In a buffer solution having equal concentrations of B^(-) and HB the value of K_b for B^(-) is 10^(-9) . The pH of buffer solution is

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Correct answer: (B) 5. For acidic buffer pH can be find out as follows pH=pKa+log_10([salt])/([acid]) As here K_b=10^(-9) So K_a=10^(-5) pK_a=5 As pH=5+⁡log_10([B^(-)])/([HB]) As [B^(-)]=[HB] pH=5+log 1=5 + 0 = 5

In a buffer solution having equal concentrations of $B^{-}$ and HB the value of $K_{b}$ for $B^{-}$ is $1 0^{- 9}$ . The pH of buffer solution is

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More Ionic Equilibrium Questions

In a buffer solution having equal concentrations of B- and HB the value of Kb for B- is 10-9 . The pH of buffer solution is

Solution

More Ionic Equilibrium Questions

In a buffer solution having equal concentrations of $B^{-}$ and HB the value of $K_{b}$ for $B^{-}$ is $1 0^{- 9}$ . The pH of buffer solution is