A mixture of methanoic acid and sodium methanoate in aqueous solution acts as an acidic buffer solution. The equation shows the dissociation of methanoic acid. HCOOH(aq) ⇌ HCOO− (aq) + H+ (aq) Calculate the mass, in g, of sodium methanoate (HCOONa) that must be added to 25.0 cm3 of 0.100 mol dm−3 methanoic acid to produce a buffer solution with pH = 4.05 at 298 K For methanoic acid, pKa = 3.75 at 298 K
could someone break this down for me please? and the theory behind it.
Would really appreciate it.
Thanks!