Potassium sulfate (K2SO4) is a compound that contains potassium, sulfur, and oxygen. It is commonly used as a fertilizer to supply essential nutrients to plants and improve soil quality.
| IUPAC Name | Potassium sulfate |
| Molecular Formula | K2SO4 |
| CAS Number | 7778-80-5 |
| Synonyms | Sulfuric acid, dipotassium salt; Dipotassium sulfate; Arcanite; Sulphuric acid, potassium salt (1:2); potassium sulphate; sal polychrestum; arcanum duplicatum |
| InChI | InChI=1S/2K.H2O4S/c;;1-5(2,3)4/h;;(H2,1,2,3,4)/q2*+1;/p-2 |
Potassium Sulfate Properties
Potassium Sulfate Formula
The chemical formula for potassium sulfate is K2SO4. This means that each molecule of potassium sulfate contains two potassium atoms, one sulfur atom, and four oxygen atoms. The formula for potassium sulfate is useful for determining the stoichiometry of reactions involving the compound, as well as for calculating the amount of potassium sulfate needed for a specific application.
Potassium Sulfate Molar Mass
K2SO4 has a molar mass of approximately 174.259 g/mol. This value is calculated by adding up the atomic masses of each element in the compound, which are two potassium atoms, one sulfur atom, and four oxygen atoms. The molar mass is a useful value for determining the amount of K2SO4 needed for a specific application, such as fertilizer production or laboratory experiments.
Potassium Sulfate Boiling Point
The boiling point of K2SO4 is approximately 1,690°C (3,074°F). This is the temperature at which the compound transitions from a liquid to a gaseous state. The high boiling point of K2SO4 makes it useful for applications that require high-temperature stability, such as in the production of fertilizers and industrial chemicals.
Potassium Sulfate Melting Point
The melting point of K2SO4 is approximately 1,069°C (1,956°F). This is the temperature at which the solid compound transitions into a liquid state. The relatively high melting point of K2SO4 makes it useful for high-temperature applications, such as in the production of glass, ceramics, and fertilizers.
Potassium Sulfate Density g/mL
The density of K2SO4 is approximately 2.66 g/mL at room temperature. This means that one milliliter of K2SO4 weighs 2.66 grams. The density of K2SO4 is dependent on temperature and pressure, and it can be used to calculate the mass or volume of the compound needed for a specific application.
Potassium Sulfate Molecular Weight
The molecular weight of K2SO4 is 174.259 g/mol. This value is calculated by adding up the atomic weights of all the elements in the compound. The molecular weight is useful for calculating the amount of K2SO4 needed for specific applications, such as in fertilizers or industrial chemicals.
Potassium Sulfate Structure
The structure of K2SO4 is a crystalline lattice structure, with each potassium ion surrounded by six oxygen ions in an octahedral shape. The sulfur atom is located in the center of the lattice, with each sulfur atom surrounded by four oxygen ions in a tetrahedral shape. This lattice structure gives K2SO4 its characteristic properties, such as its high melting and boiling points.
| Appearance | White crystalline solid |
| Specific Gravity | 2.66 at 20°C |
| Color | Colorless |
| Odor | Odorless |
| Molar Mass | 174.259 g/mol |
| Density | 2.66 g/cm³ at 20°C |
| Melting Point | 1,069°C (1,956°F) |
| Boiling Point | 1,690°C (3,074°F) |
| Flash Point | Not applicable |
| Water Solubility | 111 g/L at 20°C |
| Solubility | Soluble in water, insoluble in ethanol |
| Vapor Pressure | 0.0 mmHg at 25°C |
| Vapor Density | Not applicable |
| pKa | 1st: 2.17; 2nd: 7.20; 3rd: 11.8 |
| pH | 5.5-8.5 (1% solution) |
Potassium Sulfate Safety and Hazards
K2SO4 is generally considered safe for use in industrial, agricultural, and laboratory settings. However, the compound can cause irritation or damage to the skin, eyes, and respiratory system if it is ingested or inhaled in large quantities. In addition, K2SO4 may react with certain chemicals, such as strong acids, to produce hazardous fumes or fires. It is important to handle K2SO4 with care, using proper protective equipment and following safety guidelines. Storage of K2SO4 should be done in a cool, dry, and well-ventilated area, away from incompatible materials.
| Hazard Symbols | None |
| Safety Description | S24/25: Avoid contact with skin and eyes. |
| UN IDs | UN 6066 |
| HS Code | 3104.30.00 |
| Hazard Class | Non-hazardous for transportation |
| Packing Group | Not applicable |
| Toxicity | Low toxicity |
Potassium Sulfate Synthesis Methods
Several methods exist for synthesizing K2SO4.
One common method involves the reaction of potassium chloride with sulfuric acid. The reaction produces K2SO4 and hydrogen chloride as a byproduct.
Another method involves the reaction of potassium hydroxide with sulfuric acid. This reaction also produces K2SO4 and water as a byproduct.
K2SO4 can also be obtained from the mineral langbeinite, which is a naturally occurring mineral that contains K2SO4, magnesium sulfate, and sodium chloride. Typically, miners mine the mineral and process it to remove impurities and separate the K2SO4.
Another method of producing K2SO4 involves the reaction of potassium carbonate with sulfuric acid. This reaction produces K2SO4 and carbon dioxide as a byproduct.
Potassium Sulfate Uses
K2SO4 has a wide range of applications across various industries. Here are some of the most common uses of K2SO4:
- Fertilizer: A popular fertilizer due to its high potassium content. Used in the cultivation of fruits, vegetables, and other crops.
- Glass industry: Used as a flux in the production of glass. It helps to lower the melting point of the glass and improve its durability.
- Pharmaceutical industry: Used as a component in various medications, including laxatives and electrolyte replacement solutions.
- Food industry: Used as a food additive to regulate acidity and as a leavening agent in baked goods.
- Industrial applications: Used in several industrial applications, including the production of alum, potassium carbonate, and other chemicals.
- Animal feed: Used as a feed supplement for livestock and poultry to promote healthy growth and development.
- Water treatment: Used in water treatment to control scale and corrosion in boilers and other equipment.
Questions:
Q: Is potassium sulfate soluble?
A: Yes, K2SO4 is soluble in water. It has a solubility of approximately 111 g/L at room temperature.
Q: Which will be the solid product when strontium bromide and potassium sulfate react?
A: When strontium bromide and K2SO4 react, the solid product formed is strontium sulfate (SrSO4) which is an insoluble white solid.
Q: What else is produced during the replacement reaction of silver nitrate and potassium sulfate?
A: In the replacement reaction of silver nitrate and K2SO4, silver sulfate (Ag2SO4) and potassium nitrate (KNO3) are produced as well.
Q: Is potassium sulfate an acid or base?
A: K2SO4 is neither an acid nor a base, it is a salt. It is formed from the neutralization reaction between an acid (sulfuric acid) and a base (potassium hydroxide).
Q: Is k2so4 soluble in water?
A: Yes, K2SO4 is soluble in water. It is highly soluble, and its solubility increases with temperature.
Q: Which salt is produced when h2so4 reacts with naoh? k2so3 na2so4 na2so3 k2so4 A: When H2SO4 reacts with NaOH, the salt produced is Na2SO4 (sodium sulfate) along with water.
Q: How many moles of k2so4 are in 15.0 g of k2so4?
A: To determine the number of moles of K2SO4 in 15.0 g of K2SO4, we need to divide the given mass by the molar mass of K2SO4 which is 174.259 g/mol. Thus, the number of moles of K2SO4 in 15.0 g is 0.086 mol.
Q: What would be the formula of the precipitate that forms when pb(no3)2 (aq) and k2so4 (aq) are mixed?
A: When Pb(NO3)2 (aq) and K2SO4 (aq) are mixed, the precipitate formed is PbSO4 (lead sulfate), which is an insoluble white solid. The balanced equation for this reaction is Pb(NO3)2 + K2SO4 → PbSO4 + 2KNO3.