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30 January, 10:51

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.

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  1. 30 January, 11:05
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    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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