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At $298 \ K$ temperature,calculate the $pH$ of a $0.25 \ M$ solution of $(CH_3)_2NH$ given that its $K_b$ is $5.4 \times 10^{-4}$.

$A$ weak monobasic acid is $2 \%$ dissociated in its $0.1 \ M$ solution. What is its dissociation constant?

For two acids $A$ and $B$,the values of $pK_{a1} = 1.2$ and $pK_{a2} = 2.8$ are given. Which of the following is correct?

$A$ weak monoacidic base dissociates to $1.5 \%$ in $0.001 \ M$ solution at $298 \ K$. Calculate the dissociation constant of the weak base.

For a $0.1 \ M$ solution of a weak acid $HQ$,the $pH$ is $3$. The ionization constant $K_a$ of the acid is:

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