Sodium chloride (NaCl) is a compound composed of sodium and chlorine ions. It is commonly known as table salt and is used for seasoning food and preserving food products.
| IUPAC Name | Sodium chloride |
| Molecular Formula | NaCl |
| CAS Number | 7647-14-5 |
| Synonyms | Halite, Rock salt, Saline, Sea salt |
| InChI | InChI=1S/ClH.Na/h1H;/q;+1/p-1 |
Sodium chloride formula
The chemical formula for sodium chloride is NaCl, representing the combination of one sodium ion (Na+) and one chloride ion (Cl-). The formula indicates the relative number of atoms or ions in the compound, allowing for easy identification and representation of its composition.
NaCl molar mass
The molar mass of sodium chloride, also known as table salt, is 58.44 g/mol. This means that one mole of sodium chloride contains 58.44 grams of the compound. The molar mass is calculated by adding the atomic masses of sodium (Na) and chlorine (Cl) in the compound, which are 22.99 g/mol and 35.45 g/mol, respectively.
Sodium chloride boiling point
Sodium chloride has a high boiling point of 1413°C (2575°F) due to its ionic bonding. When heated, the energy input breaks the ionic bonds between the sodium and chloride ions, causing the compound to undergo a phase change from a solid to a liquid state. The boiling point of sodium chloride is higher than that of many other compounds due to the strong electrostatic attraction between the ions.
Sodium chloride melting point
The melting point of sodium chloride is 801°C (1474°F). Like the boiling point, the high melting point is due to the strong ionic bonds between the sodium and chloride ions. When heated, the energy input overcomes the electrostatic forces holding the ions together, causing the compound to transition from a solid to a liquid state.
Sodium chloride density g/ml
The density of sodium chloride is 2.165 g/mL at room temperature (25°C or 77°F). The density is a measure of the mass per unit volume of a substance. The high density of sodium chloride is due to the compact arrangement of its atoms and the strong ionic bonding between the sodium and chloride ions.
Sodium chloride molecular weight
The molecular weight of sodium chloride is 58.44 g/mol, as previously mentioned. The molecular weight is calculated by adding the atomic weights of all atoms in a molecule. Although sodium chloride does not exist as a molecule in the traditional sense, its molecular weight is calculated based on the formula unit of NaCl.
Sodium chloride Structure
Sodium chloride has a crystalline structure, consisting of a regular arrangement of sodium and chloride ions in a 1:1 ratio. The structure is a face-centered cubic lattice, with each sodium ion surrounded by six chloride ions and each chloride ion surrounded by six sodium ions. The ionic bonding in sodium chloride results in a lattice structure that is very stable and difficult to break apart.
| Appearance | White crystalline solid |
| Specific Gravity | 2.165 |
| Color | Colorless |
| Odor | Odorless |
| Molar Mass | 58.44 g/mol |
| Density | 2.165 g/mL |
| Melting Point | 801°C (1474°F) |
| Boiling Point | 1413°C (2575°F) |
| Flash Point | Not applicable |
| Water Solubility | 359 g/L at 20°C |
| Solubility | Soluble in water and glycerol; insoluble in ethanol and acetone |
| Vapour Pressure | Negligible |
| Vapour Density | Not applicable |
| pKa | 7 |
| pH | 7 (neutral) |
Sodium Chloride Safety and Hazards
Sodium chloride (NaCl) is generally considered safe for human consumption and use. However, exposure to high concentrations of NaCl can lead to irritation of the eyes, skin, and respiratory tract. Ingesting large amounts of NaCl can result in dehydration, electrolyte imbalances, and even death. Sodium chloride can also be a fire and explosion hazard when in contact with combustible materials. Proper handling and storage are necessary to prevent accidents. It is important to follow proper safety guidelines and precautions when handling and using NaCl to minimize the risks of harm.
| Hazard Symbols | None |
| Safety Description | Harmful if ingested or inhaled. Causes irritation to skin and eyes. |
| UN IDs | UN 7646 |
| HS Code | 2501.00.90 |
| Hazard Class | Non-toxic |
| Packing Group | Not applicable |
| Toxicity | LD50 (oral, rat) – 3,000 mg/kg |
Sodium Chloride Synthesis Methods
Various sources can provide sodium chloride, including salt mines and seawater, but it is also possible to synthesize it in the laboratory through chemical reactions.
One common method of synthesizing sodium chloride is through the reaction of hydrochloric acid (HCl) and sodium hydroxide (NaOH). This reaction produces sodium chloride and water as byproducts. The equation for this reaction is:
HCl + NaOH → NaCl + H2O
Another method involves reacting sodium carbonate (Na2CO3) with hydrochloric acid (HCl) to produce sodium chloride, carbon dioxide, and water. The equation for this reaction is:
2HCl + Na2CO3 → 2NaCl + CO2 + H2O
The reaction between sodium and chlorine gases is one such method for synthesizing sodium chloride. This reaction requires high temperatures and careful control to prevent the formation of unwanted byproducts. The equation for this reaction is:
2Na + Cl2 → 2NaCl
Chemists can choose to modify or vary the methods of synthesizing sodium chloride based on factors such as cost, reagent availability, and the desired purity and yield of the final product. These methods ensure the production of sodium chloride even if natural sources are scarce.
Sodium Chloride Uses
Sodium chloride, also known as table salt, has numerous uses in various industries and applications. Some of the common uses of sodium chloride are:
- Food industry: Used as a seasoning and flavor enhancer in various food products, including snacks, processed meats, and baked goods.
- Medical industry: Used in intravenous solutions and other medical treatments to replenish fluids and electrolytes in the body.
- Chemical industry: Used in the production of various chemicals, including chlorine, sodium hydroxide, and sodium carbonate.
- Water treatment: Used in the treatment of water to remove impurities and make it safe for consumption.
- Agriculture: Used as a fertilizer for crops, particularly in areas where the soil is deficient in essential nutrients.
- De-icing: Used as a de-icing agent on roads and sidewalks during winter to prevent accidents due to slippery surfaces.
- Textile industry: Used in the production of synthetic fibers, such as nylon and polyester.
- Oil and gas industry: Used in the drilling and extraction of oil and gas.
- Animal husbandry: Used as a dietary supplement for livestock to promote healthy growth and development.
These are just a few examples of the many uses of sodium chloride. Its versatility and availability make it an essential ingredient in many products and processes across a wide range of industries.
Questions:
Q: Is sodium chloride a compound?
A: Yes, sodium chloride is a compound.
Q: Is sodium chloride ionic or covalent?
A: Sodium chloride is an ionic compound.
Q: What is sodium chloride?
A: Sodium chloride is a white crystalline compound with the chemical formula NaCl. It is commonly known as table salt and is essential for human and animal nutrition.
Q: What is sodium chloride used for?
A: Sodium chloride has numerous uses in various industries and applications, including as a seasoning and flavor enhancer in food, as a medical treatment, in the production of chemicals, in water treatment, as a de-icing agent, in the textile and oil and gas industries, and as a dietary supplement for livestock.
Q: Is sodium chloride soluble in water?
A: Yes, sodium chloride is highly soluble in water.