A buffer solution is prepared in which the concentration of NH_(3) is 0.30 M and the concentrationof NH_(4)^(+) is 0.20 M. If the equilibrium constant, K_(b) for NH_(3) equals 1.8xx10^(-5), what is the pH of this solution ?

A buffer solution is prepared in which the concentration of NH_(3) is

1.	A buffer solution is prepared in which the concentration of NH_(3) is 0.30 M and the concentrationof NH_(4)^(+) is 0.20 M. If the equilibrium constant, K_(b) for NH_(3) equals 1.8xx10^(-5), what is the pH of this solution ?
Answer» <P>8.73 9.08 9.43 11.72 Solution :`p_(OH)=pK_(B)+log.(["Salt"])/(["BASE"])=4.74+log.(0.20)/(0.30)` `=4.74+(0.301-0.4.74)=4.74-0.176` `=4.56` `:. pH = 14 - 4.56 = 9.44`