$A$ weak monoprotic acid of $0.1 \ M$ ionizes to $1\%$ in solution. What will be the $pH$ of the solution?

Accumulation of lactic acid $(HC_3H_5O_3),$ a monobasic acid in tissues,leads to pain and a feeling of fatigue. In a $0.10 \ M$ aqueous solution,lactic acid is $3.7 \%$ dissociated. The value of the dissociation constant,$K_a,$ for this acid will be:

What is the $pH$ of acetic acid at equilibrium,given that acetic acid concentration is $0.1 \ M$ and it is $30 \%$ dissociated at equilibrium? $(\log 3=0.47)$

If the $pH$ of $0.10 \ M$ monobasic acid at $298 \ K$ is $5.0$,the value of $p K_a$ at the same temperature is

Calculate the $[H^{+}]$ ion concentration in a $1.00 \ M$ $HCN$ solution $(K_a = 4 \times 10^{-10})$.

The $pH$ of a $0.1 \ M$ solution of a weak monoprotic acid that is $1\%$ ionized is: