4) A redox titration: 20.00 mL of 0.00500 M Sn²+ solution below. Titration reaction: Bucony C Ce+ + e-------> Ce³+ Sn + 2e-> Sn²+ 0.00500 M Sa was titrated with 0.0200 M Ce according to the reactio Cod unce de P Magre 2 Ce+ + Sn²+> 2 Ce³+ + Sn¹+ Eº 1.470 V 0.139 V a) What is VE (the equivalence volume) (of Ce**) needed to reach the endpoint? b) Calculate the potential (voltage) relative to SCE, when 5.00 mL Ce+ is added. SCE = +0.241 V
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- A 1.000-g sample containing KHC2O4, H2C2O4, and impurities required 38.22 mL of 0.1000 M NaOH for acid-base titration. Another 1.000-g sample required 27.02 mLof 0.04000 M KMnO4 for redox titration in acid solution, according to the following reaction: MnO4- + 5C2O42- + 16H+ ⇄ 2Mn2+ + 10CO2 + 8H2O How many mmols of KHC2O4 are there in the sample?The amount of copper in a wire was determined by a redox titration using KMnO4 as the titrant. A 0.4185-g sample was dissolved in acid and the liberated Cu2+ quantitatively reduced to Cu+, using a reductor column. Titrating with 0.0250 M KMnO4 requires 41.27 mL to reach the endpoint. Determine the % w/w CuO in the sample of meteorite. Answer: % CuO =The solubility of borax, which is made up of sodium tetraborate (Na2B4O5(OH)4 8H2O), was analyzed. The dissolution of borax is: Na2B4O5(OH)4 • 8H2O(s) ⇌ 2 Na+(aq) + B4O5(OH)42–(aq) + 8 H2O(l) A 50 mL saturated solution was prepared. After filtration of solution, 5 mL aliquot was transferred to a flask and titrated using 0.432 M HCl. The endpoint was found to be 4.73 mL of the titrant. Tetraborate anion (B4O5(OH)42-) is a weak base which reacts with HCl like the following reaction: B4O5(OH)42–(aq) + 2 H+(aq) + 3 H2O(l) ⇌ 4 H3BO3(aq) What is Ksp expression for the dissolution? What is the tetraborate ions concentration in the filtrate? What is the molar solubility and Ksp of borax if the titration was done at room temperature (298 K)?
- A potentiometric titration was done using a solution containing 200 mL of water, 20 mL of 3 M sulfuric acid, 5 mL of concentrated phosphoric acid and 10.00 mL of 0.5964 N K2Cr2O7. The amount of titrant added was 19.24 mL of 0.3355 N Fe2+ solution. [H+] = 1.41 x 10-3 M during the titration. Find the concentrations of all species relevant to the redox chemistry present in solution at this point in the titration.calculate the mass of Sn when 50 mL of a sample containing Sn2+ is titrated with 42.00 mL of 0.0150M MnO4- to reach endpoint3I- + OCl- + 2H+ ----> I3- + Cl- + H2: A 25.00 ml sample of liquid bleach was diluted to 1000 ml in a graduated flask. A 25 ml portion of the diluted sample was pipetted into an Erlenmeyer flask and treated with excess KI to oxidize OCl- to Cl- and I3- was produced at the end of the reaction. The released I3 was titrated with 0.09892 M Na2S2O3 and 8.96 ml was spent to reach the turning point besides the starch indicator. What is the percent by weight/volume of NaOCl in the bleach sample? (NaOCl:74.44 g/mol)
- A 1.963-g sample of an alloy is dissolved in HNO3 and diluted to volume in a 100-mL volumetric flask. Titrating a 25.00-mL portion with 0.1078 M KSCN requires 27.19 mL to reach the end point. What is the %w/w Ag in the alloy?A 20 ml aliquot of malonic acid solution was treated with 10.0 ml of 0.25M Ce4+ leading to the reaction CH2(COOH)2 + 6Ce4+ + 2H2O ® HCOOH + 2CO2 + 6Ce3+ + 6H+ After standing for 10 minutes at 60oC, the solution was cooled and the x’ss Ce4+ was titrated with 0.1M Fe2+, requiring 14.4 ml to reach the ferroin end point. Calculate the M of the malonic in the sample.a) What mass of Fe(NH4)2(SO4)2•2H2O(s) is required to prepare a 500 mL solution containing 100 ppm (m:v) in Fe? b) Using this stock solution, what aliquot must be used to prepare calibration solutions, 100 mL volume, of the following concentrations: 0.100 ppm, 0.500 ppm, 2.00 ppm, 4.00 ppm, and 7.00 ppm.
- 1. 1093-g sample of impure Na2CO3 was analyzed by residual precipitimetry. After adding 50.00 mL of 0.06911 M AgNO3, the sample was back-titrated with 0.05781 M KSCN, requiring 27.36 mL to reach the endpoint. The percentage Na2CO3 (MW = 106.0 g/mole) in the tested sample is ________ % ? Note: Express final answer using least number of significant figures. 2. The alkalinity of natural waters is usually controlled by OH- (MW = 17.01 g/mole), CO3-2 (MW = 60.01 g/mole), and HCO3- (MW = 61.01 g/mole), which may be present singularly or in combination. Titrating a 10.0-mL sample to a phenolphthalein endpoint requires 38.12 mL of a 0.5812 M solution of HCl, and an additional 18.67 mL of the same titrant to reach the methyl orange endpoint. The composition of the sample is _________% CO3-2 and ___________ % OH- Note: Express final answers using least number of significant figures.The arsenic in a 1.010 g sample of a pesticide was converted to H3AsO4 by suitable treatment. The acid was then neutralized, and exactly 40.00 mL of 0.06222M AgNO3 was added to precipitate the arsenic quantitatively as Ag3AsO4. The excess Ag in the filtrate and in the washings from theprecipitate was titrated with 10.76 mL of 0.1000MKSCN; the reaction wasAg+ + SCN-→ AgSCN(s) Calculate the percent AsO3 in the sample.Using basic conditions, MnO4- can be used as titrant for the analysis of Mn2+, with both the analyte and the titrant ending up as MnO2. In the analysis of a mineral sample for manganese, a 0.5165-g sample is dissolved, and the manganese is reduced to Mn2+. The solution is made basic and titrated with 0.03358 M KMnO4, requiring 34.88 mL to reach the endpoint. Calculate the %w/w Mn in the mineral sample. Answer: % Mn =