" 13.ph of a "0.5" M aqueous NaCN solution "(pK_(b)" of "CN^(-)=4.70)" ,is "

What is the pH of a 0.50M aqueous NaCN solution ? (pK_(b)of CN^(-)=4.70)

What is the pH of a 0.50M aqueous NaCN solution ? (pK_(b)of CN^(-)=4.70)

pH of 0.5 M aqueous NaCN solution is (pK_a of HCN = 9.3, log 5 = 0.7)

The pH of 0.2 M aqueous solution of NH_4Cl will be (pK_b of NH_4OH = 4.74, log 2 = 0.3)

The pH of basic buffer mixtures is given by : pH=pK_(a)+log((["Base"])/(["Salt"])) , whereas pH of acidic buffer mixtures is given by: pH= pK_(a)+log((["Salt"])/(["Acid"])) . Addition of little acid or base although shows no appreciable change for all practical purpose, but since the ratio (["Base"])/(["Salt"]) or (["Salt"])/(["Acid"]) change, a slight decrease or increase in pH results in. Mole of HCI required to prepare a buffer solution of pH=8.5 with 0.1 mole of NaCN in one litre solution is: (pK_(a) for CN^(-)=4.61)