2. A solution that may contain Cu", Bi?", Sn, or Sb?* 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 HNO; and gives only a white precipitate upon the addition of NH¸OH. 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?
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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?A solution of unknown group I ions gives a white precipitate with HCl.When treated with hot water, it gives a solution to which K2CrO4 is added, and a yellow precipitate forms.The white precipitate that remains after the hot water treatment dissolves completely in NH3. Which ions are present and which are not?A pink solid has the formula CoCl3 5NH3 H2O. A solution of this salt is also pink and rapidly precipitates 3mol AgCl(s) on titration with silver nitrate solution. When the pink solid is heated, it loses 1mol H2O to give a purple solid with the same mole ratio of NH3:Cl:Co as the pink solid. The purple solid releases two of its chloride ions rapidly; then on dissolution and titration with AgNO3, release one of its chloride ions slowly. Deduce the structures, draw and name 2 octhahedral complexes
- a. What cations may be present in a pale blue solution that turns deep blue and forms a white precipitate upon 6M NH3(aq)? b. A white solid dissolves in water to form a neutral solution. No precipitate forms when the solution is treated with a solution of NH4Cl/ NH3 buffer, nor when (NH4)2S is added. When the solution is acidified with HC2H3O2 and K2CrO4 is added a yellow precipitate forms. This precipitate dissolves upon addition of concentrated HCl. Acidification of a solution of the solid with HNO3 followed by addition of AgNO3 causes formation of a white precipitate. What is the identity of the original solid?An antihistamine sample, brompheniramine maleate, weighing 5.01234 g was dissolved in alcohol and decomposed with metallic sodium. The resulting solution was treated with 12.00mL of 0.3121M AgNO3 to precipitate all of the liberated bromide ions as AgBr. The excess AgNO3 remaining in the solution was titrated with 9.123mL of 0.2181M KSCN to reach the endpoint. What is the %Br in the sample? Br- + Ag+ --> AgBr(s) Ag+ + SCN- --> AgSCN(s) Br = 79.904 g/molUtilize the systematic treatment to determine the concentrations of all species present in a solution of: 1.) 0.35 M CaF in H2O 2.) saturated PbSO4 buffered at pH 7 3.) 0.05 M KC2O4 in H2O Please show COMPLETE solution
- Chromel 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.A solution containing a mixture of metal cations was treated with dilute HCl and no precipitate formed. Next, H, S was bubbled through the acidic solution. A precipitate formed and was filtered off. Then, the pH was raised to about 8 and H,S was again bubbled through the solution. A precipitate again formed and was filtered off. Finally, the solution was treated with a sodium carbonate solution, which resulted in no precipitation. Classify the metal ions based on whether they were definitely present, definitely absent, or whether it is possible they were present in the original mixture. Definitely present Definitely absent Possibly present Cd²+ Ag* Ba2+ Mn2+ Mg2+ Fe2+ A13+ Pb2+ Sn2+ Lit Hg3* Hg²+ Sb3+ Answer BankA solution containing a mixture of metal cations was treated with dilute HCl and no precipitate formed. Next, H, S was bubbled through the acidic solution. A precipitate formed and was filtered off. Then, the pH was raised to about 8 and H, S was again bubbled through the solution. A precipitate again formed and was filtered off. Finally, the solution was treated with a sodium carbonate solution, which resulted in no precipitation. Classify the metal ions based on whether they were definitely present, definitely absent, or whether it is possible they were present in the original mixture. Definitely present Definitely absent Possibly present Answer Bank Hg3+ Pb2+ Lit Bj³+ Sn2+ Ni2+ A13+ Ag* Zn2+ Ba2+ Mg2+ Hg²+ Cu?+
- A solution containing a mixture of metal cations was treated with dilute HCl and no precipitate formed. Next, H, S was bubbled through the acidic solution. A precipitate formed and was filtered off. Then, the pH was raised to about 8 and H,S was again bubbled through the solution. A precipitate again formed and was filtered off. Finally, the solution was treated with a sodium carbonate solution, which resulted in no precipitation. Classify the metal ions based on whether they were definitely present, definitely absent, or whether it is possible they were present in the original mixture. Definitely present Definitely absent Possibly presentA solution containing a mixture of metal cations was treated with dilute HCl and no precipitate formed. Next, H,S was bubbled through the acidic solution. A precipitate formed and was filtered off. Then, the pH was raised to about 8 and H, S was again bubbled through the solution. A precipitate again formed and was filtered off. Finally, the solution was treated with a sodium carbonate solution, which resulted in no precipitation. Classify the metal ions based on whether they were definitely present, definitely absent, or whether it is possible they were present in the original mixture. Definitely present Definitely absent Possibly present Answer Bank Bi3+ Cu²+ Ni?+ Lit Ag+ Sn2+ Pb2+ A13+ Ba2+ Zn²+ Hg²+ Mg?+ Hgž+A solution containing a mixture of metal cations was treated with dilute HCl and no precipitate formed. Next, H, S was bubbled through the acidic solution. A precipitate formed and was filtered off. Then, the pH was raised to about 8 and H, S was again bubbled through the solution. A precipitate again formed and was filtered off. Finally, the solution was treated with a sodium carbonate solution, which resulted in no precipitation. Classify the metal ions based on whether they were definitely present, definitely absent, or whether it is possible they were present in the original mixture. Definitely present Definitely absent Possibly present Ag* Hg²+ Lit Ba²+ Pb2+ Mg²+ Hg3* 2+ Answer Bank Zn2+ Sn2+ Ni2+ Cu2+ Bi3+ A13+ Incorrect