Difference between revisions of "Sodium iodide"
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| BoilingPt_notes = | | BoilingPt_notes = | ||
| Density = 3.67 g/cm<sup>3</sup> | | Density = 3.67 g/cm<sup>3</sup> | ||
| − | | Formula = | + | | Formula = NaI |
| HenryConstant = | | HenryConstant = | ||
| LogP = | | LogP = | ||
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| pKb = 8-9.5 | | pKb = 8-9.5 | ||
| Solubility = 158.7 g/100 ml (0 °C)<br>184.2 g/100 ml (25 °C)<br>227.8 g/100 ml (50 °C)<br>294 g/100 ml (70 °C)<br>302 g/100 ml (100 °C) | | Solubility = 158.7 g/100 ml (0 °C)<br>184.2 g/100 ml (25 °C)<br>227.8 g/100 ml (50 °C)<br>294 g/100 ml (70 °C)<br>302 g/100 ml (100 °C) | ||
| − | | SolubleOther = Reacts with [[sulfuric acid]]<br>Soluble in [[acetone]], [[acetonitrile]], [[ethanol]], [[formamide]], [[formic acid]], [[isopropanol]], [[methanol]]<br>Slightly soluble in [[dimethylformamide]], [[sulfur dioxide]]<br>Insoluble in halocarbons, hydrocarbons | + | | SolubleOther = Reacts with [[sulfuric acid]]<br>Soluble in [[acetone]], [[acetonitrile]], [[ethanol]], [[formamide]], [[formic acid]], [[isopropanol]], [[methanol]]<br>Slightly soluble in [[dimethylformamide]], liq. [[sulfur dioxide]]<br>Insoluble in halocarbons, hydrocarbons |
| Solubility1 = 32.3 g/100 g (41.5 °C) | | Solubility1 = 32.3 g/100 g (41.5 °C) | ||
| Solvent1 = acetamide | | Solvent1 = acetamide | ||
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==Properties== | ==Properties== | ||
===Chemical=== | ===Chemical=== | ||
| − | Addition of a strong acid, like sulfuric acid will liberate iodine. | + | Addition of a strong acid, like [[sulfuric acid]] will form [[hydroiodic acid]], which decomposes to liberate elemental [[iodine]]. |
| + | |||
| + | : 2 NaI + H<sub>2</sub>SO<sub>4</sub> → Na<sub>2</sub>SO<sub>4</sub> + 2 HI | ||
| + | : 2 HI → H<sub>2</sub> + I<sub>2</sub> | ||
===Physical=== | ===Physical=== | ||
| − | Sodium iodide is a colorless solid, soluble in water. | + | Sodium iodide is a colorless odorless solid, soluble in water. |
==Availability== | ==Availability== | ||
| Line 140: | Line 143: | ||
==Preparation== | ==Preparation== | ||
| − | Can be made by neutralizing sodium hydroxide | + | Can be made by neutralizing [[hydroiodic acid]] with [[sodium hydroxide]]/[[Sodium carbonate|carbonate]]/[[Sodium bicarbonate|bicarbonate]]: |
| + | |||
| + | : NaOH + HI → NaI + H<sub>2</sub>O | ||
| + | : Na<sub>2</sub>CO<sub>3</sub> + 2 HI → 2 NaI + H<sub>2</sub>O + CO<sub>2</sub> | ||
| + | : NaHCO<sub>3</sub> + HI → NaI + H<sub>2</sub>O + CO<sub>2</sub> | ||
Another route is addition of iodine to [[sodium thiosulfate]]. | Another route is addition of iodine to [[sodium thiosulfate]]. | ||
| + | |||
| + | : Na<sub>2</sub>S<sub>2</sub>O<sub>3</sub> + 2 HI → 2 NaI + H<sub>2</sub>O + CO<sub>2</sub> | ||
==Projects== | ==Projects== | ||
| Line 154: | Line 163: | ||
===Storage=== | ===Storage=== | ||
| − | + | Sodium iodide should be kept in closed bottles, plastic or glass. | |
===Disposal=== | ===Disposal=== | ||
Revision as of 18:17, 29 May 2019
| Names | |
|---|---|
| IUPAC name
Sodium iodide
| |
| Other names
Sodium monoiodide
| |
| Properties | |
| NaI | |
| Molar mass | 149.89 g/mol |
| Appearance | White solid |
| Odor | Odorless |
| Density | 3.67 g/cm3 |
| Melting point | 661 °C (1,222 °F; 934 K) |
| Boiling point | 1,304 °C (2,379 °F; 1,577 K) |
| 158.7 g/100 ml (0 °C) 184.2 g/100 ml (25 °C) 227.8 g/100 ml (50 °C) 294 g/100 ml (70 °C) 302 g/100 ml (100 °C) | |
| Solubility | Reacts with sulfuric acid Soluble in acetone, acetonitrile, ethanol, formamide, formic acid, isopropanol, methanol Slightly soluble in dimethylformamide, liq. sulfur dioxide Insoluble in halocarbons, hydrocarbons |
| Solubility in acetamide | 32.3 g/100 g (41.5 °C) |
| Solubility in acetone | 50.4425 g/100 g (25 °C) |
| Solubility in acetonitrile | 24.9 g/100 g (25 °C) |
| Solubility in ammonia | 162 g/100 g (25 °C) |
| Solubility in dichloromethane | 0.009 g/100 g (25 °C) |
| Vapor pressure | ~0 mmHg |
| Thermochemistry | |
| Std molar
entropy (S |
91 J·mol−1·K−1 |
| Std enthalpy of
formation (ΔfH |
−288 kJ·mol−1 |
| Hazards | |
| Safety data sheet | Sigma-Aldrich |
| Flash point | Non-flammable |
| Lethal dose or concentration (LD, LC): | |
| LD50 (Median dose)
|
4.340 mg/kg (rat, oral) |
| Related compounds | |
| Related compounds
|
Potassium iodide |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Sodium iodide (NaI) is a chemical compound, a salt formed from sodium and iodine.
Contents
Properties
Chemical
Addition of a strong acid, like sulfuric acid will form hydroiodic acid, which decomposes to liberate elemental iodine.
- 2 NaI + H2SO4 → Na2SO4 + 2 HI
- 2 HI → H2 + I2
Physical
Sodium iodide is a colorless odorless solid, soluble in water.
Availability
Sodium iodide is sold by chemical suppliers.
Preparation
Can be made by neutralizing hydroiodic acid with sodium hydroxide/carbonate/bicarbonate:
- NaOH + HI → NaI + H2O
- Na2CO3 + 2 HI → 2 NaI + H2O + CO2
- NaHCO3 + HI → NaI + H2O + CO2
Another route is addition of iodine to sodium thiosulfate.
- Na2S2O3 + 2 HI → 2 NaI + H2O + CO2
Projects
- Make hydrogen iodide and hydroiodic acid
- Make elemental iodine
- Finkelstein reaction
Handling
Safety
Sodium iodide has low toxicity.
Storage
Sodium iodide should be kept in closed bottles, plastic or glass.
Disposal
Can be recycled or dumped in trash.
