pH of Ba(OH)2 solution is 12. Its solubility product is :
5.0×10−7
0.6×10−12
4.0×10−8
5.0×10−9
A
5.0×10−7
B
0.6×10−12
C
4.0×10−8
D
5.0×10−9
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Solution
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Given: pH=12
Hence, pOH=14−pH=14−12=2 or [OH−]=10−2.
[Ba2+]=0.5×[OH−]=0.5×10−2.
The expression for the solubility product of barium hydroxide is,
Ksp=[Ba2+][OH−]2=(0.5×10−2)(1×10−2)2=5×10−7.
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