CaCO3 / Kg H2O). Since the density of water is 1.0 g/mL, one ppm would be the same as the number of mg of CaCO3 per liter of water. Determine the number of moles of CaCO3 present in the titrated sample of water, assuming that all the Ca2+ combines with CO32−. (enter your answer with 3 significant figures) Calculate the number of grams of…
- Asking for lab help Fe3+ (aq) + SCN- (aq) = FeSCN2+ (aq) + heat pale yellow redWe have a solution at equilibrium after mixing 10 drops of 0.10M FeCl3 (aq), 10 drops 0.10M KSCN (aq), and then adding enough deionized water to bring the whole thing up to 25mL. We then added 2mL of that solution to a test tube. If I add 2.0mL of deionized water to that test tube, following Le Chateiler's Principles, how should the equilibrium be expected to change? Please give a detailed explination as to why.In the titration of 25.00 mL of a water sample, it took 20.690 mL of 4.050x 10−3 M EDTA solution to reach the endpoint. Calculate the number of moles of EDTA required to titrate the water sample. (enter your answer with 3 significant figures) The total hardness is due to one or a combination of Ca2+, Mg2+, and Fe2+ in your sample. It is convenient to express this hardness as though it was entirely due to Ca2+. Making this assumption, determine the number of moles of Ca2+ present in the bottled water sample titrated. The total hardness is always listed in parts-per-million (ppm) of CaCO3 (or mg CaCO3 / Kg H2O). Since the density of water is 1.0 g/mL, one ppm would be the same as the number of mg of CaCO3 per liter of water. Determine the number of moles of CaCO3 present in the titrated sample of water, assuming that all the Ca2+ combines with CO32−. Calculate the number of grams of CaCO3 present and convert to mg. Calculate the ppm of CaCO3 = mg CaCO3 / Liters H2O used. (enter…Determine the pH of (a) a 0.40 M CH3COOH solution and (b) a solution that is 0.40 M CH3COOH and 0.20 M CH3 Ka for CH3COOH = 1.8 X 10-5. Could you have predicted that the pH would rise after addition of sodium acetate to pure 0.40 M acetic acid from part (a) by applying Le Chatelier’s principle?
