The dissociation constant of an acid $HA$  is $1 \times {10^{ - 5}}$. The $pH$ of $0.1$ molar solution of the acid will be

  • A

    $5$

  • B

    $4$

  • C

    $3$

  • D

    $1$

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

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  • [AIIMS 2004]

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  • [IIT 2009]

When $CO_2$ dissolves in water, the following equilibrium is established

$C{O_2} + 2{H_2}O\, \rightleftharpoons {H_3}{O^ + } + HCO_3^ - $

for which the equilibrium constant is $3.8 \times 10^{-7}$ and $pH = 6.0$. The ratio of  $[HCO_3^- ]$ to $[CO_2]$ would be :-