stads_29 Posted October 1, 2009 Share Posted October 1, 2009 Hey, have this question which i just cant wrap my head around, any help would be appreciated. Formic Acid (HCOOH) - pKa = 3.8 is a weak acid that partially dissociates to form its conjugate base (HCOO-) and releases protons into aqueous solutions. Whats the pH of a solution in which (HCOOH) = .7M and (HCOO-) = .15M? Then, if the pH of sol. of Formic acid has been titrated to a final pH of 2.8, Whats the ratio of conjugate base : Weak acid? And suppose your given stock solutions of formic acid and sodium salt of the conjugate base : (HCOOH) = 3.OM and (HCOONa) = 1.5M, How would you make a .1 M buffer(total formic acid + sodium formate concentration), 100mL total at pH 3.5, using above solutions? Link to comment Share on other sites More sharing options...
Rusty123 Posted October 3, 2009 Share Posted October 3, 2009 I would use the Henderson Hasselback Equation for the first 2 questions in your problem. Link to comment Share on other sites More sharing options...
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