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A 10.0-mL solution of 0.050 0 M AgNO3 was titrated with 0.025 0 M NaBr in the cell
S.C.E. || titration solution | Ag(s)
Find the cell voltage for 0.1 and 30.0 mL of titrant.
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- A 0.3285 g sample containing chloride and inert material is titrated with 0.1012 M AgNO3, requiring 34.99 mL to reach the Ag,Cro. end point. Titration of a blank sample consumes 0.32 mL of the AgNO, titrant. Determine the % w/w chloride in the sample.Determine the % w/w chloride in the sample. A 0.3285 g sample containing chloride and inert material is titrated with 0.1012 M AgNO3, requiring 34.99 mL to reach the Ag2CrO4 end point. Titration of a blank sample consumes 0.32 mL of the AgNO3 titrant.A student wanted to determine the amount of NaOCI in a commercial bleaching solution. He diluted 2 g of bleach in a 100 ml volumetric flask. A 50 ml sample of the diluted bleach was mixed with excess acidified potassium iodide KI and a few drops of an indicator. The resulting solution was titrated with Na-S.O, solution. The titration required 17 mL of 0.05M Na,S,O, solution. The series of reactions that take place during this experiment: 21+OCI+ 2H1₂ + Cl + H₂O 1₂+28,0,³ →21+S,0,² a) Calculate the number of moles of OCI- in 50 mL diluted bleach and in 100 mL.
- - 144 / Natural Sciences / Chemistry And Polymer Science / Chemi zzes / Buffers en Titrasies | Buffers and Titrations A 0.386 g sample of propanoic acid (CH3CH,COOH, K, = 1.3. x 10-5) was dissolved to a final volume of 50.0 cm, This solution underwent titration with 0.32 M NaOH. Calculate the pH of solution at the equivalence point. %3D fi h- Bi ek Please give the answer to 2 decimal places. Ge pl Answer: Check1. Commercial vinegar was titrated with NaOH solution to determine the content of acetic acid, CH3COOH. For 20.0 cm3 of the vinegar, 26.7 cm3of 0.60 mol dm-3 NaOH solution was required.What was the concentration of acetic acid in the vinegar if no other acid was present? (Thanks for your help) A. 0.45 mol dm-3B. 0.60 mol dm-3C. 0.80 mol dm-3D. 1.60 mol dm-35. Titration of 50.00 mL of 0.02502 M Na2C2O4 required 34.75 mL of a potassium permanganate solution. 2MNO4 ¨+ 5H2C2O4 + 6H* → 2Mn²*+ 10CO2(g) + 8H2O Calculate the molar concentration of the KMNO4 solution.
- A 10.00 mL sample containing 8.00 g/L of a mixture of KCI and NaCl was titrated with 0.10 M standard solution of AgNO3; where 5.6 mL was needed to reach the end-point. Calculate the mass of sample (in grams). 1. O0.0033 2. O0.0800 3. O0.0083 4. O0.0337A 10.0 mL solution of 0.050 M AgNO3 was titrated with 0.0250 M NaBr in the cell: S.C.E || titration solution | Ag(s) Find the cell voltage for 30.0 mL of titrant. (A) +0.093 V (B) -0.039 V (C) -0.093 V (D) +0.039 V12. Collect a sample of lake water; a) 100 mL titrate with 0.05N HCI to HCO3 eq.pt. and we need to add 0.5 mL of acid solution. What is the CO3 ALK as M and mg CaCO3/L? b) 100 mL titrate with 0.03N NaOH to CO; eq.pt. and we need to add 0.6 mL of base solution. What is the OH ALK as M and mg CaCO3/L? c) What is the Cr and pH value?
- The phosphate in a 3.000 g sample of industrial detergent was precipitated by the addition of 1.000 g of AgNO3. The solution was filtered and the filtrate required 18.23 mL of 0.1377 M KSCN for titration to the FeSCN2+ end point. Calculate the percentage of phosphate in the detergent.4) A redox titration: 20.00 mL of 0.00500 M Sn²+ solution was titrated with 0.0200 M Ce+*+ according to the reactio below. Titration reaction: Burst coreaning Co Ce4+ + e-------> Ce³+ Sn²+ + 2e ------> Sn²+ appy 0.00500 M Sn Calomal Pt wire Magneto stirring bar 2 Ce4+ + Sn²+ --> 2 Ce³+ + Sn¹+ Eº 1.470 V 0.139 V a) What is VE (the equivalence volume) (of Ce4+) needed to reach the endpoint? b) Calculate the potential (voltage) relative to SCE, when 5.00 mL Ce4+ is added. SCE = +0.241 VA solution of HClO4 was standardized by dissolving 0.4008 g of primary-standardgrade HgO in a solution of KBr: HgO(s) + 4Br- + H2O --> HgBr42- + 2OH-. The liberated OH- consumed 43.75 mL of the acid. Calculate the molar concentration of the HClO4.