At 20°C the solubility product of strontium sulphate is 4.0 x 107 mol? dm6. Compare the solubility of strontium sulphate in a) pure water and b) 0.1M NazSO4.
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At 20°C the solubility product of strontium sulphate is 4.0 x 107 mol? dm6. Compare the solubility of strontium sulphate in a) pure water and b) 0.1M NazSO4.
The formula for strontium sulphate is SrSO4
hence the solubility reaction of SrSO4 is
=> SrSO4 (s) -------> Sr2+ (aq) + SO42- (aq)
Hence the solubility product or equilibrium constant expression will be
Ksp = Kc = [Sr2+ ] X [SO42- ] = 4 X 10-7
a) Assuming the solubility of SrSO4 is s molar
Hence it means s concentration of SrSO4 will dissolve in water
Hence the concentration of ions forming will be [Sr2+ ] = s = [SO42- ]
Hence substituting the values we get
s X s = 4 X 10-7 => s = solubility of SrSO4 in pure water = 6.32 X 10-4 mol/dm3
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