What is the molar solubility of `Mn(OH)_(2)``(K_(sp)=4.5xx10^(-14))` in a buffer solution containing equal amounts of `NH_(4)^(+)` and `NH_(3)` `(K_(b)=1.8xx10^(-5))`?

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) )

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 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) )

Calculate solubility of AgCN (K_(sp)= 4 xx 10^(-16)) in a buffer solution of PH=3. [(K_a)_(HCN)= 4 xx 10^(-10)] .

The pH of 0.10 M NH_(3) solution (K_(b)=1.8xx10^(-5)) is :

The molarity of NH_(3) of pH = 12 at 25^(@)C is (K_(b) = 1.8 xx 10^(-5))

The molarity of NH_(3) of pH = 12 at 25^(@)C is (K_(b) = 1.8 xx 10^(-5))