The $K_a$ of a weak acid $HA$ is $1.00 \times 10^{-5}$. If $0.100 \ mol$ of this acid is dissolved in $1 \ L$ of water,what is the percentage dissociation of the acid at equilibrium?

What is the $pH$ of a $1 \ M$ $CH_3COOH$ solution? Given that the $K_a$ of acetic acid $= 1.8 \times 10^{-5}$.

It has been found that the $pH$ of a $0.01 \ M$ solution of an organic acid is $4.15$. Calculate the concentration of the anion,the ionization constant of the acid and its $pK_a$.

The $pH$ of $1\, N$ aqueous solutions of $HCl$,$CH_{3}COOH$ and $HCOOH$ follows the order

An acid solution of $pH=6$ is diluted $1000$ times,the $pH$ of the final solution becomes

The $K_a$ of monobasic acid $A, B$ and $C$ are $10^{-6}, 10^{-8}$ and $10^{-10}$ respectively. The concentrations of $A, B$ and $C$ are respectively $0.1 \ M, 0.01 \ M$ and $0.001 \ M$. Which of the following is correct for $pOH$ of $A, B$ and $C$?