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The solubility of a salt of weak acid (AB) at pH 3 is Y×10−3molL−1. The value of Y is _______.(Given that the value of solubility product of AB Ksp=2×10−10 and the value of ionization constant of HB Ka=1×10−8)

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answer is 4.47.

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Detailed Solution

S=KspH+Ka+1=2×10−1010−310−8+1≃2×10−5=4.47×10−3M

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