[" 3.(13) In order to prepare a buffer of pH "8.26" ,the amount of "(NH,sSO_(4)" required to be mixea with "1L" of "(q_(4)" 2"],[NH," is "[pKb=4.74]],[" 1) "1.0ma/L" ."]

For the preparation of a buffer of pH = 8.26 , the amount of (NH_4)_(2)SO_(4) required to be mixed with one litre of 0.1 (M) NH_3(aq), pK_b = 4.74 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:

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:

In a buffer solution, total concentration of NH_(3) and NH_(4)Cl is 0.6 (M). If the pH of the buffer be 9.0 then, find the amount of NH_(3) and NH_(4)Cl required to prepare 1L of that buffer. Given: pK_(b)(NH_(3))=4.74

To prepare a buffer solution of pH=4.04, amount of Barium acetate to be added to 100mL of 0.1 M acetic acid solution [ pkb (CH3COO-)=9.26] is:

To prepare a buffer solution of pH=4.04, amount of Barium acetate to be added to 100 mL of 0.1 M acetic acid solution [pK_b(CH_(3)COO^(-))=9.26] is:

To prepare a buffer solution of pH=4.04, amount of Barium acetate to be added to 100 mL of 0.1 M acetic acid solution [pK_b(CH_(3)COO^(-))=9.26] is:

Calculate the amount of NH_(3) and NH_(4)CI required to prepare a buffer solution of pH 9.0 when total concentration of buffering reagents is 0.6 mol L^(-1) . (pK_(b)for NH_(3)=4.7,log 2=0.30)