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What is the order of solubility of carbonates ,sulphates & hydrogencarbonates in metal carbonates , metal sulphates and metal hydrogencarbonates...???
I have my aieee exams approaching !!! Help me yaar... Three cheers ***
Explanation of solubility trends(usually dealt with later in course e.g. in UK A2 advanced level)
The simplest approach is to consider thetwo enthalpy change trends.
Theprocess of dissolving can be analysed in terms of two theoretical stagese.g. for simple cation–anion ionic compound.
In the arguments outlined belowMn+could be Gp1 or Gp2 metal cation etc.,Xn–could be halide, oxide, hydroxide, sulphate, carbonate anion etc., and n is the charge on ion – the n's may be different or the same):
(1)Mn+aXn–b(s)==> aMn+(g)+ bXn–(g)(breaking the lattice apart into its constituent ions)
This process is always endothermic, and is called thelattice enthalpy. Its usually defined in the opposite direction by saying it is 'the energy released when 1 mole of an ionic lattice is formed from its constituent gaseous ions' (at 298K, 1 atmos./101kPa pressure).
*The lattice enthalpy decreases down the group as the cation radius increases (anion radius constant for a particular seriese.g. sulphates). Therefore, energetically, the solvationin terms of lattice energy is increasingly favoured down the group.
(2) Mn+(g)+ aq==>Mn+(aq)andXn–(g)+ aq==>Xn–(aq)
Representing the solvation–hydration of ions.
The equations above represent to the two 'hydration enthalpies', the heat released when an isolated gaseous ion becomes solvated by water to form an aqueous solution (1M, 298K, 1 atmos./101kPa pressure)
*The hydration enthalpy for the cation decreases down the group as the radius gets larger. Therefore, energetically, the solvation is less favoured down the group as the cation radius increases.
* In both cases the numerical enthalpy value increases the smaller the radii as charges closer,and the greater the ionic charge (constant for a series), both factors increase the electrical attraction of either cation–anion in the crystal or ion–water in aqueous solution.
Thank YouRuchiAskiitians Faculty
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