Calculate the amount of `(NH_(4))_(2)SO_(4)` in grams which must be added to `500 ml` of `0.2 M NH_(3)` to yield a solution of `pH=9`, `K_(b)` for `NH_(3)=2xx10^(-5)`

Calculate the amount of (NH_(4))_(2)SO_(4) in grams which must be added to 500ml of 0.2MNH_(3) to give a solution of pH=9.3 .Given pK_(b) for NH_(3)=4.7 .

Calculate the weight of (NH_(4))_(2)SO_(4) which must be added to 500mL of 0.2M NH_(3) to yield a solution of pH = 9.35. K_(a) for NH_(3) = 1.78 xx 10^(-5) .

What will be the amount of (NH_(4))_(2)SO_(4) (in g) which must be added to 500 mL of 0.2 M NH_(4)OH to yield a solution of pH 9.35? ["Given," pK_(a)"of "NH_(4)^(+)=9.26,pK_(b)NH_(4)OH=14-pK_(a)(NH_(4)^(+))]

Amount of (NH_(4))_(2)SO_(4) which must be added to 50mL of 0.2 M NH_(4)OH solution to yield a solution of pH 9.26 is ( pK_(b) of NH_(4)OH=4.74 )

Calculate pH of - 10^(-3) NH_(2)SO_(4)