Sodium iodate

Sodium iodate
Names

Other names Iodic acid, sodium salt
Identifiers
CAS Number	7681-55-2^N
3D model (Jmol)	Interactive image
ChemSpider	22760^Y
ECHA InfoCard	100.028.793
EC Number	231-672-5
PubChem	23675764
RTECS number	NN1400000
InChI InChI=1S/HIO3.Na/c2-1(3)4;/h(H,2,3,4);/q;+1/p-1^Y Key: WTCBONOLBHEDIL-UHFFFAOYSA-M^Y InChI=1/HIO3.Na/c2-1(3)4;/h(H,2,3,4);/q;+1/p-1 Key: WTCBONOLBHEDIL-REWHXWOFAB
SMILES [Na+].[O-]I(=O)=O
Properties
Chemical formula	INaO₃
Molar mass	197.89 g·mol⁻¹
Appearance	White orthorhombic crystals
Odor	Odorless
Density	4.28 g/cm³
Melting point	425 °C (797 °F; 698 K) (anhydrous) decomposes^[1] 19.85 °C (67.73 °F; 293.00 K) (pentahydrate)
Solubility in water	2.5 g/100 mL (0 °C) 8.98 g/100 mL (20 °C) 9.47 g/100 mL (25 °C)^[2] 32.59 g/100 mL (100 °C)^[3]
Solubility	Soluble in acetic acid Insoluble in alcohol
Solubility in dimethylformamide	0.5 g/kg^[2]
Structure
Crystal structure	Orthorhombic
Thermochemistry
Specific heat capacity (C)	125.5 J/mol·K^[2]
Std molar entropy (S^o₂₉₈)	135 J/mol·K^[2]
Std enthalpy of formation (Δ_fH^o₂₉₈)	−490.4 kJ/mol^[2]
Gibbs free energy (Δ_fG˚)	35.1 kJ/mol^[2]
Hazards
GHS pictograms	^[4]
GHS signal word	Danger
GHS hazard statements	H272, H302, H317, H334^[4]
GHS precautionary statements	P220, P261, P280, P342+311^[4]
EU classification (DSD)	O Xn
R-phrases	R8, R22, R42/43
S-phrases	S17, S22, S36/37, S45
NFPA 704	0 1 1 OX
Lethal dose or concentration (LD, LC):
LD₅₀ (median dose)	108 mg/kg (mice, intravenous)^[2]
Related compounds
Other anions	Sodium iodide Sodium periodate Sodium bromate Sodium chlorate
Other cations	Potassium iodate Silver iodate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
N verify (what is ^YN ?)
Infobox references

Sodium iodate (Na I O₃) is the sodium salt of iodic acid. Sodium iodate is an oxidizing agent, and as such it can cause fires upon contact with combustible materials or reducing agents.

Preparation

It can be prepared by reacting a sodium-containing base such as sodium hydroxide with iodic acid, for example:

HIO₃ + NaOH → NaIO₃ + H₂O

It can also be prepared by adding iodine to a hot, concentrated solution of sodium hydroxide or its carbonate:

3 I₂ + 6 NaOH → NaIO₃ + 5 NaI + 3 H₂O

Reactions

Sodium iodate can be oxidized to sodium periodate in water solutions by hypochlorites or other strong oxidizing agents:

NaIO 3 + NaOCl \to NaIO 4 + NaCl

Safety

Conditions/substances to avoid are: heat, shock, friction, combustible materials, reducing materials, aluminium, organic compounds, carbon, hydrogen peroxide, sulfides.

References

↑ Lide, David R. (1998). Handbook of Chemistry and Physics (87 ed.). Boca Raton, FL: CRC Press. pp. 4–85. ISBN 0-8493-0594-2.
1 2 3 4 5 6 7 http://chemister.ru/Database/properties-en.php?dbid=1&id=759
↑ Seidell, Atherton; Linke, William F. (1919). Solubilities of Inorganic and Organic Compounds (2nd ed.). D. Van Nostrand Company.
Results here are multiplied by water's density at temperature of solution for unit conversion.
1 2 3 Sigma-Aldrich Co., Sodium iodate. Retrieved on 2014-05-25.

Sodium compounds

NaAlO₂ NaBH₄ NaBH₃(CN) NaBO₂ NaBiO₃ NaBr NaBrO NaBrO₃ NaCH₃COO NaC₆H₅CO₂ NaC₆H₄(OH)CO₂ NaCN NaCl NaClO NaClO₂ NaClO₃ NaClO₄ NaF Na₂FeO₄ NaH NaHCO₃ NaH₂PO₄ NaHSO₃ NaHSO₄ NaI NaIO₃ NaIO₄ Na₅IO₆ NaMnO₄ NaN₃ NaNH₂ NaNO₂ NaNO₃ NaOCN NaO₂ NaO₃ NaOH NaPO₂H₂ NaReO₄ NaSCN NaSH NaTcO₄ NaVO₃ Na₂CO₃ Na₂C₂O₄ Na₂CrO₄ Na₂Cr₂O₇ Na₂GeO₃ Na₂MnO₄ Na₃MnO₄ Na₂MoO₄ Na₂MoS₄ Na₂N₂O₂ Na₂O Na₂O₂ Na₂O(UO₃)₂ Na₂PO₃F Na₂S Na₂SO₃ Na₂SO₄ Na₂S₂O₃ Na₂S₂O₄ Na₂S₂O₅ Na₂S₂O₆ Na₂S₂O₇ Na₂S₂O₈ Na₂S₄O₆ Na₂Se Na₂SeO₃ Na₂SeO₄ Na₂SiO₃ Na₂Si₂O₅ Na₄SiO₄ Na₂Te Na₂TeO₃ Na₂TeO₄ Na₂Po Na₂Ti₃O₇ Na₂U₂O₇ NaWO₄ Na₂Zn(OH)₄ Na₃N Na₃P Na₃PO₄ Na₃VO₄ Na₄Fe(CN)₆ Na₄P₃O₇ Na₅P₃O₁₀

Chemical formulas

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