Sulfuric Acid

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Gas phase thermochemistry data

Go To: Top, Reaction thermochemistry data, Henry's Law data, Gas phase ion energetics data, Mass spectrum (electron ionization), References, Notes

Data compilation copyright by the U.S. Secretary of Commerce on behalf of the U.S.A. All rights reserved.

Quantity Value Units Method Reference Comment
ΔfH°gas-735.13kJ/molReviewChase, 1998Data last reviewed in September, 1977
Quantity Value Units Method Reference Comment
S°gas,1 bar298.78J/mol*KReviewChase, 1998Data last reviewed in September, 1977

Gas Phase Heat Capacity (Shomate Equation)

Cp° = A + B*t + C*t2 + D*t3 + E/t2
H° − H°298.15= A*t + B*t2/2 + C*t3/3 + D*t4/4 − E/t + F − H
S° = A*ln(t) + B*t + C*t2/2 + D*t3/3 − E/(2*t2) + G
    Cp = heat capacity (J/mol*K)
    H° = standard enthalpy (kJ/mol)
    S° = standard entropy (J/mol*K)
    t = temperature (K) / 1000.

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Temperature (K) 298. to 1200.1200. to 6000.
A 47.28924139.2289
B 190.33149.513663
C -148.1299-1.795577
D 43.866310.118069
E -0.740016-15.61486
F -758.9525-813.0976
G 301.2961416.1854
H -735.1288-735.1288
ReferenceChase, 1998Chase, 1998
Comment Data last reviewed in September, 1977 Data last reviewed in September, 1977

Reaction thermochemistry data

Go To: Top, Gas phase thermochemistry data, Henry's Law data, Gas phase ion energetics data, Mass spectrum (electron ionization), References, Notes

Data compilation copyright by the U.S. Secretary of Commerce on behalf of the U.S.A. All rights reserved.

Data compiled as indicated in comments:
B - John E. Bartmess
MS - José A. Martinho Simões
M - Michael M. Meot-Ner (Mautner) and Sharon G. Lias
ALS - Hussein Y. Afeefy, Joel F. Liebman, and Stephen E. Stein

Note: Please consider using the reaction search for this species. This page allows searching of all reactions involving this species. A general reaction search form is also available. Future versions of this site may rely on reaction search pages in place of the enumerated reaction displays seen below.

Individual Reactions

HO4S- + Hydrogen cation = Sulfuric Acid

By formula: HO4S- + H+ = H2O4S

Quantity Value Units Method Reference Comment
ΔrH°1295. ± 23.kJ/molD-EAWang, Nicholas, et al., 2000gas phase; Lit BDE seems too weak. This plus Viggiano, Henchman, et al., 1992 gives BDE=106; B
ΔrH°1295. ± 11.kJ/molG+TSViggiano, Henchman, et al., 1992gas phase; B
ΔrH°1325.5kJ/molLattHouse Jr. and Kemper, 1987gas phase; From lattice energy of NH4HSO4, with new PA(NH3); B
ΔrH°<1319.6kJ/molG+TSVigiano, Perry, et al., 1980gas phase; I- + H2SO4 ->.; B
ΔrH°<1312. ± 8.4kJ/molEIAEAdams, Smith, et al., 1986gas phase; From H2SO4 (AP 0eV); B
Quantity Value Units Method Reference Comment
ΔrG°1265. ± 23.kJ/molH-TSWang, Nicholas, et al., 2000gas phase; Lit BDE seems too weak. This plus Viggiano, Henchman, et al., 1992 gives BDE=106; B
ΔrG°1265. ± 10.kJ/molIMRBViggiano, Henchman, et al., 1992gas phase; B
ΔrG°<1288.7kJ/molIMRBVigiano, Perry, et al., 1980gas phase; I- + H2SO4 ->.; B
ΔrG°<1281. ± 9.6kJ/molH-TSAdams, Smith, et al., 1986gas phase; From H2SO4 (AP 0eV); B

C2H5NaO (cr) + 0.5(Sulfuric Acid • 1100Water) (solution) = Ethanol (solution) + 0.5sodium sulphate (solution)

By formula: C2H5NaO (cr) + 0.5(H2O4S • 1100H2O) (solution) = C2H6O (solution) + 0.5Na2O4S (solution)

Quantity Value Units Method Reference Comment
ΔrH°-118.4 ± 3.8kJ/molRSCBlanchard, Joly, et al., 1974solvent: Sulphuric acid aqueous solution; The reaction enthalpy relies on -10.6 kJ/mol for the enthalpy of solution of EtOH(l) and on 9.97±0.04 for the enthalpy of solution of Na2SO4(cr) Blanchard, Joly, et al., 1974. A value of -490.8 ± 5.9 kJ/mol was derived in Blanchard, Joly, et al., 1974 for the enthalpy of formation. However, this value is affected by a calculation error. Also, the authors have not accounted for the acid dilution (this correction could not be made in the present database, due to lack of information). These problems were also noted in the data compilations Tel'noi and Rabinovich, 1980 and Wagman, Evans W.H., et al., 1982, where the values quoted for the enthalpy of formation, which rely on the experimental data reported in Blanchard, Joly, et al., 1974, are -410.0 ± 4.2 kJ/mol and -413.8 kJ/mol, respectively. See also comments in Liebman, Martinho Simões, et al., 1995; MS

(HO4S- • 2Sulfuric Acid) + HO3S = (HO4S- • HO3S • 2Sulfuric Acid)

By formula: (HO4S- • 2H2O4S) + HO3S = (HO4S- • HO3S • 2H2O4S)

Quantity Value Units Method Reference Comment
ΔrH°87.9kJ/molATMArnold and Qiu, 1984gas phase; Entropy change calculated or estimated; M
ΔrH°75.kJ/molATMArnold, Viggiano, et al., 1982gas phase; Entropy change calculated or estimated, DG>, ΔrH>; M
Quantity Value Units Method Reference Comment
ΔrS°100.J/mol*KN/AArnold and Qiu, 1984gas phase; Entropy change calculated or estimated; M
ΔrS°100.J/mol*KN/AArnold, Viggiano, et al., 1982gas phase; Entropy change calculated or estimated, DG>, ΔrH>; M

Free energy of reaction

ΔrG° (kJ/mol) T (K) Method Reference Comment
61.9250.ATMArnold and Qiu, 1984gas phase; Entropy change calculated or estimated; M
50.233.ATMArnold, Viggiano, et al., 1982gas phase; Entropy change calculated or estimated, DG>, ΔrH>; M

(HO4S- • 2Sulfuric Acid) + Sulfuric Acid = (HO4S- • 3Sulfuric Acid)

By formula: (HO4S- • 2H2O4S) + H2O4S = (HO4S- • 3H2O4S)

Quantity Value Units Method Reference Comment
ΔrH°87.0kJ/molATMArnold and Qiu, 1984gas phase; Entropy change calculated or estimated; M
ΔrH°82.8kJ/molATMArnold, Viggiano, et al., 1982gas phase; Entropy change calculated or estimated; M
Quantity Value Units Method Reference Comment
ΔrS°100.J/mol*KN/AArnold and Qiu, 1984gas phase; Entropy change calculated or estimated; M
ΔrS°100.J/mol*KN/AArnold, Viggiano, et al., 1982gas phase; Entropy change calculated or estimated; M

Free energy of reaction

ΔrG° (kJ/mol) T (K) Method Reference Comment
61.1250.ATMArnold and Qiu, 1984gas phase; Entropy change calculated or estimated; M
59.233.ATMArnold, Viggiano, et al., 1982gas phase; Entropy change calculated or estimated; M

(HO4S- • Water • 3Sulfuric Acid) + Water = (HO4S- • 2Water • 3Sulfuric Acid)

By formula: (HO4S- • H2O • 3H2O4S) + H2O = (HO4S- • 2H2O • 3H2O4S)

Quantity Value Units Method Reference Comment
ΔrH°54.4kJ/molATMArnold, Viggiano, et al., 1982gas phase; Entropy change calculated or estimated; M
Quantity Value Units Method Reference Comment
ΔrS°100.J/mol*KN/AArnold, Viggiano, et al., 1982gas phase; Entropy change calculated or estimated; M

Free energy of reaction

ΔrG° (kJ/mol) T (K) Method Reference Comment
30.233.ATMArnold, Viggiano, et al., 1982gas phase; Entropy change calculated or estimated; M

(H2O4S- • Sulfuric Acid) + HO3S = (H2O4S- • HO3S • Sulfuric Acid)

By formula: (H2O4S- • H2O4S) + HO3S = (H2O4S- • HO3S • H2O4S)

Quantity Value Units Method Reference Comment
ΔrH°92.5kJ/molATMArnold and Qiu, 1984gas phase; Entropy change calculated or estimated; M
Quantity Value Units Method Reference Comment
ΔrS°100.J/mol*KN/AArnold and Qiu, 1984gas phase; Entropy change calculated or estimated; M

Free energy of reaction

ΔrG° (kJ/mol) T (K) Method Reference Comment
66.5250.ATMArnold and Qiu, 1984gas phase; Entropy change calculated or estimated; M

(HO4S- • 2Sulfuric Acid) + Nitric acid = (HO4S- • Nitric acid • 2Sulfuric Acid)

By formula: (HO4S- • 2H2O4S) + HNO3 = (HO4S- • HNO3 • 2H2O4S)

Quantity Value Units Method Reference Comment
ΔrH°66.5kJ/molATMArnold, Viggiano, et al., 1982gas phase; Entropy change calculated or estimated; M
Quantity Value Units Method Reference Comment
ΔrS°100.J/mol*KN/AArnold, Viggiano, et al., 1982gas phase; Entropy change calculated or estimated; M

Free energy of reaction

ΔrG° (kJ/mol) T (K) Method Reference Comment
43.1233.ATMArnold, Viggiano, et al., 1982gas phase; Entropy change calculated or estimated; M

(HO4S- • 3Sulfuric Acid) + Nitric acid = (HO4S- • Nitric acid • 3Sulfuric Acid)

By formula: (HO4S- • 3H2O4S) + HNO3 = (HO4S- • HNO3 • 3H2O4S)

Quantity Value Units Method Reference Comment
ΔrH°70.7kJ/molATMArnold, Viggiano, et al., 1982gas phase; Entropy change calculated or estimated; M
Quantity Value Units Method Reference Comment
ΔrS°100.J/mol*KN/AArnold, Viggiano, et al., 1982gas phase; Entropy change calculated or estimated; M

Free energy of reaction

ΔrG° (kJ/mol) T (K) Method Reference Comment
46.4233.ATMArnold, Viggiano, et al., 1982gas phase; Entropy change calculated or estimated; M

(HO4S- • 2Sulfuric Acid) + Water = (HO4S- • Water • 2Sulfuric Acid)

By formula: (HO4S- • 2H2O4S) + H2O = (HO4S- • H2O • 2H2O4S)

Quantity Value Units Method Reference Comment
ΔrH°50.6kJ/molATMArnold, Viggiano, et al., 1982gas phase; Entropy change calculated or estimated; M
Quantity Value Units Method Reference Comment
ΔrS°100.J/mol*KN/AArnold, Viggiano, et al., 1982gas phase; Entropy change calculated or estimated; M

Free energy of reaction

ΔrG° (kJ/mol) T (K) Method Reference Comment
26.233.ATMArnold, Viggiano, et al., 1982gas phase; Entropy change calculated or estimated; M

(HO4S- • 3Sulfuric Acid) + Water = (HO4S- • Water • 3Sulfuric Acid)

By formula: (HO4S- • 3H2O4S) + H2O = (HO4S- • H2O • 3H2O4S)

Quantity Value Units Method Reference Comment
ΔrH°57.7kJ/molATMArnold, Viggiano, et al., 1982gas phase; Entropy change calculated or estimated; M
Quantity Value Units Method Reference Comment
ΔrS°100.J/mol*KN/AArnold, Viggiano, et al., 1982gas phase; Entropy change calculated or estimated; M

Free energy of reaction

ΔrG° (kJ/mol) T (K) Method Reference Comment
33.233.ATMArnold, Viggiano, et al., 1982gas phase; Entropy change calculated or estimated; M

(HO4S- • 4Sulfuric Acid) + Water = (HO4S- • Water • 4Sulfuric Acid)

By formula: (HO4S- • 4H2O4S) + H2O = (HO4S- • H2O • 4H2O4S)

Quantity Value Units Method Reference Comment
ΔrH°58.2kJ/molATMArnold, Viggiano, et al., 1982gas phase; Entropy change calculated or estimated; M
Quantity Value Units Method Reference Comment
ΔrS°100.J/mol*KN/AArnold, Viggiano, et al., 1982gas phase; Entropy change calculated or estimated; M

Free energy of reaction

ΔrG° (kJ/mol) T (K) Method Reference Comment
34.233.ATMArnold, Viggiano, et al., 1982gas phase; Entropy change calculated or estimated; M

(HO4S- • Sulfuric Acid) + Sulfuric Acid = (HO4S- • 2Sulfuric Acid)

By formula: (HO4S- • H2O4S) + H2O4S = (HO4S- • 2H2O4S)

Quantity Value Units Method Reference Comment
ΔrH°92.0kJ/molATMArnold and Qiu, 1984gas phase; Entropy change calculated or estimated; M
Quantity Value Units Method Reference Comment
ΔrS°100.J/mol*KN/AArnold and Qiu, 1984gas phase; Entropy change calculated or estimated; M

Free energy of reaction

ΔrG° (kJ/mol) T (K) Method Reference Comment
66.1250.ATMArnold and Qiu, 1984gas phase; Entropy change calculated or estimated; M

(HO4S- • 3Sulfuric Acid) + Sulfuric Acid = (HO4S- • 4Sulfuric Acid)

By formula: (HO4S- • 3H2O4S) + H2O4S = (HO4S- • 4H2O4S)

Quantity Value Units Method Reference Comment
ΔrH°77.4kJ/molATMArnold, Viggiano, et al., 1982gas phase; Entropy change calculated or estimated; M
Quantity Value Units Method Reference Comment
ΔrS°100.J/mol*KN/AArnold, Viggiano, et al., 1982gas phase; Entropy change calculated or estimated; M

Free energy of reaction

ΔrG° (kJ/mol) T (K) Method Reference Comment
54.233.ATMArnold, Viggiano, et al., 1982gas phase; Entropy change calculated or estimated; M

(HO4S- • 4Sulfuric Acid) + Sulfuric Acid = (HO4S- • 5Sulfuric Acid)

By formula: (HO4S- • 4H2O4S) + H2O4S = (HO4S- • 5H2O4S)

Quantity Value Units Method Reference Comment
ΔrH°79.1kJ/molATMArnold, Viggiano, et al., 1982gas phase; Entropy change calculated or estimated; M
Quantity Value Units Method Reference Comment
ΔrS°100.J/mol*KN/AArnold, Viggiano, et al., 1982gas phase; Entropy change calculated or estimated; M

Free energy of reaction

ΔrG° (kJ/mol) T (K) Method Reference Comment
54.233.ATMArnold, Viggiano, et al., 1982gas phase; Entropy change calculated or estimated; M

C2H5LiO (cr) + 0.5(Sulfuric Acid • 1100Water) (solution) = 0.5Li2O4S (solution) + Ethanol (solution)

By formula: C2H5LiO (cr) + 0.5(H2O4S • 1100H2O) (solution) = 0.5Li2O4S (solution) + C2H6O (solution)

Quantity Value Units Method Reference Comment
ΔrH°-113.6 ± 1.3kJ/molRSCBlanchard, Joly, et al., 1974solvent: Sulphuric acid aqueous solution; The reaction enthalpy relies on -10.6 kJ/mol for the enthalpy of solution of EtOH(l) and on -17.5±0.3 for the enthalpy of solution of Li2SO4(cr) Blanchard, Joly, et al., 1974.; MS

C2H5KO (cr) + 0.5(Sulfuric Acid • 1100Water) (solution) = Ethanol (solution) + 0.5K2O4S (solution)

By formula: C2H5KO (cr) + 0.5(H2O4S • 1100H2O) (solution) = C2H6O (solution) + 0.5K2O4S (solution)

Quantity Value Units Method Reference Comment
ΔrH°-132.3 ± 2.9kJ/molRSCBlanchard, Joly, et al., 1974solvent: Sulphuric acid aqueous solution; The reaction enthalpy relies on -10.6 kJ/mol for the enthalpy of solution of EtOH(l) and on 35.1±0.1 for the enthalpy of solution of K2SO4(cr) Blanchard, Joly, et al., 1974.; MS

Dimethylzinc (l) + (Sulfuric Acid • 100Water) (solution) = 2Methane (g) + (zinc sulphate • 100Water) (solution)

By formula: C2H6Zn (l) + (H2O4S • 100H2O) (solution) = 2CH4 (g) + (O4SZn • 100H2O) (solution)

Quantity Value Units Method Reference Comment
ΔrH°-341.8 ± 0.8kJ/molRSCCarson, Hartley, et al., 1949Please also see Pedley and Rylance, 1977 and Cox and Pilcher, 1970.; MS

Diethylzinc (l) + (Sulfuric Acid • 100Water) (solution) = 2Ethane (g) + (zinc sulphate • 100Water) (solution)

By formula: C4H10Zn (l) + (H2O4S • 100H2O) (solution) = 2C2H6 (g) + (O4SZn • 100H2O) (solution)

Quantity Value Units Method Reference Comment
ΔrH°-354.4 ± 4.2kJ/molRSCCarson, Hartley, et al., 1949Please also see Pedley and Rylance, 1977 and Cox and Pilcher, 1970.; MS

Dodecane + Sulfuric Acid = C12H26O3S + Water

By formula: C12H26 + H2O4S = C12H26O3S + H2O

Quantity Value Units Method Reference Comment
ΔrH°290. ± 17.kJ/molCmRoth and Rist-Schumacher, 1944liquid phase; ALS

Propene + Sulfuric Acid = isopropyl hydrogen sulphate

By formula: C3H6 + H2O4S = isopropyl hydrogen sulphate

Quantity Value Units Method Reference Comment
ΔrH°-38. ± 0.8kJ/molEqkEntelis, Korovina, et al., 1960liquid phase; ALS

Henry's Law data

Go To: Top, Gas phase thermochemistry data, Reaction thermochemistry data, Gas phase ion energetics data, Mass spectrum (electron ionization), References, Notes

Data compilation copyright by the U.S. Secretary of Commerce on behalf of the U.S.A. All rights reserved.

Data compiled by: Rolf Sander

Henry's Law constant (water solution)

kH(T) = k°H exp(d(ln(kH))/d(1/T) ((1/T) - 1/(298.15 K)))
k°H = Henry's law constant for solubility in water at 298.15 K (mol/(kg*bar))
d(ln(kH))/d(1/T) = Temperature dependence constant (K)

k°H (mol/(kg*bar)) d(ln(kH))/d(1/T) (K) Method Reference Comment
1.×10+11 MN/AValue derived from partial pressure of H2SO4 over a concentrated solution. This can only be considered an order-of-magnitude approximation. The solubility at lower aqueous-phase concentrations should be larger.
5.×10+14 MN/AValue derived from partial pressure of H2SO4 over a concentrated solution. This can only be considered an order-of-magnitude approximation. The solubility at lower aqueous-phase concentrations should be larger.

Gas phase ion energetics data

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Data compilation copyright by the U.S. Secretary of Commerce on behalf of the U.S.A. All rights reserved.

Data evaluated as indicated in comments:
HL - Edward P. Hunter and Sharon G. Lias

Data compiled as indicated in comments:
B - John E. Bartmess
MM - Michael M. Meot-Ner (Mautner)
LL - Sharon G. Lias and Joel F. Liebman

Quantity Value Units Method Reference Comment
Proton affinity (review)699.4kJ/molN/AHunter and Lias, 1998HL
Quantity Value Units Method Reference Comment
Gas basicity666.9kJ/molN/AHunter and Lias, 1998HL
Quantity Value Units Method Reference Comment
ΔfH°(+) ion500. ± 20.kJ/molN/AN/A 

Gas basicity at 298K

Gas basicity (review) (kJ/mol) Reference Comment
683. ± 5.Do, Klein, et al., 1998T = T(eff) = 800 - 1250K; H2S; H2CO. ΔGB values from kinetic bracketing were extrapolated to 298 K. ΔSp from ab initio rot. and vib. constants; MM
≥680.Do, Klein, et al., 1998MM

Protonation entropy at 298K

Protonation entropy (J/mol*K) Reference Comment
4.9Do, Klein, et al., 1998T = T(eff) = 800 - 1250K; H2S; H2CO. ΔGB values from kinetic bracketing were extrapolated to 298 K. ΔSp from ab initio rot. and vib. constants; MM

Ionization energy determinations

IE (eV) Method Reference Comment
12.40 ± 0.05EISnow and Thomas, 1990LL

Appearance energy determinations

Ion AE (eV) Other Products MethodReferenceComment
HSO3+13.9 ± 0.1HOEISnow and Thomas, 1990LL
H2O+13.2 ± 0.2SO3EISnow and Thomas, 1990LL
SO2+15.97 ± 0.15H2O2EISnow and Thomas, 1990LL
SO3+13.8 ± 0.2H2OEISnow and Thomas, 1990LL

De-protonation reactions

HO4S- + Hydrogen cation = Sulfuric Acid

By formula: HO4S- + H+ = H2O4S

Quantity Value Units Method Reference Comment
ΔrH°1295. ± 23.kJ/molD-EAWang, Nicholas, et al., 2000gas phase; Lit BDE seems too weak. This plus Viggiano, Henchman, et al., 1992 gives BDE=106; B
ΔrH°1295. ± 11.kJ/molG+TSViggiano, Henchman, et al., 1992gas phase; B
ΔrH°1325.5kJ/molLattHouse Jr. and Kemper, 1987gas phase; From lattice energy of NH4HSO4, with new PA(NH3); B
ΔrH°<1319.6kJ/molG+TSVigiano, Perry, et al., 1980gas phase; I- + H2SO4 ->.; B
ΔrH°<1312. ± 8.4kJ/molEIAEAdams, Smith, et al., 1986gas phase; From H2SO4 (AP 0eV); B
Quantity Value Units Method Reference Comment
ΔrG°1265. ± 23.kJ/molH-TSWang, Nicholas, et al., 2000gas phase; Lit BDE seems too weak. This plus Viggiano, Henchman, et al., 1992 gives BDE=106; B
ΔrG°1265. ± 10.kJ/molIMRBViggiano, Henchman, et al., 1992gas phase; B
ΔrG°<1288.7kJ/molIMRBVigiano, Perry, et al., 1980gas phase; I- + H2SO4 ->.; B
ΔrG°<1281. ± 9.6kJ/molH-TSAdams, Smith, et al., 1986gas phase; From H2SO4 (AP 0eV); B

Mass spectrum (electron ionization)

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Data compilation copyright by the U.S. Secretary of Commerce on behalf of the U.S.A. All rights reserved.

Data compiled by: NIST Mass Spectrometry Data Center, William E. Wallace, director

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References

Go To: Top, Gas phase thermochemistry data, Reaction thermochemistry data, Henry's Law data, Gas phase ion energetics data, Mass spectrum (electron ionization), Notes

Data compilation copyright by the U.S. Secretary of Commerce on behalf of the U.S.A. All rights reserved.

Chase, 1998
Chase, M.W., Jr., NIST-JANAF Themochemical Tables, Fourth Edition, J. Phys. Chem. Ref. Data, Monograph 9, 1998, 1-1951. [all data]

Wang, Nicholas, et al., 2000
Wang, X.B.; Nicholas, J.B.; Wang, L.S., Photoelectron spectroscopy and theoretical calculations of SO4- and HSO4-: Confirmation of high electron affinities of SO4 and HSO4, J. Phys. Chem. A, 2000, 104, 3, 504-508, https://doi.org/10.1021/jp992726r . [all data]

Viggiano, Henchman, et al., 1992
Viggiano, A.A.; Henchman, M.J.; Dale, F.; Deakyne, C.A.; Paulson, J.F., Gas-Phase Reactions of Weak Bronsted Bases I-, PO3-, HSO4-, FSO3-, and CF3SO3- with Strong Bronsted Acids H2SO4, FSO3H, and CF3SO3H - A Quantitative Study, J. Am. Chem. Soc., 1992, 114, 11, 4299, https://doi.org/10.1021/ja00037a039 . [all data]

House Jr. and Kemper, 1987
House Jr.; Kemper, K.A., Proton Affinities of Sulfate and Bisulfate Ions, J. Thermal Anal., 1987, 32, 6, 1855, https://doi.org/10.1007/BF01913977 . [all data]

Vigiano, Perry, et al., 1980
Vigiano, A.A.; Perry, R.A.; Albritton, D.L.; Ferguson, E.E.; Fehsenfeld, F.C., The role of H2SO4 in stratospheric negative ion chemistry, J. Geophys. Res., 1980, 85, 4551. [all data]

Adams, Smith, et al., 1986
Adams, N.G.; Smith, D.; Viggiano, A.A.; Paulson, J.F.; Henchman, M.J., Dissociative attachment reactions of electron with strong acid molecules, J. Chem. Phys., 1986, 84, 6728. [all data]

Blanchard, Joly, et al., 1974
Blanchard, J.M.; Joly, R.D.; Lettoffe, J.M.; Perachon, G.; Thourey, J., J. Chim. Phys. Phys.-Chim. Biol., 1974, 71, 472. [all data]

Tel'noi and Rabinovich, 1980
Tel'noi, V.I.; Rabinovich, I.B., Russ. Chem. Rev., 1980, 49, 603. [all data]

Wagman, Evans W.H., et al., 1982
Wagman, D.D.; Evans W.H.; Parker, V.B.; Schumm, R.H.; Halow, I.; Bailey, S.M.; Churney, K.L.; Nuttall, R.L., The NBS Tables of Chemical Thermodynamic Properties; J. Phys. Chem. Ref. Data, 1982, 11, Suppl. 2. [all data]

Liebman, Martinho Simões, et al., 1995
Liebman, J.F.; Martinho Simões, J.A.; Slayden, S.W., In Lithium Chemistry: A Theoretical and Experimental Overview Wiley: New York, Sapse, A.-M.; Schleyer, P. von Ragué, ed(s)., 1995. [all data]

Arnold and Qiu, 1984
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Arnold, Viggiano, et al., 1982
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Carson, Hartley, et al., 1949
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Pedley and Rylance, 1977
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Cox and Pilcher, 1970
Cox, J.D.; Pilcher, G., Thermochemistry of Organic and Organometallic Compounds in Academic Press, New York, 1970. [all data]

Roth and Rist-Schumacher, 1944
Roth, W.A.; Rist-Schumacher, E., Beitrag zur thermochemie der sulfonsauren und saurechlorid, Z. Electrochem., 1944, 50, 7-9. [all data]

Entelis, Korovina, et al., 1960
Entelis, S.G.; Korovina, G.V.; Chirkov, N.M., The thermodynamics of propylene absorption by the H2SO4-H20 system, Dokl. Akad. Nauk SSSR, 1960, 134, 856-859. [all data]

Hunter and Lias, 1998
Hunter, E.P.; Lias, S.G., Evaluated Gas Phase Basicities and Proton Affinities of Molecules: An Update, J. Phys. Chem. Ref. Data, 1998, 27, 3, 413-656, https://doi.org/10.1063/1.556018 . [all data]

Do, Klein, et al., 1998
Do, K.; Klein, T.P.; Pommering, C.A.; Bachrach, S.M.; Sunderlin, L.S., The gas-phase basicity of sulfuric acid, J. Am. Chem. Soc., 1998, 120, 6093. [all data]

Snow and Thomas, 1990
Snow, K.B.; Thomas, T.F., Mass spectrum, ionization potential, and appearance potentials for fragment ions of sulfuric acid vapor, Int. J. Mass Spectrom. Ion Processes, 1990, 96, 49. [all data]

Notes

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