The boiling point of a 0.200 mol kg^-1 aqueous solution of a weak monobasic acid HA is elevated by 0.130 K. Take K_b=0.52 K kg mol^-1, Delta T_b=iK_bm and the equilibrium HA H+ + A-. The degree of dissociation of HA is

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The boiling point of a $0.200 mol k g^{- 1}$ aqueous solution of a weak monobasic acid HA is elevated by $0.130 K$ . Take $K_{b} = 0.52 K kg mo l^{- 1}$ , $Δ T_{b} = i K_{b} m$ and the equilibrium $HA H X^{+} + A X^{-}$ . The degree of dissociation of HA is

i = Δ T_{b} / (K_{b} m) = 0.130/ (0.52 \times 0.200) = 1.25

. For

HA H X^{+} + A X^{-}

i = 1 + α

, so

α = 0.25

. Using

α = (i - 1) /2

or setting

α = i - 0.5

are the usual slips.