## HNO3 (aq) + 1 NaOH (aq) → NaNO3 (aq) + H2O (ℓ)

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## Stoichiometry

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 HNO3           Mass: g or Solution Volume: mL of Concentration: mol/L NaOH           Mass: g or Solution Volume: mL of Concentration: mol/L NaNO3          Mass: g H2O            Mass: g Heat Released: kJ

## Enthalpy of Reaction

[1ΔHf(NaNO3 (aq)) + 1ΔHf(H2O (ℓ))] - [1ΔHf(HNO3 (aq)) + 1ΔHf(NaOH (aq))]
[1(-447.46) + 1(-285.83)] - [1(-207.36) + 1(-470.09)] = -55.8399999999999 kJ
-55.84 kJ     (exothermic)

## Entropy Change

[1ΔSf(NaNO3 (aq)) + 1ΔSf(H2O (ℓ))] - [1ΔSf(HNO3 (aq)) + 1ΔSf(NaOH (aq))]
[1(205.44) + 1(69.91)] - [1(146.44) + 1(48.25)] = 80.66 J/K
80.66 J/K     (increase in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[1ΔGf(NaNO3 (aq)) + 1ΔGf(H2O (ℓ))] - [1ΔGf(HNO3 (aq)) + 1ΔGf(NaOH (aq))]
[1(-373.24) + 1(-237.18)] - [1(-111.34) + 1(-419.18)] = -79.9000000000001 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 77.