You should determine how you will make the following solutions: 1- 0.8 M NAOH + 20 mM EDTA: Make 250 ml from solid NaOH and 0.5 M EDTA 2- Make 500 mL each of 6x SSC and 2x SSC from 20x SSc 3- TBS-T (This is 1x TBS (or Tris buffered saline) buffer with 0.1% Tween-20). We have a 10x TBS solution in the lab and a bottle of Tween-20. Make 1L of 1x TBS with 0.1% Tween-20. 4- Blocking buffer. Should be made fresh each time. Mix 2.5 g of non-fat dry milk powder with 50 mL 1x TBS-T
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- Bay Water Titration The concentration of Cl- in ocean water is about 500-600 mM. The baywater is diluted by a factor of 12.5 using a 20.00 mL volumetric pipet and a 250 mL volumetric flask. Using a 15.00 mL volumetric pipet, 15.00 mL is transferred into three clean Erlenmeyer flasks. 10 mL of 1% dextrin solution, 20 mL of de-ionized water, and 3-4 drops of indicator are added and titrated each with the AgNO3 solution. From the procedure, find: Dilution factor Volume of diluted bay water Then calculate: The [Cl-] of diluted bay water The [Cl-] of bay water Consider this information: [AgNO3] = 0.04043177 trial # Veq 1 13.91 2 13.73 3 13.9 4 13.86 5 13.87 6 13.84 average 13.85167 [Cl-]Bay = ([AgNO3](Veq(ave))/Vdil bay water pipeted) (Vflask/Vbay water)In the conductivity test, _____________________ is going to result to a brightly lit light bulb. a. 70% v/v ethanol b. 1.0 M citric acid c. Mixture of 10.0 mL 1.0 M Mg(OH)2 and 10.0 mL 1.0 M HNO3 d. Glacial acetic acidHow much amount (in grams) do you need to prepare the following solutions 500.0 mL 0.1000 M stock EDTA solution from Na2H2EDTA•2H2O (FW=372.24) and MgCl2•6H2O crystals 100.0 mL 0.0500 M stock Ca2+ solution from pure CaCO3 (FW=100.09) and concentrated HCl 250 mL 1.0 M NH3-NH4+ pH 10 buffer solution from NH4Cl and NH3
- Determine the total hardness of water (ppm CaCO3; MM: 100.09 g/mole) if 100.0mL sample of drinking water required 38.41mL of 4.65 x 10-3 M EDTA for titration. 179 ppm CaCO3 357 ppm CaCO3 452 ppm CaCO3 733 ppm CaCO30.15 gm of calcium carbonate is dissolved in 1 liter of distilled water. 20 ml of this standard hard water requires 25 ml of EDTA solution. 100 ml of unknown hard water requires 18 ml of EDTA solution. The same water sample after boiling requires 12 ml of EDTA solution. Calculate Temporary hardness of water sample in ppm.Procedure Preparation of Dilute Solution of Vinegar • Using a 10 mL pipette, transfer 10mL of vinegar into 100 mL volumetric flask. • Dilute to mark of the volumetric flask using distilled water. B. Titration of Diluted Solution of Vinegar • Transfer 25 mL of diluted solution to 250 mL Erlenmeyer flask. • Add 0.5 mL phenolphthalein indicator. Set aside. • Transfer 50mL of 0.110 M NaOH into a 50 mL burette. • Titrate the diluted solution until the phenolphthalein endpoint (very faint pink). • Record volume of NaOH used. Answer the question: What is the experimentally determined concentration of acetic acid in your vinegar solution: (Please give your answer to three significant figures.) ______ M Acetic Acid
- Make oleic acid vesicles by making a solution of 0.5mL of 50mM oleic acid, 1 mM HPTS in 0.2 M Tris-HCl, 50 mM NaCl, pH 8.5 (i.e. buffer A) in a microcentrifuge tube in the following order. How much HPTS should you add? How much oleic acid?Make 50 ml of the extraction buffer containing the following ingredients using the stock solution you made (1M Tris-HCl, 5 M NaCl, 0.5 M EDTA, and 10% SDS). You add each solution into one sterile tube using sterile pipets and add an appropriate amount of sterile ddH2O to make it 50 ml. Include the amount of sterile ddH2O. Extraction buffer composition: 200 mM Tris-HCl (pH 8.0) 2 M NaCl 25 mM EDTA (pH 8.0) 1% SDSPrepare 100.00 mL of a solution with ALL the following chemicals into together; CHEMICALS PROVIDED solid FeCl3 6H2O, iron(II) chloride hexahydrate (source of FeCl3) dilute hydrochloric acid in the rack – 3.0 M solid sodium salicylate – 99.7% assay Concentrations needed in the 100mL solution FeCl3: 0.020 M HCl: 0.050 M Salicylate (mg/L): 40.25 PLEASE SHOW HOW TO CALUATE AND WORK. The only equations you will need to use are the equations for molarity and dilutions.
- Accurately weigh out about 6g copper(ii) sulfate crystals into a weighing boat. Use the copper(ii) sulfate crystals to make up 250cm3 of standardized copper (ii) sulfate solution Pipette 25cm3 of this solution into a conical flask Add 1.5g potassium iodide and swirl thoroughly Titrate this solution with standard 0.1 moldm-3 Na2S2O3 in a burette. When the iodine color fades, add 1 cm3 starch indicator. Use your titration data below to calculate the percentage by mass of copper in the copper(ii) sulfate crystals.An unknown sample of Cu2+gave an absorbance of 0.262. Then 1.00 mL of solution containing 100 ppm (ug/mL)Cu2+was mixed with 95.0 mL of the unknown and the mixture was diluted to 100 mL in a volumetric flask with deionized water. The absorbanceof the new solution was 0.500. a.Denoting the initial unknown concentrationas [Cu2+]i,write an expression for the final concentrationafter dilution [Cu2+] b.Find [Cu2+]in the unknown.1) 100 mL tap water is titrated with 20 mL of 0.02 M EDTA solution to determine the hardness of the water. The second 100 mL tap water is precipitated as CaC2O4 and removed by filtration and the filtrate is titrated with 8.0 mL of the same EDTA solution. What are the concentrations (as ppm) of Ca2+ (40.078 g/mol) and Mg2+ (24.305 g/mol) ions in the water? 2) 10 g of a solution, containing one or more of NaOH, Na3PO4, Na2HPO4, NaH2PO4, H3PO4 and HCl substances, is titrated with 1.0 M NaOH using the phenolphthalein indicator and 34.5 mL NaOH is used. Another 10 g mixture was titrated to reach the bromocresol green end point and 20.50 mL NaOH is used. What is the composition of the solution? What are the percentages of the species(H:1.0078, O:15.99, Na: 22.98, P:30.974, Cl:35.453)?