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[" 45.If "pK(b)" for "CN^(-)" at "25^(@)...

[" 45.If "pK_(b)" for "CN^(-)" at "25^(@)C" is "4.7." The "pH" of "0.5M],[" aqueous "NaCN" solution is :- "],[[" (1) "12," (2) "10],[" (3) "11.5," (4) "11]]

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If pK_(a) for CN^(-) at 25^(@)C is 4.7, the pH of 0.5 M aqueous NaCN solution is

If Pk_b for CN^- at 25^@C is 4.7. Find the pH of 0.5 M aqueous NaCN solution,

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

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