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- Suppose titration of 100.00 mL mixture of 0.0500 M in Br + 0.08 M CI with 0.4000 M AgNO3. What is pAg at the second end point?In the titration of 50.00 mL 0.0200M weak base B using 0.0150 M HCI, which indicator is the best one to be used? (pK, of the weak base B is 10.50). Indicator 2: Methyl red: pH transition = 4.8-6.0 Indicator 1: Cresol purple: pH transition = 1.2-2.8 Indicator 4: Thymolthalein: pH transition = 8.5-10.5 O Indicator 5: Indigo Carmine: pH transition= 11.6- 14.0 O Indicator 3: Cresol red: pH transition = 7.2-8.8Calculate pFe+ at each of the points in the titration of 25.00 mL of 0.02190 M Fe+ by 0.03634 M EDTA at a pH of 7.00. The values for log Kr and aya. can be found in the chempendix. 10.50 mL pFe2+ the equivalence point, Ve pFe?+ 18.50 ml pFe?+ %3D
- In the titration of 50.00 mL 0.0200M weak base B using 0.0150 M HCI, which indicator is the best one to be used? (pK, of the weak base B is 10.50). Indicator 4: Thymolthalein: pH transition = 8.5-10.5 OIndicator 5: Indigo Carmine: pH transition= 11.6- 14.0 Indicator 3: Cresol red: pH transition 7.2-8.8 Indicator 1: Cresol purple: pH transition = 1.2-2.8 Indicator 2: Methyl red: pH transition = 4.8-6.0Plot the titration curve for titration of 50mL of 0.0150M Fe2+ solution buffered to pH's 7.0 with 0.03M EDTA. A-) OmL, B-) 10mL, C-) 25 mL, D-) Calculate the pFe after 26 mL of titrant additions. (Kr.Y= 2.1x10^14, a4=4.8x10^-4)Calculate pAg at each of the following points in the titration of 20.00 mL of 0.0500 M AgNO3 with 0.0250 M NH4SCN.Ksp AgSCN = 1.10 × 10-12 a. 0.00 mL NH4SCNb. 20.00 mL NH4SCNc. 40.00 mL NH4SCNd. 45.00 mL NH4SCNe. 50.00 mL NH4SCN
- 100.0 mL sample of drinking water was buffered with ammonia at pH 10 and after addition of EBT required 21.4 mL of 0.00512 M EDTA for titration. FW CaCO3 = 100.09 g/mol. What will be the change in color at the end point? What is the water hardness in terms of ppm CaCO3?. What is the role of ammonia buffer in the analysis?Calculate the following points on the titration curve for the reaction of 20.00 mL of 0.1075 M Pb4+ with 0.1250 M Cu+. The analytical reaction is Pb4+ + 2Cu+ ⇋ Pb2+ + 2Cu2+ and Pb4+ + 2e− ⇋ Pb2+ E° = 1.690 V Cu2+ + e− ⇋ Cu+ E° = 0.161 V After the addition of 17.20 mL of 0.1250 M Cu+. After the addition of 34.40 mL of 0.1250 M Cu+. What is the equilibrium constant for the reaction between Pb4+ and Cu+?Calculate pFe2+ at each of the points in the titration of 25.00 mL of 0.02233 M Fe2+ by 0.03516 M EDTA at a pH of 5.00. The values for log Kf and ays- can be found in the chempendix. 11.00 mL pFe2+ 2.322 %3D the equivalence point, Ve pFe2+ 4.81 %3D 8.5756 19.50 mL pFe2+ Incorrect
- Calculate the silver ion concentration in terms of pAg during the titration of 70.00 mL of 0.07000 M NaCl with 0.1000 M AgNO3 after the addition of the following volumes of reagent: (a) in the preequivalence point region at 20.00 mL, (b) at the equivalence point (25.00 mL), (c) after the equivalence point at 50.00 mL. For AgCl, Ksp = 1.82E10-10. Show your answer with three significant figures.The titration of 50.0mL of 0.100M HC2H3O2 (Ka3D1.8 x 10-5) with 0.100M NAOH. The pH of the solution at the Equivalence Point will be *Titration of 0.2121 g of primary standard Na,C,0, (133.999 g/mol) required 21.66 mL of KIMnO, (158.034 g/mol) to reach the end point. Calculate the molar concentration of KMNO,? 2 MnO, +5 C20,2 + 16 H+ 2 Mn2+ 10 CO2 +8 H20 1. 000146 2. O0.0292 3. 00.00731 4. 00.1462