AlF3 is insoluble in liquid HF, but dissolves if NaF is present. When BF3is added to the solution, AlF3 precipitates. Explain the three observations. Show equations if can be applied

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 Bank

Please provide detailed solution and give the explanation of the concept....

Please don't provide handwritten solution ....

4. Solid nickel carbonate (NiCO3) is pretty insoluble in water, as are many metal carbonates. But it is much more soluble in aqueous solutions of NaCN because nickel (II) reacts with cyanide anion to form a tetracyanonickelate complex. Nickel (II) is also mildly acidic, but you can ignore that part of the system if you want. A.) Write the balanced chemical equations AND the corresponding equilibrium constant expressions that explain the solubility behavior of nickel carbonate in aqueous 0.1 M NaCN. B.) Write the charge balance expression that applies to the BCE's you wrote above. C.) Write one mass balance expression for the system.

1. In which species does bromine have an oxidation number 0? 2. Balanced molecular equation for complete neutralization of H2SO4 by KOH in aq solution is?

You want to separate Cd2* and Fe2+ (initial concentration 103 mol/L) by means ofprecipitation of the corresponding sulphides. Is therea pH range in which one of the two metals is precipitated quantitatively(concentration in the solution less than or equal to 10" mol/L) is precipitatedwhile the other is still completely_in solution?Calculate and name this pH range where pH values below 0are set equal to O. Illustrate the situation graphically by drawing

Please solve this

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

3. To verify the existence of silver in your solution, one should first form a white precipitate by addition of NaCl. Next, the precipitate should dissolve in aqueous ammonia. Silver can re- precipitate by addition of 6M HNO,. Using chemical equations, describe the identity of the product formed in each step. E (Your three steps should be after addition of NaCl, after addition of ammonia and after addition of HNO,.) 3° 3° it in mirod with sodium chloride