A buffer solution made with `NH_3` and `NH_4Cl` has a pH of 10.0 which procedure could be used to lower the pH ?
1.Adding HCl , 2.Adding `NH_3` , 3. Adding `NH_4Cl`

Solution of 0.1 N NH_4OH and 0.1 NH_4Cl has has pH 9.25 Then pK_b of NH_4OH is

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-

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) .

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

NH_(4)Cl rarr NH_(3)+HCl . Which type of reaction is the ?

pH of a buffer solution composed of NH_(3) and NH_(4)Cl is 9.26. will there be any change in pH if 100 mL of distilled water is added to 100 mL of this buffer solution?

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)

One litre of a buffer solution is prepared by dissolving 0.6 mole. of NH_3 and 0.4 mole of NH_4CI . What is the pH of the solution ? For NH_3K_b = 1.8 xx 10^(-5) . What is the pH of the buffer after addition of 0.1 mole of NaOH ?