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 $H B \left( K _{ a }\right)=1 \times 10^{-8}$ )

  • [IIT 2018]
  • A

    $4.47$

  • B

    $4.48$

  • C

    $4.49$

  • D

    $4.50$

Similar Questions

The hydrogen ion concentration of $0.1\,N$ solution of $C{H_3}COOH,$ which is $30\%$ dissociated, is

The $pH$ of $0.005 \,M$ codeine $\left( C _{18} H _{21} NO _{3}\right)$ solution is $9.95 .$ Calculate its ionization constant and $p K_{ b }$

$K_b$ for $NH_4OH$ is $1.8\times 10^{-5}.$ The $[\mathop O\limits^\Theta  H]$ of $0.1\,M\,NH_4OH$ is

Dissociation constant for a monobasic acid is $10^{-4}$ . What is the $pH$ of the monobasic acid ? (If $\%$ dissociation $= 2\,\%$ )

The ${K_b}$ of ammonia is $1.8 \times {10^{ - 5}}$ at $298$ $K$ temperature. Calculate the $pH$ of $0.1$ $M$ solution.