A buffer solution has equal volume of 0.20 M `NH_(4)OH` and 0.02 `MNH_(4)Cl :` The `pK_(b)` of the base is 5. The pH is

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) )

Solution of 0.1 N NH_(4)OH and 0.1 N NH_(4)Cl has pH 9.25 , then find out pK_(b) of NH_(4)OH .

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) .

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) .

An aqueous solution at room temperature contains 0.01 M NH_(4)Cl and 0.1M NH_(4)OH (pK_(b)=5), the pH of the solution is : a. 7.5 b. 10 c. 6.5 d. 6.8

A buffer solution contains 0.02 moles of NH_4OH and 0.03 moles of NH_4CI dissolved in 1 litre of the solution. Calculate the pH of the solution. Dissociation constant of NH_4OH "is" 1.8 xx 10^-5

The pH of 0.02 M NH_(4)Cl (aq) (pK_(b)=4.73) is equal to

pH of an aqueous solution of 0.6M NH_(3) and 0.4M NH_(4)Cl is 9.4 (pK_(b) = 4.74) . The new pH when 0.1M Ca(OH)_(2) solution is added to it.

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) )

"0.1 M" NH_(4)"OH & 0.01M "NH_(4)OH are taken. Which is a stronger base