## HF (aq) + 1 KOH (aq) → KF (aq) + H2O (ℓ)

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## Reaction Type:

Double Displacement

## Stoichiometry

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 HF             Mass: g or Solution Volume: mL of Concentration: mol/L KOH            Mass: g or Solution Volume: mL of Concentration: mol/L KF             Mass: g H2O            Mass: g Heat Released: kJ

## Enthalpy of Reaction

[1ΔHf(KF (aq)) + 1ΔHf(H2O (ℓ))] - [1ΔHf(HF (aq)) + 1ΔHf(KOH (aq))]
[1(-508.04) + 1(-285.83)] - [1(-255.64) + 1(-482.39)] = -55.8399999999999 kJ
-55.84 kJ     (exothermic)

## Entropy Change

[1ΔSf(KF (aq)) + 1ΔSf(H2O (ℓ))] - [1ΔSf(HF (aq)) + 1ΔSf(KOH (aq))]
[1(247.98) + 1(69.91)] - [1(145.48) + 1(91.75)] = 80.66 J/K
80.66 J/K     (increase in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(KF (aq)) + 1ΔGf(H2O (ℓ))] - [1ΔGf(HF (aq)) + 1ΔGf(KOH (aq))]
[1(-545.64) + 1(-237.18)] - [1(-262.34) + 1(-440.58)] = -79.8999999999999 kJ
-79.90 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-79.89 kJ     (spontaneous)

## Equilibrium Constant, K (at 298.15 K)

9.969038464e+013
This process is favorable at 25°C.

## Reference(s):

Ebbing, Darrell D. General Chemistry 3rd ed.; Houghton Mifflin Company: Boston, MA, 1990; p 98.