Calculate the pH of 1.0 L of 0.10 M pyridine solution to which 0.3 mol of pyridinium chloride `C_5H_5NH^+Cl`, has been added, assuming no change in volume.

0.15 mole of pyridinium chloride has been added into 500 cm^(3) of 0.2M pyridine solution. Calculate pH and hydroxyl ion contration in the resulting solution, assuming no change in volume. (K_(b)"for pyridine" = 1.5xx10^(-9)M)

0.15 mole of pyridinium chloride has been added into 500 cm^(3) of 0.2M pyridine solution. Calculate pH and hydroxyl ion contration in the resulting solution, assuming no change in volume. (K_(b)"for pyridine" = 1.5xx10^(-9)M)

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

0.15 mole of pyridinium chloride has been added into 500 cm^(3) of 0.2 M pyridine solution. Calculate pH of the resulting solution, assuming no change in volume. (K, for pyridine = 1.5 xx 10^(-9) M)

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 2.75 What is K_(b) for pyridine, C_(5)H_(5)N ?