The solubility of a salt of weak acid $( A B )$ at $pH 3$ is $Y \times 10^{-3} mol L ^{-1}$. The value of $Y$ is . . . . . (Given that the value of solubility product of $A B \left( K _{ sp }\right)=2 \times 10^{-10}$ and the value of ionization constant of $\left.H B \left( K _{ a }\right)=1 \times 10^{-8}\right)$
The solubility of a salt of weak acid $( A B )$ at $pH 3$ is $Y \times 10^{-3} mol L ^{-1}$. The value of $Y$ is . . . . . (Given that the value of solubility product of $A B \left( K _{ sp }\right)=2 \times 10^{-10}$ and the value of ionization constant of $\left.H B \left( K _{ a }\right)=1 \times 10^{-8}\right)$
- A
$4.40$
- B
$4.44$
- C
$4.45$
- D
$4.47$
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