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- In the MgO experiment, you made a buffer solution by combining 57 mL of 17 M NH3 with 7.0 grams of NH4Cl (FW = 58.49) and then diluting to give a total volume of 100 mL. Calculate the pH of this buffer solution given the pKb for ammonia is 4.76.Volhard titration. A 30.00-mL solution of unknown I2 was treated with 50.00 mL of 0.365 0 M AgNO3. The precipitated AgI was filtered off, and the filtrate (plus Fe31) was titrated with 0.287 0 M KSCN. When 37.60 mL had been added, the solution turned red. How many milligrams of I2 were present in the original solution?The ksp for Ca3(PO4)2 is 2.07 x 10^-33 at 25°C. calculate the aqueous solubility of Ca3(PO4)2 in terms of the following: a. the molarity of ions produced in solution b. the mass of salt that dissolves in 100ml of water at 25°C.
- At the half-way point in the titration of a weak acid with a strong base the pH was measured as 5.16. What is the acidity constant and the pKa of the acid? What is the pH of the solution that is 0.025 M in the acid?25.00 mL aliquots of the solution in problem 1 are titrated with EDTA to the calmagite end point. A blank containing a small measured amount of Mg^2+ requires 2.12 mL of the EDTA to reach the end point. An aliquot to which the same amount of Mg^2+ is added requires 25.88 mL of the EDTA to reach the end point.Tris or tris(hydroxymethyl)aminomethane is an organic buffering reagent most often used in nucleic acid extractions. Tris (MW = 121.14 g/mol) has a pKa of 8.07 at 25oC, with a white crystalline powder appearance. What is the buffering range/s of Tris buffer? How would you prepare 500mL of a 0.200 M Tris buffer solution using Tris and NaTris or sodium Tris (MW = 143.14 g/mol)?
- Titration of 50.00 mL of 0.04715 M Na2C2O4 required 39.25 mL of a potassium permanganate solution. 2MnO4- + 5C2O4-2 +16H+ -> 2Mn2+ + 10CO2(g) + 8H2O Calculate the molar concentration of the KMnO4 solution What molecules would interfere with the titrimetric analysis?A 1.0 g sample containing urea was dissolved in water and diluted in a 100.00 mL volumetric flask. 20.00 mL aliquot was mixed with 30.00 mL water and subjected to digestion with concentrated H2SO4. The ammonia produced is collected in 30.00 mL of 0.0500 M HCl and the excess acid is back titrated with 0.0500 M NaOH, requiring 6.80 mL. Calculate the weight percent urea [(NH2)2CO, FW=60.06 g/mol] in the sample. Please use the factor label method in answering.A 1.0 g sample containing urea was dissolved in water and diluted in a 100.00 mL volumetric flask. 20.00 mL aliquot was mixed with 30.00 mL water and subjected to digestion with concentrated H2SO4. The ammonia produced is collected in 30.00 mL of 0.0500 M HCl and the excess acid is back titrated with 0.0500 M NaOH, requiring 6.80 mL. Calculate the weight percent urea [(NH2)2CO, FW=60.06 g/mol] in the sample.
- A 2.02.0 mL aliquot of 0.001 M NaSCNNaSCN is diluted to 30.030.0 mL with 0.2 M Fe(NO3)3Fe(NO3)3 and 0.1 M HNO3.HNO3. How many moles of SCN−SCN− are present? If all the SCN−SCN− is complexed with Fe3+Fe3+ to form FeSCN2+,FeSCN2+, what is the molar concentration of FeSCN2+?What is the mole ratio of sodium acetate to acetic acid (Ka=1.8 x 10^-5) in a buffer with the pH of 4.00? Report to 3 sig figs1. What is the molar solubility of PbCl2 in a solution of 0.23 M CaCl2? Ksp = 1.6 ✕ 10-5 for PbCl2. 2. What is the Qsp when 32.0 mL of 6.50 ✕ 10-7 M Na3PO4 are mixed with 41.4 mL of 5.50 ✕ 10-5 M CaCl2? Assume the volumes are additive. Ksp = 2.0 ✕ 10-29. 3. What is the Qsp when 61.0 mL of 1.50 ✕ 10-4 M AgNO3 are mixed with 80.0 mL of 5.20 ✕ 10-3 M CaCl2? Assume the volumes are additive. Ksp = 1.6 ✕ 10-10. 4. What [I-1] is needed to start the precipitation of AgI from a saturated solution of AgCl? Ksp = 2.9 ✕ 10-16 for AgI and Ksp = 1.2 ✕ 10-10 for AgCl.