The solubility product (Ksp) of solid barium sulphate at 298 K is 1.1×10-10. The molar solubility, (S ) of Ba2+ and SO42- are
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a
1.05×10-7 mol L-1
b
1.05×10-10 mol L-1
c
1.05×10-6 mol L-1
d
1.05×10-5 mol L-1
answer is D.
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Detailed Solution
BaSO4(s)⇌∴in water Saturated solution Ba2+(aq)+SO42-(aq) If molar solubility is S, then 1.1×10-10=(S)(S)=S2or, S=1.05×10-5Thus, molar solubility of barium sulphate will be equal to 1.05×10-5 mol L-1