Calculate the dissociation constant of a $0.001 \ M$ weak monoacidic base undergoing $2 \%$ dissociation.

The conjugate base of the strong acid in the reaction $CH_3COOH + HCl \rightleftharpoons Cl^{\Theta} + CH_3COOH_2^{\oplus}$ is:

Arrange $NH_4^+$,$H_2O$,$H_3O^+$,$HF$,and $OH^-$ in increasing order of their acidic strength.

The first ionization constants ($pK_a$ values) for the following dicarboxylic acids are given:
Oxalic acid: $pK_1$
Malonic acid: $pK_2$
Heptanedioic acid: $pK_3$
Which of the following represents the incorrect order of their $pK_a$ values?

Which of the following statements is true?

Given the following $K_a$ values,determine which species is the strongest base: $HSO_4^- = 1.2 \times 10^{-2}$,$H_2PO_4^- = 6.3 \times 10^{-8}$,$HCO_3^- = 4.7 \times 10^{-11}$.