In a buffer solution containing equal concentration of B^- and HB , the K_b for B^- is 10^-10 . The pH of the buffer solution is: - Chemistry MCQ Chemistry | ExamTest.live

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In a buffer solution containing equal concentration of B^{-} and HB, the K_{b} for B^{-} is 1 0^{- 10} . The pH of the buffer solution is:

A $4$
B $10$
C $7$
D $6$

Solution & Step-by-step Explanation

1. Use Henderson-Hasselbalch equation for basic buffer (or relate K_{a} and K_{b}): K_{a} \cdot K_{b} = K_{w} = 1 0^{- 14} K_{a} = 1 0^{- 14} /1 0^{- 10} = 1 0^{- 4} p K_{a} = - lo g (1 0^{- 4}) = 4 For an acidic buffer (HB/B^{-}): pH = p K_{a} + lo g (\frac{[ Conjugate Base ]}{[ Acid ]}) Since [B^{-}] = [HB], lo g (1) = 0 . pH = p K_{a} = 4 .

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In a buffer solution containing equal concentration of B^{-} and HB, the K_{b} for B^{-} is 1 0^{- 10} . The pH of the buffer solution is:

4

10

7

6

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Ionic Equilibrium Buffer Solutions pH

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In a buffer solution containing equal concentration of $B^{-}$ and $HB$ , the $K_{b}$ for $B^{-}$ is $1 0^{- 10}$ . The $pH$ of the buffer solution is:

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In a buffer solution containing equal concentration of B− and HB, the Kb​ for B− is 10−10. The pH of the buffer solution is:

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In a buffer solution containing equal concentration of $B^{-}$ and $HB$ , the $K_{b}$ for $B^{-}$ is $1 0^{- 10}$ . The $pH$ of the buffer solution is: