A1.00 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 100.0 ml of 1.00 m hcl. the ka for hf is 3.5 × 10-4.

pH = 3.09

Explanation:

Solve this problem using the Henderson-Hasselbach formula  after calculating the changes in the buffer following the addition of  HCl. The addition of the acid consumes the conjugate base in a one to one reaction. The moles present are calculated by multiplying the molarity by the volume in liters.

R:      HF                          ⇆   H⁺            +       F⁻

I:  0.250 mol                                             0.250  mol

C:+ 0.100 mol                                           -0.100   mol

E:  0.350   mol                                           0.150   mol

pH = pKa + log ( (F⁻) /(HF))

pH = -log ( 3.5 x 10 ⁻⁴)  + log ( 0.15/ 0.35)

pH =   3.46   +  ( -0.37 ) = 3.09

Note: Here we do not need to calculate the change in concentrations since the volume appears in the ratio and cancel themselves.

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