The $pH $ of a $0.01\,M$ solution of acetic acid having degree of dissociation $12.5\%$ is

  • A

    $5.623$

  • B

    $2.903$

  • C

    $3.723$

  • D

    $4.509$

Similar Questions

The percentage of pyridine $(C_5H_5N)$ that forms pyridinium ion $(C_5H_5N^+H)$ in a $0.10\, M$ aqueous pyridine solution ($K_b$ for $C_5H_5N = 1.7 \times 10^{-9}$) is

  • [NEET 2016]

Values of dissociation constant, $K_a$ are given as follows

      Acid       $K_a$
      $HCN$       $6.2\times 10^{-10}$
      $HF$       $7.2\times 10^{-4}$
      $HNO_2$       $4.0\times 10^{-4}$

Correct order of increasing base strength of the base $CN^-,F^-$ and $NO_2^-$ will be

  • [JEE MAIN 2013]

Derive the equation of ionization constant $({K_b})$ of weak base.

A certain amount of $H_2CO_3$ & $HCl$ are dissolved to form $1$ litre solution. At equilibrium it is found that concentration of $H_2CO_3$ & $CO_3^{-\,-}$ are $0.1\,M$ & $0.01\,M$ respectively. Calculate the $pH$ of solution. Given that for $H_2CO_3$ $K_{a_1} =10^{-5}$ & $K_{a_2} =10^{-8}$

$25$ $mL$ $0.1$ $M$ $HCl$ solution is diluted till $500$ $mL$. Calculate $pH$ of dilute solution.