Potassium Oxalate

The solubility of potassium oxalate in water is approximately 22.4 g/100 mL at room temperature (25°C). This means that 100 mL of water can dissolve up to 22.4 grams of potassium oxalate before reaching saturation. It should be noted that the solubility may vary slightly with temperature and pressure changes.

The molar mass of potassium oxalate monohydrate is 184.24 g/mol.

The molecular formula of potassium oxalate is K2C2O4. This compound consists of two potassium ions (K+) and one oxalate ion (C2O42-), which contains two carbon atoms (C) and four oxygen atoms (O).

The molar mass of potassium oxalate is 166.22 g/mol. This can be calculated by adding the atomic masses of the constituent elements, which are 39.10 g/mol for potassium, 12.01 g/mol for carbon, and 2 x 16.00 g/mol for oxygen (since there are two oxygen atoms in the oxalate ion). Thus, the total molar mass is:

M(K2C2O4) = 2 x M(K) + M(C) + 2 x M(O)

= 2 x 39.10 g/mol + 12.01 g/mol + 2 x 16.00 g/mol

= 78.20 g/mol + 12.01 g/mol + 32.00 g/mol

= 122.21 g/mol + 32.00 g/mol

= 154.21 g/mol

However, since there are two potassium oxalate units in the formula K2C2O4, we need to multiply this value by 2 to get the molar mass of one unit:

M(K2C2O4) x 2 = 154.21 g/mol x 2 = 308.42 g/mol

Therefore, the molar mass of potassium oxalate is 308.42 g/mol.

Potassium oxalate is a white crystalline solid with a formula of K2C2O4. Its physical properties include:

1. Melting point: The melting point of potassium oxalate is 365 °C.

2. Solubility: Potassium oxalate is soluble in water, ethanol, and methanol but insoluble in most organic solvents.

3. Density: The density of potassium oxalate is 2.13 g/cm³.

4. pH: Potassium oxalate solutions are slightly acidic with a pH of around 6.

5. Crystal structure: Potassium oxalate crystallizes in the monoclinic crystal system.

6. Thermal stability: Potassium oxalate decomposes upon heating to produce potassium carbonate and carbon dioxide.

7. Hygroscopicity: Potassium oxalate is hygroscopic, which means it can absorb moisture from the air.

8. Optical properties: Potassium oxalate is transparent to light and has a refractive index of around 1.5.

Overall, potassium oxalate is a stable and relatively inert compound with a range of physical properties that make it useful in various applications, such as in the production of photographic films and as a reducing agent in some chemical reactions.

When potassium oxalate reacts with hydrochloric acid, a double displacement reaction occurs. The potassium cation (K+) from the potassium oxalate combines with the chloride anion (Cl-) from the hydrochloric acid to form potassium chloride (KCl), which is soluble in water. Meanwhile, the oxalate anion (C2O4 2-) combines with two hydrogen ions (H+) from the hydrochloric acid to form oxalic acid (H2C2O4), which is a weak organic acid and also soluble in water. Overall, the balanced chemical equation for the reaction is:

K2C2O4 + 2HCl → 2KCl + H2C2O4

The reaction is exothermic and releases heat. Additionally, the oxalic acid formed can further react with more hydrochloric acid to produce carbon dioxide gas (CO2) and water (H2O). This reaction is given by the following equation:

H2C2O4 + 2HCl → CO2 + 2H2O + 2Cl-

Overall, the reaction between potassium oxalate and hydrochloric acid results in the formation of potassium chloride and oxalic acid, with the possibility of further reacting to produce carbon dioxide gas and water.

Potassium oxalate has several common uses, including:

1. Metal cleaning: Potassium oxalate is used as a metal cleaner to remove rust and tarnish from metals like brass, copper, and bronze.

2. Photography: It is used in photography as a reducing agent for developing photographic films and papers.

3. Bleaching agent: Potassium oxalate is also used as a bleaching agent for certain dyes and fabrics.

4. Medical applications: It has been used in some medical applications such as the treatment of hyperoxaluria, a condition where the body produces too much oxalate that can lead to kidney stones.

5. Laboratory reagent: It is used as a laboratory reagent for analytical chemistry, primarily for gravimetric analysis and titration.

It should be noted that while potassium oxalate has various uses, it can be toxic if ingested or inhaled in large quantities, so caution must be exercised when handling it.

Potassium oxalate is a toxic and potentially hazardous compound. It can cause severe irritation to the skin, eyes, and respiratory system upon contact or inhalation. Ingestion of potassium oxalate can also lead to gastrointestinal distress, kidney damage, and even death in extreme cases.

Additionally, potassium oxalate is highly reactive with many other chemicals and can pose a fire or explosion hazard if not handled properly. It is also harmful to aquatic life and should be disposed of carefully to prevent environmental contamination.

Therefore, it is important to handle potassium oxalate with caution, wear appropriate personal protective equipment (PPE), and follow proper chemical handling and disposal procedures to minimize the risks associated with this compound.

The production process of potassium oxalate typically involves the reaction of potassium hydroxide (KOH) with oxalic acid (H2C2O4), which results in the formation of potassium oxalate (K2C2O4) and water (H2O). The reaction is typically carried out under controlled conditions, such as at a specific temperature and pressure, to ensure proper formation and purity of the product.

Specifically, the process involves dissolving a known amount of KOH in water, followed by slow addition of oxalic acid to the solution with constant stirring. This causes the formation of solid potassium oxalate, which is typically separated from the reaction mixture through filtration or centrifugation.

The separated potassium oxalate may be washed with water to remove any impurities and dried to obtain the final product. The purity of the product can be assessed using techniques such as thin-layer chromatography or spectroscopy.

Overall, the production process of potassium oxalate requires careful control of reaction conditions and purification steps to ensure the desired product is obtained with high purity and yield.

The structure of potassium oxalate is a salt consisting of potassium ions (K+) and oxalate ions (C2O42-). The oxalate ion has a planar structure with two carbonyl groups (C=O) and two carboxyl groups (COO-) on adjacent carbon atoms. The potassium ions are then coordinated to the oxalate ions through ionic bonds. The overall structure of potassium oxalate is a crystalline solid with a highly ordered arrangement of ions in a lattice structure.

Potassium oxalate is a salt that can behave differently under various environmental conditions. In acidic conditions, it can react with acids to form oxalic acid and potassium salts of the acid used. In basic conditions, it can react with strong bases to form insoluble precipitates of calcium oxalate or other oxalate salts. Potassium oxalate can also decompose when exposed to high temperatures or intense light, producing carbon dioxide, carbon monoxide, and potassium carbonate. Additionally, it can react with metals to produce hydrogen gas and metal oxalates. Overall, the behavior of potassium oxalate depends on the specific environmental conditions it is exposed to.