Sodium Hydroxide Specific Heat Capacity



Specific heat for some common liquids and fluids - acetone, oil, paraffin, water and many more

  1. Equal volumes, 50.0 mL, of 3.0 M hydrochloric acid and 3.0 M sodium hydroxide solutions having an initial temperature of 20.0°C react in a calorimeter. The resultant solution records a temperature of 40.0°C. The heat gained by the resultant solution can be calculated using.
  2. Determination of Heat Capacity. Introduction: The purpose of this experiment was to determine the heat capacity of an adiabatic calorimeter. An adiabatic calorimeter is an apparatus used to measure heat changes for experiments done at constant pressure. Heat capacity is the amount of heat required to raise the heat of a system one degree.

The specific heat for some commonly used liquids and fluids is given in the table below.

The specific heat for some commonly used liquids and fluids is given in the table below. For conversion of units, use the Specific heat online unit converter. See also tabulated values of specific heat of gases, food and foodstuff, metals and semimetals, common solids and other common substances as well as values of molar specific heat of common organic substances and inorganic substances.

For conversion of units, use the Specific heat online unit converter.

See also tabulated values of specific heat of gases, food and foodstuff, metals and semimetals, common solids and other common substances as well as values of molar specific heat of common organic substances and inorganic substances.

ProductSpecific Heat
- cp -
(kJ/(kg K))(Btu/(lb oF))
(Kcal/kg oC)
Acetic acid2.0430.49
Acetone2.150.51
Alcohol, ethyl 32oF (ethanol)2.30.548
Alcohol, ethyl 104oF (ethanol)2.720.65
Alcohol, methyl. 40 - 50oF2.470.59
Alcohol, methyl. 60 - 70oF2.510.6
Alcohol, propyl2.370.57
Ammonia, 32oF4.61.1
Ammonia, 104oF4.861.16
Ammonia, 176oF5.41.29
Ammonia, 212oF6.21.48
Ammonia, 238oF6.741.61
Aniline2.180.514
Benzene, 60oF1.80.43
Benzene, 150oF1.920.46
Benzine2.1
Benzol1.80.43
Bismuth, 800oF0.150.0345
Bismuth, 1000oF0.1550.0369
Bismuth, 1400oF0.1650.0393
Bromine0.470.11
n-Butane, 32oF2.30.55
Calcium Chloride3.060.73
Carbon Disulfide0.9920.237
Carbon Tetrachloride0.8660.207
Castor Oil1.80.43
Chloroform1.050.251
Citron Oil1.840.44
Decane2.210.528
Diphenylamine1.930.46
Dodecane2.210.528
Dowtherm1.550.37
Ether2.210.528
Ethyl ether2.220.529
Ethylene glycol2.360.56
Dichlorodifluoromethane R-12 saturated -40oF0.880.211
Dichlorodifluoromethane R-12 saturated 0oF0.910.217
Dichlorodifluoromethane R-12 saturated 120oF1.020.244
Fuel Oil min.1.670.4
Fuel Oil max.2.090.5
Gasoline2.220.53
Glycerine2.430.576
Heptane2.240.535
Hexane2.260.54
Hydrochlor acid3.14
Iodine2.150.51
Kerosene2.010.48
Linseed Oil1.840.44
Light Oil, 60oF1.80.43
Light Oil, 300oF2.30.54
Mercury0.140.03
Methyl alcohol2.51
Milk3.930.94
Naphthalene1.720.41
Nitric acid1.72
Nitro benzole1.520.362
Octane2.150.51
Oil, Castor1.970.47
Oil, Olive1.970.47
Oil, mineral1.670.4
Oil, turpentine1.8
Oil, vegetable1.670.4
Olive oil1.970.47
Paraffin2.130.51
Perchlor ethylene0.905
Petroleum2.130.51
Petroleum ether1.76
Phenol1.430.34
Potassium hydrate3.680.88
Propane, 32oF2.40.576
Propylene2.850.68
Propylene Glycol2.50.60
Sesame oil1.630.39
Sodium, 200oF1.380.33
Sodium, 1000oF1.260.3
Sodium hydrate3.930.94
Soya bean oil1.970.47
Sulfuric acid concentrated1.38
Sulfuric acid1.34
Toluene1.720.41
Trichlor ethylene1.30
Tuluol1.510.36
Turpentine1.720.411
Water, fresh4.191
Water, sea 36oF3.930.938
Xylene1.720.41
  • 1 kJ/(kg K) = 1000 J/(kgoC) = 0.2389 kcal/(kg oC) = 0.2389 Btu/(lbmoF)
  • T(oC) = 5/9[T(oF) - 32]

For conversion of units, use the Specific heat online unit converter.

See also tabulated values of specific heat of Gases, Food and foodstuff, Metals and semimetals, Common solids and other Common substances.

Heating Energy

The energy required to heat a product can be calculated as

q = cp m dt (1)

where

q = heat required (kJ)

cp = specific heat (kJ/kg K, kJ/kg oC)

dt = temperature difference (K, oC)

Example - Required Heat to increase Temperature i Water

10 kg of water is heated from 20 oC to 100 oC - a temperature difference 80 oC (K). The heat required can be calculated as

q = (4.19 kJ/kg K) (10 kg) (80 oC)

= 3352 kJ

Related Topics

  • Material Properties - Material properties for gases, fluids and solids - densities, specific heats, viscosities and more
  • Thermodynamics - Effects of work, heat and energy on systems

Related Documents

  • Ammonia - Density at Varying Temperature and Pressure - Online calculator, figures and tables showing density and specific weight of ammonia at temperatures ranging -50 to 425 °C (-50 to 800 °F) at atmospheric and higher pressure - Imperial and SI Units
  • Ammonia - Dynamic and Kinematic Viscosity - Online calculator, figures and tables showing dynamic (absolute) and kinematic viscosity of gasous and liquid ammonia at temperatures ranging from -73 to 425°C (-100 to 800°F) at pressure ranging from 1 to 1000 bara (14.5 - 14500 psia) - SI and Imperial Units
  • Ammonia - Properties at Gas-Liquid Equilibrium Conditions - Figures and tables showing how the properties of liquid and gaseous ammonia changes along the boiling/condensation curve (temperature and pressure between triple point and critical point conditions). An ammonia phase diagram are included.
  • Ammonia - Specific Heat at varying Temperature and Pressure - Online calculator, figures and tables showing specific heat, CP and CV, of gasous and liquid ammonia at temperatures ranging from -73 to 425°C (-100 to 800°F) at pressure ranging from 1 to 100 bara (14.5 - 1450 psia) - SI and Imperial Units
  • Ammonia - Thermal Conductivity at Varying Temperature and Pressure - Online calculator, figures and tables showing thermal conductivity of liquid and gaseous ammonia at temperatures ranging -70 to 425 °C (-100 to 800 °F) at atmospheric and higher pressure - Imperial and SI Units
  • Ammonia - Thermophysical Properties - Chemical, Physical and Thermal Properties of Ammonia. Phase diagram included.
  • Ammonia - Vapour Pressure at gas-liquid equilibrium - Figures and table showing ammonia saturation pressure at boiling point, SI and Imperial units
  • Electric Heating of a Mass - Electric heating of an object or mass - energy supply and temperature change
  • Heat Capacity - The heat capacity of a substance is the amount of heat required to change its temperature by one degree, and has units of energy per degree
  • Heat Emission from Pipes Submerged in Oil or Fat - Heat emission from steam or water heating pipes submerged in oil or fat - forced and natural circulation
  • Heat Up Applications - Energy Required and Heat Transfer Rates - Energy required to heat up a substance
  • Light Oil Suction Flow Velocity - Recommended suction flow velocity when pumping light oils
  • Liquid ammonia - Thermal Properties at saturation pressure - Density, specific heat, thermal conductivity, viscosity and Prandtls no. of liquid ammonia at its saturation pressure
  • Mixing Fluids - Final mass and temperature when mixing fluids
  • Mixing Liquids and/or Solids - Final Temperatures - Calculate the final temperature when liquids or solids are mixed
  • Oil Tanks Heat Loss - Heat loss from lagged and unlagged, sheltered and exposed oil tanks
  • Polymers - Specific Heats - Specific heat of polymers like epoxy, PET, polycarbonate and more
  • Specific Heat - Online Unit Converter - Online specific heat converter with the most commonly used units
  • Specific Heat and Individual Gas Constants of Gases - Specific heat at constant volume, specific heat at constant pressure, specific heat ratio and individual gas constant - R - common gases as argon, air, ether, nitrogen and many more ..
  • Specific Heat of Food and Foodstuff - Specific heat of common food and foodstuff like apples, bass, beef, pork and many more
  • Specific Heat of Solids - Common solids - like brick, cement, glass and many more - and their specific heats - in Imperial and SI units
  • Steel Pipes and Temperature Expansion - Temperature expansion of carbon steel pipes
  • Storing Thermal Heat in Materials - Energy stored as sensible heat in materials
  • Sulfuric Acid - Density - Density of sulfuric acid at various temperatures and concentrations
  • Water - Specific Heat - Online calculator, figures and tables showing specific heat of liquid water at constant volume or constant pressure at temperatures from 0 to 360 °C (32-700 °F) - SI and Imperial units

Tag Search

  • en: specific heat capacity fluids liquids
  • es: fluidos capacidad calorífica líquidos específicos
  • de: spezifische Wärmekapazität Flüssigkeiten Flüssigkeiten
  • Formula: HNaO
  • Molecular weight: 39.9971
  • IUPAC Standard InChI:
    • InChI=1S/Na.H2O/h;1H2/q+1;/p-1
    • Download the identifier in a file.
  • IUPAC Standard InChIKey:HEMHJVSKTPXQMS-UHFFFAOYSA-M
  • CAS Registry Number: 1310-73-2
  • Chemical structure:
    This structure is also available as a 2d Mol fileor as a computed3d SD file
    The 3d structure may be viewed usingJavaorJavascript.
  • Species with the same structure:
  • Information on this page:
  • Data at other public NIST sites:
  • Options:

Data at NIST subscription sites:

Specific Heat Capacity Bbc Bitesize

NIST subscription sites provide data under theNIST Standard ReferenceData Program, but require an annual fee to access.The purpose of the fee is to recover costs associatedwith the development of data collections included insuch sites. Your institution may already be a subscriber.Follow the links above to find out more about the datain these sites and their terms of usage.

Gas phase thermochemistry data

Go To:Top, Condensed phase thermochemistry data, Reaction thermochemistry data, Gas phase ion energetics data, References, Notes

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

QuantityValueUnitsMethodReferenceComment
ΔfH°gas-197.76kJ/molReviewChase, 1998Data last reviewed in December, 1970
QuantityValueUnitsMethodReferenceComment
S°gas,1 bar228.47J/mol*KReviewChase, 1998Data last reviewed in December, 1970

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.

View plotRequires a JavaScript / HTML 5 canvas capable browser.

View table.

Temperature (K)2500. - 6000.
A49.46492
B7.000125
C-1.391757
D0.095206
E-0.256928
F-213.6706
G284.8609
H-197.7572
ReferenceChase, 1998
CommentData last reviewed in December, 1970

Condensed phase thermochemistry data

Go To:Top, Gas phase thermochemistry data, Reaction thermochemistry data, Gas phase ion energetics data, References, Notes

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

QuantityValueUnitsMethodReferenceComment
ΔfH°liquid-416.88kJ/molReviewChase, 1998Data last reviewed in December, 1970
QuantityValueUnitsMethodReferenceComment
S°liquid,1 bar75.91J/mol*KReviewChase, 1998Data last reviewed in December, 1970
QuantityValueUnitsMethodReferenceComment
ΔfH°solid-425.93kJ/molReviewChase, 1998Data last reviewed in December, 1970
QuantityValueUnitsMethodReferenceComment
S°solid64.46J/mol*KReviewChase, 1998Data last reviewed in December, 1970

Liquid 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.

View plotRequires a JavaScript / HTML 5 canvas capable browser.

View table.

Temperature (K)596. - 2500.
A88.34725
B-2.495103
C-3.013028
D0.862607
E0.042216
F-442.9350
G183.9320
H-416.8783
ReferenceChase, 1998
CommentData last reviewed in December, 1970

Solid 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.

View plotRequires a JavaScript / HTML 5 canvas capable browser.

View table.

Temperature (K)298. - 572.572. - 596.
A419.483786.02304
B-1717.7540.000000
C2953.5730.000000
D-1597.2210.000000
E-6.0468840.000000
F-517.8662-448.8512
G933.0738169.6281
H-425.9312-425.9312
ReferenceChase, 1998Chase, 1998
CommentData last reviewed in December, 1970Data last reviewed in December, 1970

Reaction thermochemistry data

Go To:Top, Gas phase thermochemistry data, Condensed phase thermochemistry data, Gas phase ion energetics data, References, Notes

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

Data compiled as indicated in comments:
ALS - Hussein Y. Afeefy, Joel F. Liebman, and Stephen E. Stein
MS - José A. Martinho Simões

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

Sodium Hydroxide Specific Heat Capacity Units

2 + = + +

By formula: 2HNaO + C2H3FO = C2H3NaO2 + FNa + H2O

QuantityValueUnitsMethodReferenceComment
ΔrH°-56.15 ± 0.08kJ/molCmPritchard and Skinner, 1950liquid phase; Corrected for CODATA value of ΔfH; HF(100); ALS
ΔrH°-177.kJ/molCmCarson and Skinner, 1949liquid phase; ALS

2 + = + 2 + 2

By formula: 2HNaO + C2H6O4 = H2 + 2CHNaO2 + 2H2O

QuantityValueUnitsMethodReferenceComment
ΔrH°-293.3 ± 5.0kJ/molCmJenkins and Style, 1953solid phase; Reanalyzed by Cox and Pilcher, 1970, Original value = -292. kJ/mol; ALS

+ =

By formula: HNaO + C2H2O = C2H3NaO2

QuantityValueUnitsMethodReferenceComment
ΔrH°-208.2 ± 1.6kJ/molCmNuttall, Laufer, et al., 1971gas phase; ALS
ΔrH°-197.3kJ/molCmRice and Greenberg, 1934gas phase; ALS

C2Na2 (cr) + 2 (l) = 2( • 1418) (solution) + (g)

Hydroxide

By formula: C2Na2 (cr) + 2H2O (l) = 2(HNaO • 1418H2O) (solution) + C2H2 (g)

QuantityValueUnitsMethodReferenceComment
ΔrH°-161.8 ± 1.5kJ/molRSCJohnson, van Deventer, et al., 1973Please also see Pedley and Rylance, 1977.; MS

C2HNa (cr) + (l) = ( • 1418) (solution) + (g)

By formula: C2HNa (cr) + H2O (l) = (HNaO • 1418H2O) (solution) + C2H2 (g)

QuantityValueUnitsMethodReferenceComment
ΔrH°-54.2 ± 0.8kJ/molRSCJohnson, van Deventer, et al., 1973Please also see Pedley and Rylance, 1977.; MS

3 + = CNa2O3 + + +

By formula: 3HNaO + C3H5ClO2 = CNa2O3 + C2H6O + ClNa + H2O

QuantityValueUnitsMethodReferenceComment
ΔrH°-323.3 ± 1.7kJ/molCmDavies, Finch, et al., 1980liquid phase; Heat of hydrolysis; ALS

2 + = + + CNO.Na

By formula: 2HNaO + CBrN = BrNa + H2O + CNO.Na

QuantityValueUnitsMethodReferenceComment
ΔrH°-234.6 ± 0.71kJ/molCmLord and Woolf, 1954solid phase; Heat of hydrolysis; ALS

2 + = + + CNO.Na

By formula: 2HNaO + CIN = INa + H2O + CNO.Na

QuantityValueUnitsMethodReferenceComment
ΔrH°-193.9 ± 0.3kJ/molCmLord and Woolf, 1954solid phase; Heat of hydrolysis; ALS

2 + = + + CNO.Na

By formula: 2HNaO + CClN = ClNa + H2O + CNO.Na

QuantityValueUnitsMethodReferenceComment
ΔrH°-277.5 ± 0.4kJ/molCmLord and Woolf, 1954solid phase; Heat of Hydrolysis; ALS

+ = +

By formula: C2HBr3O + HNaO = CHNaO2 + CHBr3

QuantityValueUnitsMethodReferenceComment
ΔrH°-93.72kJ/molCmPritchard and Skinner, 1950, 2liquid phase; Heat of hydrolysis; ALS

+ = +

By formula: HNaO + C2HCl3O = CHNaO2 + CHCl3

QuantityValueUnitsMethodReferenceComment
ΔrH°-102.8kJ/molCmPritchard and Skinner, 1950, 2liquid phase; Heat of hydrolysis; ALS

+ = +

By formula: HNaO + C2H5NO = C2H3NaO2 + H3N

QuantityValueUnitsMethodReferenceComment
ΔrH°-45.6kJ/molCmCalvet, 1933solid phase; Heat of hydrolysis; ALS

C6H5NaO (cr) + (l) = (cr) + (cr)

By formula: C6H5NaO (cr) + H2O (l) = C6H6O (cr) + HNaO (cr)

QuantityValueUnitsMethodReferenceComment
ΔrH°21.4 ± 3.6kJ/molRSCLeal, Pires de Matos, et al., 1991MS

C2H5NaO (cr) + (l) = (cr) + (l)

By formula: C2H5NaO (cr) + H2O (l) = HNaO (cr) + C2H6O (l)

QuantityValueUnitsMethodReferenceComment
ΔrH°-5.7 ± 1.9kJ/molRSCLeal, Pires de Matos, et al., 1991MS

(cr) + (l) = (cr) + (l)

By formula: CH3NaO (cr) + H2O (l) = HNaO (cr) + CH4O (l)

QuantityValueUnitsMethodReferenceComment
ΔrH°-6.5 ± 2.4kJ/molRSCLeal, Pires de Matos, et al., 1991MS

Gas phase ion energetics data

Go To:Top, Gas phase thermochemistry data, Condensed phase thermochemistry data, Reaction thermochemistry data, References, Notes

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

Data evaluated by:Edward P. Hunter and Sharon G. Lias

QuantityValueUnitsMethodReferenceComment
Proton affinity (review)1071.8kJ/molN/AHunter and Lias, 1998
QuantityValueUnitsMethodReferenceComment
Gas basicity1044.8kJ/molN/AHunter and Lias, 1998

References

Sodium Hydroxide Specific Heat Capacity Of Water

Go To:Top, Gas phase thermochemistry data, Condensed phase thermochemistry data, Reaction thermochemistry data, Gas phase ion energetics data, Notes

Data compilation copyrightby 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]

Pritchard and Skinner, 1950
Pritchard, H.O.; Skinner, H.A.,The heat of hydrolysis of acetyl fluoride,J. Chem. Soc., 1950, 1099. [all data]

Carson and Skinner, 1949
Carson, A.S.; Skinner, H.A.,201. Carbon-halogen bond energies in the acetyl halides,J. Chem. Soc., 1949, 936-939. [all data]

Jenkins and Style, 1953
Jenkins, A.D.; Style, D.W.G.,The thermochemistry and pyrolysis of bishydroxymethyl,J. Chem. Soc., 1953, 2337-23. [all data]

Cox and Pilcher, 1970
Cox, J.D.; Pilcher, G.,Thermochemistry of Organic and Organometallic Compounds, Academic Press, New York, 1970, 1-636. [all data]

Nuttall, Laufer, et al., 1971
Nuttall, R.L.; Laufer, A.H.; Kilday, M.V.,The enthalpy of formation of ketene,J. Chem. Thermodyn., 1971, 3, 167-174. [all data]

Rice and Greenberg, 1934
Rice, F.O.; Greenberg, J.,Ketene. III. Heat of formation and heat of reaction with alcohols,J. Am. Chem. Soc., 1934, 38, 2268-2270. [all data]

Johnson, van Deventer, et al., 1973
Johnson, G.K.; van Deventer, E.H.; Ackerman, J.P.; Hubbard, W.N.; Osborne, D.W.; Flotow, H.L.,J. Chem. Thermodyn., 1973, 5, 57. [all data]

Pedley and Rylance, 1977
Pedley, J.B.; Rylance, J.,Computer Analysed Thermochemical Data: Organic and Organometallic Compounds, University of Sussex, Brigton, 1977. [all data]

Davies, Finch, et al., 1980
Davies, R.H.; Finch, A.; Gardner, P.J.,The standard enthalpy of formation of liquid and gaseous ethylchloroformate (C3H5O2Cl),J. Chem. Thermodyn., 1980, 12, 291-296. [all data]

Lord and Woolf, 1954
Lord, G.; Woolf, A.A.,The cyanogen halides. Part III. Their heats of formation and free energies,J. Chem. Soc., 1954, 2546-2551. [all data]

Pritchard and Skinner, 1950, 2
Pritchard, H.O.; Skinner, H.A.,The heats of hydrolysis of chloral and bromal, and the C-C bond dissociation energies in chloral and bromal,J. Am. Chem. Soc., 1950, 1928-1931. [all data]

Calvet, 1933
Calvet, E.,Mesures thermochimiques directes en chimie organique vitesses et chaleurs de saponification des amides. II.-Mesures effectuees et resultats obtenus,J. Chim. Phys., 1933, 30, 140-146. [all data]

Leal, Pires de Matos, et al., 1991
Leal, J.P.; Pires de Matos, A.; Martinho Simões, J.A.,J. Organometal. Chem., 1991, 403, 1. [all data]

Sodium Hydroxide Specific Heat Capacity Calculations

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]

Notes

Sodium Hydroxide Specific Heat Capacity Calculator

Go To:Top, Gas phase thermochemistry data, Condensed phase thermochemistry data, Reaction thermochemistry data, Gas phase ion energetics data, References

  • Symbols used in this document:
    S°gas,1 barEntropy of gas at standard conditions (1 bar)
    S°liquid,1 barEntropy of liquid at standard conditions (1 bar)
    S°solidEntropy of solid at standard conditions
    ΔfH°gasEnthalpy of formation of gas at standard conditions
    ΔfH°liquidEnthalpy of formation of liquid at standard conditions
    ΔfH°solidEnthalpy of formation of solid at standard conditions
    ΔrH°Enthalpy of reaction at standard conditions
  • Data from NIST Standard Reference Database 69:NIST Chemistry WebBook
  • The National Institute of Standards and Technology (NIST)uses its best efforts to deliver a high quality copy of theDatabase and to verify that the data contained therein havebeen selected on the basis of sound scientific judgment.However, NIST makes no warranties to that effect, and NISTshall not be liable for any damage that may result fromerrors or omissions in the Database.
  • Customer supportfor NIST Standard Reference Data products.