For the buffer solution containing `NH_(4)OH` and `NH_(4)Cl, P^(H)` of the buffer solution can be increased by

For the buffer solution containing NH_(4)OH and NH_(4) CI, P^(H) of the buffer solution can be increased by

For the buffer solution containing NH_(4)OH and NH_(4) CI, P^(H) of the buffer solution can be increased by

1 lit of buffer solution contains 0.1 mole each of NH_(4)OH and NH_(4)Cl . What will be the P^(H) of the solution when 0.01 mole of HCl is added to it [ P^(Kb) of NH_(4)OH = 4.74 ]

A buffer solution contains 0.25M NH_(4)OH and 0.3 NH_(4)C1 . a. Calculate the pH of the solution. b. How much NaOH should be added to 1L of the solution to change pH by 0.6.K_(b) =2xx10^(-5) .

A buffer solution contains 0.25M NH_(4)OH and 0.3 NH_(4)C1 . a. Calculate the pH of the solution. K_(b) =2xx10^(-5) .

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

A buffer solution containing NH_3 and NH_4Cl has a pH value of 9. pK_b for NH_3 is 4.7. If in the buffer solution total concentration of buffering reagents is 0.6 mol L^(-1) , then the amount of-

Calculate pH of the buffer solution containing 0.15 mole of NH_(4)OH " and " 0.25 mole of NH_(4)Cl. K_(b) " for " NH_(4)OH " is " 1.98 xx 10^(-5) .

Calculate pH of the buffer solution containing 0.15 mole of NH_(4)OH " and " 0.25 mole of NH_(4)Cl. K_(b) " for " NH_(4)OH " is " 1.98 xx 10^(-5) .