Conjugate base for Bronsted acids $H_{2}O$ and $HF$ are

When $K_2O$ is added to water,the solution becomes basic because it contains the concentration of which of the following?

Derive $K_w = K_a \times K_b$ and $pK_w = pK_a + pK_b$ for a weak base $B$ and its conjugate acid $BH^{+}$.

In the reaction $HNO_3 + H_2O \rightleftharpoons H_3O^{+} + NO_3^{-}$,the conjugate base of $HNO_3$ is = .......

According to the $Br\o nsted-Lowry$ theory,water is a/an:

Cis-butene dioic acid $\overset{K_{a_1}(-H^+)}{\longleftrightarrow} X_1^- \overset{K_{a_2}(-H^+)}{\longleftrightarrow} X_2^{2-}$
Trans-butene dioic acid $\overset{K'_{a_1}(-H^+)}{\longleftrightarrow} Y_1^- \overset{K'_{a_2}(-H^+)}{\longleftrightarrow} Y_2^{2-}$
The incorrect statement regarding the above information is: