What weight of pyrite ore (impure FeS2) should be taken for analysis that the no. of centigram of precipitated BaSO4 will be twice the percentage of FeS2?
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- A solution that may contain Cu2+ , Bi2+ , Sn4+ , or Sb2+ is treated with thioacetamide in an acidic medium. The black precipitate which forms is partly soluble in strongly basic solution. The precipitate which remains is soluble in 6 M HNO3 and gives only a white precipitate upon the addition of NH4OH. The basic solution, when acidified, produces an orange precipitate. Which group II ions are present? Which are absent? Which are in doubt? How would you remove all doubt?What is the percentage of Nickel in an ore if, when analyzed by the cyanide method, 20.00mL of KCN solution (containing 1.00mmol of AgNO3 per milliliter) are used? Wt of sample used = 0.2500gChromel is an alloy composed of nickel, iron and chromium.A 0.6472 g sample was dissolved and diluted to 250 mL. When a50 mL aliquot of 0.05182 M EDTA was mixed with an equal volumeof the diluted sample and all the three ions were chelated, a 5.11 mLback titration with 0.06241 M copper (II) was required.The chromium in a second 50 mL aliquot was masked through theaddition of hexamethylenetetramine, titration of the Fe and Nirequired 36.28 mL of 0.05182 M EDTA.Iron and chromium were masked with pyrophosphate in a third50 mL aliquot and the nickel was titrated with 25.91 mL of theEDTA solution.Calculate the percentage of nickel, chromium and iron in thealloy.
- An unknown salt X reacts with hot conc. H2SO4 to produce a brown coloured gas which intensifies on addition on copper turnings. On adding dilute ferrous sulphate solution to an aqueous solution of X and then carefully adding conc. H2SO4along the sides of the test tube, a brown complex Y is formed at the interface between the solution and H2SO4. Identify X andY and write the chemical equation involved in the reaction.a) Which ion, Pt(II) or Mn(II), is more likely to form a sulfide in the presence of H2S in water. b) Rationalize your answer with the trends in hard and soft character. c) Give a balance chemical equation from your reaction.The solid is treated with hot water giving a solid and a solution. The solution is treated with K2CrO4 and no precipitate forms. What is your conclusion?
- What wt. of impure calcite (CaCO3) should be taken for analysis so that no. of milliliters of CO2 obtained by treating with acid, and measured dry at 18°C and 763 mm pressure, will equal the percentage of CaO in the sample?A 0.7352g sample of ore containing Fe3+, Al3+ and Sr2+ was dissolved and made up to 500.00 mL. The analysis of metals was performed by a chemistry using complexation volumetry. Initially, an aliquot of 50.00 mL had its pH adjusted to 1.0 and titrated with a standard solution of EDTA 0.02145 mol/L, requiring 6.95 mL to reach the end point. Subsequently, another 25.00 mL aliquot was buffered at pH=5 and titrated with the same EDTA solution, requiring 6.24 mL to reach the end point. Finally, a third aliquot of 25.00 mL was titrated at pH=11, requiring 11.10 mL of the same EDTA solution to complete the titration. Determine the percentage of each of the metals in the sample Given the molar masses: Fe=55.845 g/mol; Al=26.982 g/mol and Sr=87.620 g/mol.Comparing the two quantities based on the given condition, which is greater I or II? or are they equal? can the quantities be measured? Consider the analysis of Fe in ore using permanganate as titrant. Under the same acidic conditions I. % Fe with pre-reduction II. % Fe without pre-reduction
- Which characteristic of a precipitate doesn’t do well for gravimetric analysis. a Readily filtered and washed free of contaminants b Of sufficiently high solubility (Ksp) c Unreactive with constituents of the atmosphere and high purity d Of known composition after it is dried or, if necessary, ignited. e None of the aboveCaustic potash that has been exposed to air is found on analysis to contain 90.00% KOH, 2.38% K2CO3 and 7.62% H2O. What weight of residue will be obtained if 1.00 g of this sample is added to 46.00 mL of 1.00 N HCl and the resulting solution, after neutralization with 1.070N KOH is evaporated to dryness?what wt. of limestone containing 9.57% Mg must be taken for analysis in order to precipitate of 0.551g Mg2P2O7? how many grams of Na2SO4 are required to ppte Ag2SO4 from 2.000t of AgNO3? a sample of magnetite (impure Fe3O4) weighing 0.5000g is fused with oxidizing flux and the ferric compound formed is eventually precipitated as ferric hydroxide and ignited to ferric oxide which weighs 0.4980calculate %Fe & %Fe2O3