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

Question

MARKS Content Team · Accepted Answer

Correct answer: (A) 4. For acidic buffer pH can be find out as follows pH=pKa+log_10([salt])/([acid]) Here K_b=10^(-10)K_a=10^(-4),pK_a=4 As pH=4+log_10([B^(-)])/([HB]) As [B^(-)]=[HB] pH=4+log1=4

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

Solution

More Ionic Equilibrium Questions

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

Solution

More Ionic Equilibrium Questions

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