What amount of `HCl` will be required to prepare one litre of a buffer solution of `pH 10.4` using `0.01` mole of `NaCN`? Given `K_(ion)(HCN)=4.1xx10^(-10)`.

How many mole of HCI will be required to prepare one litre of buffer solution (containing NaCN+ HCI ) of pH 8.5 using 0.01 g formula weight of NaCN ? K_(HCN)=4.1xx10^(-10))

How many mole of HCl are required to prepare one litre of buffer solution (conataining NaCN+HCl) of ph 8.5 using 0.01 g formula weight of NaCN(K_(HCN)=4.1xx10^(-10)?

How many gram moles of HCI will be required to prepare 1L of buffer solution (containing NaCN and HCI) of pH 8.5 using 0.01g formula weight of NaCN gt K_(HCN) = 4.1 xx 10^(-10) .

How many moles of HCl will be required to preapare one litre of a buffer solution (containing NaCN and HCN) of pH 8.5 using 0.01 gram formula mass of NaCN . K_a for HCN = 4.1 xx 10^(-10)?

How many gram-mole of HCl will be required to prepare one litre of buffer solution (containing NaCN and HCN) of pH 8.5 using 0.01g formula weight of NaCN?

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)

Calculate the solubility og AgCN in a buffer solution of pH 3.00 K_(sp(AgCN)) = 1.2 xx10^(-18) and K_(a(HCN)) = 4.8 xx 10^(10) M^(2) .