A buffer solution is prepared in which the concentration of `NH_3` is 0.30(M) and the concentration of `NH_4^+` is 0.20(M). 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 0.30 M and the concentration of 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 0.30M and the concentration of NH_(4)^(+) is 0.20M . If the equilibrium constant k_(b) for NH_(3) equals 1.8xx10^(-3) what is the pH of this solution?

A buffer solution is prepared in which the concentration of NH_(3) is 0.30 M and the concentration of 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? ( log 2.7=0.43 )

A buffer solution is prepared in which the concentration of NH_(3) is 0.30 M and the concentration of 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? ( log 2.7=0.43 )

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

The ionisation constant of NH_3 is 1.77 xx 10^(-5) . What is the 'a' and 'pH' of 0.05M ammonia solution?