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How many mole of HCI will be required t...

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))`

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The correct Answer is:
0.0088 mole
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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) .

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) .

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One litre of a buffer solution contains 0.1 M NH_(4)OH . The p^(kb) of base is 5.pH value of the solution is

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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 pH of a buffer solution containing 0.1 mole of acetic acid and 0.15 mole of sodium acetate. K_(c) for acetic acid is 1.75 xx 10^(-5) .

Which species has the lowest concentration in a solution prepared mixing 0.1 mole each of HCN and NaCN in 1L solution ? K_(a) (HCN)=10^(-10)

RC MUKHERJEE-IONIC EQUILIBRIUM IN AQUEOUS SOLUTIONS-Problems
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