Table 4.2 Solubility Rules for Common lonic Compounds in Water at 25°CInsoluble ExceptionsSoluble CompoundsCompounds containing alkali metalions (Li*, Na, K, Rb, Cs) andthe ammonium ion (NH)Nitrates (NO3), acetates (CH3COO ),bicarbonates (HCO3), chlorates(CIO3), and perchlorates (CIO4)Halides of Ag, Hg, and Pb2Sulfates of Ag, Ca2, Sr2, Ba, Hg, and PbHalides (Cl", Br", I)Sulfates (SO)Insoluble CompoundsSoluble ExceptionsCarbonates (CO), phosphates(PO), chromates (CrO),sulfides (S2)Compounds containing alkali metal ionsand the ammonium ionHydroxides (OH)Compounds containing alkali metal ionsand the Ba ion2+

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Asked Sep 12, 2019
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With reference to the Solubility Rule for Common ionic compounds in water, suggest one method by which you might separate:
(a) K+ from Ag+,
(b) Ba2+ from Pb2+,
(c) NH4+ from Ca2+,
(d) Ba2+ from Cu2+.

NB: I have attached a table of the solubility rules to this question as an image (an attachment below). Please open that and don't reject the question as being incomplete. Take a look at the attachment please!!!! Thanks.

Table 4.2 Solubility Rules for Common lonic Compounds in Water at 25°C
Insoluble Exceptions
Soluble Compounds
Compounds containing alkali metal
ions (Li*, Na, K, Rb, Cs) and
the ammonium ion (NH)
Nitrates (NO3), acetates (CH3COO ),
bicarbonates (HCO3), chlorates
(CIO3), and perchlorates (CIO4)
Halides of Ag, Hg, and Pb2
Sulfates of Ag, Ca2, Sr2, Ba, Hg, and Pb
Halides (Cl", Br", I)
Sulfates (SO)
Insoluble Compounds
Soluble Exceptions
Carbonates (CO), phosphates
(PO), chromates (CrO),
sulfides (S2)
Compounds containing alkali metal ions
and the ammonium ion
Hydroxides (OH)
Compounds containing alkali metal ions
and the Ba ion
2+
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Table 4.2 Solubility Rules for Common lonic Compounds in Water at 25°C Insoluble Exceptions Soluble Compounds Compounds containing alkali metal ions (Li*, Na, K, Rb, Cs) and the ammonium ion (NH) Nitrates (NO3), acetates (CH3COO ), bicarbonates (HCO3), chlorates (CIO3), and perchlorates (CIO4) Halides of Ag, Hg, and Pb2 Sulfates of Ag, Ca2, Sr2, Ba, Hg, and Pb Halides (Cl", Br", I) Sulfates (SO) Insoluble Compounds Soluble Exceptions Carbonates (CO), phosphates (PO), chromates (CrO), sulfides (S2) Compounds containing alkali metal ions and the ammonium ion Hydroxides (OH) Compounds containing alkali metal ions and the Ba ion 2+

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Expert Answer

Step 1

Separation of a given mixture of the cation is done on the basis of formation of precipitates by cation when reacting with suitable anion in the solution.

 

K+ and Ag+ can we separated  from the given solution if we add chlorine ion in it.

As K+ react with Cl- ion to form KCl which is, in liquid form and when Ag+ react with Cl- ion it forms AgCl solid salt. In this way K+ ion is separated from Ag+ ion

Step 2

Separation of Ba2+ from Pb2+

As the separation of ion is done on the basis of formation of salt or precipitation. To separates Ba2+ and Pb2+ we add OH- ion in the mixture of Ba2+ and Pb2+.

Since Ba2+ react with OH- to form Ba(OH)2 which is soluble and are in present liquid form. Whereas Pb(OH)2 is insoluble and are present in a solid-state.

Step 3

Separation of NH4+ from Ca2+

As carbonate ion (CO32-) is formed soluble compounds with alkali metal and ammonium ion therefore we add carbonate ion in the mixture of NH4+ and Ca2+ then ammonium ion form ammonium carbonate [(NH4)2CO3] which are solu...

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