How much Sodium Formate (HCOONa 68.01 g/mol) do you need to add to 400. mL of 1.00 M Formic Acid for a pH 3.5 buffer. Ka=1.77e-4
:pH = pKa + log (base/acid) 3.5 = 3.752 + log (x/1) (that 1 comes from the 1.00 M formic acid) log x = -0.252 x = 0.560 M (this is the molarity of the formate that is required) MV = g/molar mass (0.560) (0.400) = x / 68.0069 x = 15.3
is it possible to do this probleem without using the hendersen hasselbach's formula??? If so, how do you do it help pls
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