$A$ centimolar solution of a weak acid is $1.3 \%$ dissociated at $298 \ K$. What is its dissociation constant?

If $1 \ mM$ solution of ethylamine produces $pH = 9$,then the ionization constant $(K_b)$ of ethylamine is $10^{-x}$. The value of $x$ is . . . . . . (nearest integer). [The degree of ionization of ethylamine can be neglected with respect to unity.]

If a metal hydroxide with the molecular formula $M(OH)_4$ is $50\%$ ionized,then the $pH$ of its $0.0025 \ M$ solution will be:

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:

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 $\alpha = 0.01$.

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