In: Chemistry
1) Identify cations by selective precipitation and specific reaction of these mixture:
Cu(2+); Bi (3+), Cd (2+), Sb(5+); Sn (2+), Fe(3+), Co(2+), Mg(2+), Li+
2) Calculate the solubility of each of the following compounds
in moles per liter. Ignore
any acid–base properties.
PbI2, K(sp) = 1.4 * 10^-8
CdCO3, K(sp)= 5.2 * 10^-12
Sr3(PO4)2, K(sp)= 1*10^-31
1)
Group2:
Devided in to 2 groups 2A and 2B ; Based on the solubility of the cations in ammonium polysuphide (NH4)2Sx
Cu2+; Bi3+, Cd2+; these are insoluble in ammonium polysulphide. So they belong to group 2A
Sb(5+), Sn (2+); Soluble in ammonium polysulphide. So they belong to group 2B
Group 3:
Fe(3+), Co(2+); the group reagent is ammonium sulphide solution or hydrogen sulphide gas in the presence of ammonia and ammonium chloride. These cations won't react with 2nd group reactants.
Group 5:
Mg2+
belongs to this group 5.
It has similar characteristics to alkali metals. Its general
properties are similar to that of potassium as the sizes of both
ions are identical.
2)
PbI2
Ksp = [Pb2+] [I-]2
Solving for x will give :
CdCo3Ksp = [Cd2+] [Co2-]3
Sr3(PO4)2 [Sr2+]3 [Po3-]4
from this x can be calculated