The percentage dissociation of a decinormal solution of a weak acid $HA$ is: $(K_a = 4.9 \times 10^{-8})$

The $pK_a$ of acetylsalicylic acid (aspirin) is $3.5$. The $pH$ of gastric juice in the human stomach is about $2-3$ and the $pH$ in the small intestine is about $8$. Aspirin will be

The degree of ionization of $0.4 \ M$ acetic acid will be $(K_{a} = 1.8 \times 10^{-5})$.

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

Calculate the molar concentration of a weak monobasic acid if the acid dissociation constant $K_a = 1.8 \times 10^{-5}$ and the degree of dissociation $\alpha = 0.01$.

If the ionization constant of hypochlorous acid $(HOCl)$ is $2.5 \times 10^{-5}$,the $pH$ of $1.0 \ M$ of its solution is $(\log 5=0.7)$.