Calculate pH of a buffer solution that contains 0.1M `NH_(4)OH(K_(b)=10^(-5))` and 0.1 M `NH_(4)Cl.`

The pK_(a) value of NH_(3) is 5. Calculate the pH of the buffer solution, 1 L of which contains 0.01 M NH_(4)Cl and 0.10M NH_(4)OH :

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) .

What is [NH_(4)^(+)] in a solution that contain 0.02 M NH_(3)(K_(b)=1.8xx10^(-5)) and 0.01 M KOH?

Calculate the molar solubility of Fe(OH)_(3) in a buffer solution that is 0.1M in NH_(4)OH and 0.1M in NH_(4)Cl (K_(b) of NH_(4)OH=1.8xx10^(-5) , K_(sp) of Fe(OH)_(3)=2.6xx10^(-39) )

Find the pH of a buffer solution having equal volumes of 0.2MNH_(4)OH and 0.2M NH_(4)Cl (K_(b) for base =1.0xx10^(-5) )

Calculate the change in pH of 1 litre buffer solution containing 0.1 mole each of NH_(3) and NH_(4)CI upon addition of: (i) 0.02 mole of dissolved NaOH. Assume no change in volume. K_(NH_(3))=1.8xx10^(-5)

Calculate the change in pH of 1 litre buffer solution containing 0.1 mole each of NH_(3) and NH_(4)CI upon addition of: (i) 0.02 mole of dissolved gasous HCI. Assume no change in volume. K_(NH_(3))=1.8xx10^(-5)

Calculate the pH of a solution made by mixing 0.1 M NH_(3) and 0.1M (NH_(4))_(2)SO_(4). (pK_(b) of NH_(3) = 4.76)

Calculate the pH of a buffer by mixing 0.15 mole of NH_(4)OH and 0.25 mole of NH_(4)Cl in a 1000mL solution K_(b) for NH_(4)OH = 2.0 xx 10^(-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) .