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A 1.00 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.

Respuesta :

baraltoa

Answer:

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.

okpalawalter8

The pH of the solution  is mathematically given as

pH= 3.09

The pH of the solution

Question Parameters:

Generally the equation for the Chemical Reaction  is mathematically given as

[tex]HF \rightarrow H+ +F-[/tex]

Therefore

pH = pKa + log ( (F⁻) /(HF))

pH = -log ( 3.5 x 10^{-4})  + log ( 0.15/ 0.35)

pH =   3.46   +  ( -0.37 )

pH= 3.09

For more information on Chemical Reaction

https://brainly.com/question/11231920

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