A 1.50 L buffer solution is 0.250 M in HF and 0.250 M in NaF. Calculate...

A 1.50 L buffer solution is 0.250 M in HF and 0.250 M in NaF. Calculate the pH of the solution after the addition of 0.0500 moles of solid NaOH. Assume no volume change upon the addition of base. The K_a for HF is 3.5 × 10^-4.

Expert Solution

no of moles of HF = molarity * volume in L

= 0.25*1.5 = 0.375 moles

no of moles of NaF = molarity * volume in L

= 0.25*1.5 = 0.375 moles

By the addition of NaOH

no of moles of HF = 0.375-0.05 = 0.325 moles

no of moles of NaF = 0.375 + 0.05 = 0.425 moles

Pka = -logKa

= -log3.5*10^-4 = 3.4559

PH = PKa + log[NaF]/[HF]

= 3.4559 + log0.425/0.325

= 3.4559 + 0.1165 = 3.5724

queen_honey_blossom answered 1 year ago

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