Equal volume of 0.02M each solution of HCl(aq) and `NH_(3)(aq)` are mixed. Calculate pH of resultant solution at `25^(@)C`
(`K_(b)``(NH_(3))`=`10^(-5)`)

Equal volumes of two HCl solutions of pH=3 and pH=5 were mixed. What is the Ph of the resulting solution ?

Equal volums of solutions pH values 1,3,5,6 are mixed with each other . The pH of resultant solution is nearly

Equal volume of 0.2M NH_(4)OH (or ammonia) are 0.1MH_(2)SO_(4) are mixed.Calculated pH of final solution.Given : K_(b) of NH_(3)=1.8xx10^(-5) at 25^(@)C .

Calculate the pH of a 2.0 M solution of NH_4Cl. [K_b(NH_3)= 1.8 xx 10^(-5)]

What is pH of 0.02 M solution of ammonium chloride at 25^(@) C ? K_(b) (NH_(3)) = 1.8 xx 10^(-5) .

When NH_(3)(0.1 M) 50 ml mix with HCl (0.1 M) 10 ml then what is pH of resultant solution ( pK_(b)=4.75)

In what volume ratio should you mix 1.0 M solution of NH_(4)CI and NH_(3) to produce a buffer solution of pH 9.80 [pK_(b) (NH_(3)) = 4.74]