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- Cerium(IV) is a strong oxidizing agent commonly used in redox titrations. Which of the following statemnt is/are NOT true for cerium(IV)? I.A Ce** standard solution is prepared using primary-standard-grade ammonium hexanitratocerate(IV), (NH4)2Ce(NO3); dissolved in hot hydrochloric acid solution. II. Ce** is yellow and Ce3* is colorless. The color change is abrupt enough that Ce** can serve as its own indicator. III. Ce**/Ce* exists in different formal potential in different acids due to the interaction of the anions part of the acid with Ce** IV. Analysis of many organic analyte such as alcohol, aldehydes can be determined using Ce**by an indirect method involving a technique of back titration of unreacted excess Ce*with standard iron Il titrant O a. 1,11,IV O b. 1, II, III O. I,II O d. II, II, IV O e. I, II, III, IVMatch the chemical equation with its correct reaction type. 2 NaCl + [ Choose Pb(NO3)2 --> PbC12 + 2 NaNO3 Fe + Cu(NO3)2 [ Choose Fe(NO3)2 + --> Cu CH4 + 2 02 --> [ Choose v CO2 + 2 H2O 3 H2 + N2 --> 2 [ Choose v NH3 2 NaHCO3 --> [ Choose v H2O + Na2C03 + CO2Balance the following equations : K«Fe(CN)6+ H2SO4+ H2O а. ►K2SO4 + FESO4 + (NH4)2SO4 + CO b. CUSO4.5H2O →CUSO4+ H2O Al(OH)3 + CUSO4 → Al:(SO4 )3+ Cu(OH)2 с.
- 1. A 0.9882 gram sample of iron ore is dissolved, the iron reduced to Fe2+, and the solution was titrated with 36.40 mL of 0.02065 M KMnO4 in acid solution. (a) Write the titration reaction. (b) Calculate the %FeO (M.M. = 71.85) in the sample. 2. A sample of primary standard grade K2Cr2O7 (MM = 294.20) weighing 0.2153 g is dissolved, the solution acidified and excess KI added. The liberated I2 requires 44.86 mL of the Na2S2O3 for titration. (a) Write the titration reaction. (b) Calculate the molarity of the titrant solution.1. A 0.9882 gram sample of iron ore is dissolved, the iron reduced to Fe2+, and the solution was titrated with 36.40 mL of 0.02065 M KMnO4 in acid solution. (a) Write the titration reaction. (b) Calculate the %FeO (M.M. = 71.85) in the sample. 2. A sample of primary standard grade K2Cr2O7 (MM = 294.20) weighing 0.2153 g is dissolved, the solution acidified and excess KI added. The liberated I2 requires 44.86 mL of the Na2S2O3 for titration. (a) Write the titration reaction. (b) Calculate the molarity of the titrant solution. Box the final answer.An ore containing magnetite, Fe3O4, was analyzed by dissolving a 1.5419-g sample in concentrated HCl, giving a mixture of Fe2+ and Fe³+. After adding HNO3 to oxidize any Fe²+ to Fe³+, the resulting solution was diluted with water and the Fe³+ precipitated as Fe(OH)3 by adding NH3. After filtering and rinsing, the residue was ignited, giving 0.8525 g of pure Fe₂O3. Calculate the %w/w Fe3O4 in the sample.
- An ore containing magnetite, Fe3O4 was analyzed by dissolving a 1.5419 g sample in concentrated HCl, giving a mixture of Fe2+ and Fe3+. After adding HNO3 to oxidize any Fe2+ to Fe3+, the resulting solution was diluted with water and the Fe3+ precipitated as Fe(OH)3 by adding NH3. After filtering and rinsing, the residue was ignited, giving 0.8525 g of pure Fe2O3. Calculate the %w/w Fe3O4 in the sample.A 0.6599-g sample of impure magnesite, MgCO3 (MW = 84 g/mole), was decomposed with HCl; the liberated CO2 (MW = 44 g/mole) was collected on absorbent and found to weigh 0.1673-g. Calculate the percentage of magnesium (MW = 24 g/mole) in the sample. MgCO3 (s) + 2 HCl (aq) →MgCl2 (aq) + CO2 (g) + H2O(l) Weight of pure magnesium in the sample is a. 0.1825 g b. 0.0913 g c. 0.3194 g d. 0.0456 g Percentage of magnesium carbonate in the sample is a. 24.20% b. 27.66% c. 48.40% d. 96.80%We have talked about in lecture about metamorphic grade, and about the difference between progradeand retrograde mineral reactions. One such possible mineral reaction is as follows:orthoclase + sillimanite + H2O = muscovite + quartz 3a: Write a balanced chemical reaction for the above minerals, given that the formula for muscovite isK2Al6Si6O20(OH)4 3b: Indicate which reaction direction (left to right, right to left) is the prograde direction, and explainwhy you think that.
- An ore containing magnetite, Fe3O4, was analysed by dissolving a 4.9 g sample in concentrated HCl, giving a mixture of Fe2+ and Fe3+. After adding HNO3 to oxidize any Fe2+ to Fe3+, the resulting solution was diluted with water and the Fe3+ precipitated as Fe(OH)3 by adding NH3. After filtering and rinsing, the residue was ignited, giving 2.8 g of pure Fe2O3. Calculate the %w/w Fe3O4 in the sample (Fe3O4 =231.54 g/mol, Fe2O3 = 159.69 g/mol)The aluminium in a 1.2 g sample of impure NH4Al (SO4)2 was precipitated as hydrous Al2O3. The precipitate was filtered and ignited at 100° c to give anhydrous Al2O3 which weighed 0.1798 g. Calculate the % Al in the sample. (number of moles Al = 2; Al2O3 = 1)A 0.4852g sample of an iron ore was dissolved in acid to the 3+ state, then precipitated as Fe2O3 x H2O. The pp was filtered, washed and calcined to Fe2O3, which gave a weight of 0.2481g. Calculate the Fe % in the sample.