How many mole of `NH_(4)CI` must be added to one liltre of `1.0M NH_(4)OH` to have a buffer of `pH=9`? `(K_(NH_(4)OH)=1.8xx10^(-5))`

How many mole of NH_4Cl must be added to one litre of 1.0 M NH_4OH to have a buffer of pH= 9. K_(NH_(4)OH)=1.8 xx 10^(-5)?

How many moles of NH_(4)C1 should be added to 200mL solution of 1.18 M NH_(4)OH to have a pH of 9.60. K_(b) of NH_(4)OH= 2 xx 10^(-5)

How many moles of NH_(4)Cl should be added to 200mL solution of 0.18 M NH_(4)OH to have a pH of 9.60. K_(b) of NH_(4)OH= 2 xx 10^(-5)

Calculate the number of moles of NH_(4)Cl that should be added to one litre of "1.0 M "NH_(4)OH to prepare buffer solution with pH=9[K_(b)=2xx10^(-5)," take log"2=0.3]

Calculate the number of moles of NH_(4)Cl that should be added to one litre of "1.0 M "NH_(4)OH to prepare buffer solution with pH=9[K_(b)=2xx10^(-5)," take log"2=0.3]

A buffer solution of pH 9 is to be prepared by mixing NH_4Cl and NH_4OH . Calculate the number of moles of NH_4Cl that should be added to 2 litre of 1 M NH_4OH solution , K_b = 1.8 X 10^(-5)

To prepare a buffer of pH 8.26 , amount of (NH_(4))_(2)SO_(4) to be added into 500mL of 0.01M NH_(4)OH solution [pK_(a)(NH_(4)^(+))=9.26] is:

To prepare a buffer of pH 8.26 , amount of (NH_(4))_(2)SO_(4) to be added into 500mL of 0.01M NH_(4)OH solution [pK_(a)(NH_(4)^(+))=9.26] is: