A `0.25 M` solution of pyridinium chloride `C_(5)H_(5)NH^(+)Cl^(-)` was found to have a `pH` of `2.75` What is `K_(b)` for pyridine, `C_(5)H_(5)N`?

A 0.25 M solution of pyridinium chloride, C_(5)H_(5)NH^(+)Cl^(-) , was found to have a pH of 2.89 . What is the K_(b) for pyridine, C_(5)H_(5)N ?

A 0.25M solution of pyridinium chloride (C_(5)H_(5)overset(o+)NHCl^(Theta)) has pH of 2.89 . Calculate pK_(b) for pyridine (C_(5)H_(5)N) .

A 0.25M solution of pyridinium chloride (C_(5)H_(5)overset(o+)NHC1^(Theta)) has pH of 2.89 . Calculate pK_(b) for pyridine (C_(5)H_(5)N) .

Equilibrium constant for the following reaction is 1xx10^(-9) : C_(5)H_(5)N(aq.)+H_(2)O(l)hArrC_(5)H_(5)NH^(+)(aq.)+OH^(-)(aq.) Determine the moles of pyridinium chloride (C_(5)H_(5)N.HCl) that should be added t0 500 mL solution of 0.4 M pyridine (C_(5)H_(5)N) to obtain a buffer solution of pH=5 :

Equilibrium constant for the following reaction is 1xx10^(-9) : C_(5)H_(5)N(aq.)+H_(2)O(l)hArrC_(5)H_(5)NH^(+)(aq.)+OH^(-)(aq.) Determine the moles of pyridinium chloride (C_(5)H_(5)N.HCL) is added to 500ml of 0.4M of pyridine (C_(5)H_(5)N) obtain a buffer solution of pH=5 :

0.15 mol of pyridinium chloride is added to 500 mL 0.2 (M) pyridine solution. Determine the pH of the solution. Given: K_(b) (pyridine) =1.5xx10^(-9) and assume that volume of the solution does not change due to the addition of pyridinium chloride.

The pH of 0.02 M solution of ammonium chloride at 25^@C is [ k_b(NH_3)=1.8xx10^-5]

The percentage of pyridine (C_(5)H_(5)N) that forms pyridinium ion (C_(5)H_(5)N^(+)H) in a 0.10 M aqueous pyridine solution ( K_(b) for C_(5)H_(5)N=1.7xx10^(-9) ) is

The percentage of pyridine (C_(5)H_(5)N) that forms pyridinium ion (C_(5)H_(5)N^(+)H) in a 0.10 M aqueous pyridine solution ( K_(b) for C_(5)H_(5)N=1.7xx10^(-9) ) is

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