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[" To prepare a buffer of "pH=8.26" ,cal...

[" To prepare a buffer of "pH=8.26" ,calculate number of moles of "(NH_(4))_(2)SO_(4)" to be added to "1L" of "0.1M],[NH_(4)OH" solution.[pKa(NH_4 ^ prime ) = 9.26] "],[[" (1) "0.025" mole "," (2) "0.5" mole "," (3) "1" mole "," (4) "2" mole "]]

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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:

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 ?

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 )

A buffer solution contains 1 mole of (NH_(4))_(2)SO_(4) and 1 mole of NH_(4)OH(K_(b)=10^(-5)) . The pH of solution will be:

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]

pH of 0.01 M (NH_(4))_(2) SO_(4) and 0.02 M NH_(4)OH buffer (pK_(a) of NH_(4)^(+)=9.26) is