quickconverts.org
☰

Na2c2o4

Image related to na2c2o4

Understanding Sodium Oxalate (Na₂C₂O₄): Properties, Reactions, and Applications



Introduction:

Sodium oxalate (Na₂C₂O₄) is a white crystalline powder that is the sodium salt of oxalic acid. Its chemical formula, Na₂C₂O₄, indicates it comprises two sodium (Na) cations and one oxalate (C₂O₄²⁻) anion. This compound finds various applications, from analytical chemistry to industrial processes and even in some niche biological contexts. This article provides a comprehensive overview of sodium oxalate's properties, chemical reactions, uses, safety considerations, and frequently asked questions.

1. Chemical Structure and Properties:

Sodium oxalate possesses a relatively simple ionic structure. The oxalate anion (C₂O₄²⁻) is a planar molecule comprising two carbon atoms, each double-bonded to an oxygen atom, and singly bonded to another oxygen atom. This structure results in a resonance-stabilized dianion, giving it a relatively stable nature. The two sodium cations are electrostatically attracted to the negatively charged oxalate anion, forming the ionic compound. Key physical properties include:

Appearance: White crystalline powder.
Solubility: Highly soluble in water, moderately soluble in ethanol.
Melting Point: Decomposes before melting.
Molar Mass: Approximately 134 g/mol.


2. Chemical Reactions:

Sodium oxalate participates in various chemical reactions due to the reactivity of the oxalate anion. Some key reactions include:

Acid-Base Reactions: Sodium oxalate reacts with acids, such as sulfuric acid (H₂SO₄), to form oxalic acid and the corresponding sodium salt (e.g., sodium sulfate). This reaction is often used to prepare oxalic acid in the laboratory. The equation is: Na₂C₂O₄ + H₂SO₄ → H₂C₂O₄ + Na₂SO₄

Redox Reactions: The oxalate ion can act as a reducing agent, meaning it can donate electrons to other species. A crucial example is its reaction with potassium permanganate (KMnO₄) in acidic solution. This reaction is frequently used in titrations to determine the concentration of oxidizing agents. The balanced equation is: 5Na₂C₂O₄ + 2KMnO₄ + 8H₂SO₄ → K₂SO₄ + 2MnSO₄ + 5Na₂SO₄ + 10CO₂ + 8H₂O

Complexation Reactions: Oxalate ions can form stable complexes with various metal cations, particularly those of transition metals. These complexes often have distinct colors, which is useful in analytical chemistry. For example, it forms a complex with iron(III) ions.


3. Applications of Sodium Oxalate:

The versatility of sodium oxalate leads to its use in several fields:

Analytical Chemistry: It serves as a primary standard in redox titrations due to its high purity and stable nature. Its reaction with potassium permanganate allows for precise determination of the permanganate concentration.

Industrial Applications: It's used as a reducing agent in various industrial processes, such as in textile dyeing and printing. It also finds application in metal cleaning and as a component in photographic chemicals.

Medical and Biological Applications: Although less common, it has found niche applications in some biological research and as an anticoagulant in blood collection (though less frequently used now due to the availability of safer alternatives).

Food Industry: In some countries, it's used as a food additive (although its use is strictly regulated).


4. Safety and Handling:

While sodium oxalate is generally considered relatively safe, precautions should be taken during handling. It's important to avoid inhalation of dust and direct contact with skin and eyes. Oxalic acid, a potential product of its reaction with acids, is toxic. Therefore, appropriate personal protective equipment (PPE), such as gloves and eye protection, should be worn during handling. Proper ventilation is also crucial to prevent the inhalation of dust or any potentially harmful byproducts of reactions.


5. Environmental Considerations:

Although sodium oxalate itself is not considered a major environmental pollutant, its disposal should be done responsibly. Large quantities should be handled according to local environmental regulations, as its degradation products can impact the environment if not managed correctly.


Summary:

Sodium oxalate (Na₂C₂O₄) is a versatile chemical compound with a range of applications stemming from its unique properties and reactivity. Its importance in analytical chemistry as a primary standard and its roles in various industrial and niche applications highlight its significance. Understanding its chemical reactions, especially its redox and acid-base properties, is crucial for its safe and effective use. Always prioritize safety measures and responsible disposal practices when handling this compound.


Frequently Asked Questions (FAQs):

1. Is sodium oxalate toxic? While not acutely highly toxic, ingestion of large quantities can be harmful. Skin and eye contact should be avoided.

2. How is sodium oxalate prepared? It's typically prepared by neutralizing oxalic acid with sodium hydroxide (NaOH).

3. What are the alternatives to sodium oxalate in redox titrations? Other primary standards, such as potassium iodate or sodium thiosulfate, can be used depending on the specific titration.

4. Can sodium oxalate be used as a cleaning agent? Yes, in some industrial applications, it's used as a metal cleaning agent, but its use should follow appropriate safety protocols.

5. Is sodium oxalate flammable? No, it's not considered flammable. However, it decomposes upon heating.

Links:

Converter Tool

Conversion Result:

=

Note: Conversion is based on the latest values and formulas.

Formatted Text:

19cms to inches convert
165 centimeters in feet convert
225cm in feet convert
how tall is 200 cm in feet convert
112cm in feet convert
6 9 cm convert
248cm in feet convert
how many inches are in 140 cm convert
convert cms to inches calculator convert
change from cm to inch convert
what is 90 cms in inches convert
205cm to feet convert
115cm inch convert
89cm into inches convert
130cm convert to inches convert

Search Results:

称取基准Na2C2O4物质0.2262克以标定KMnO4 溶液的浓度,滴定达 … Na2C2O4被氧化成Na2CO3,失去2个电子,而高锰酸钾被还原成二价锰离子,得到5个电子.消耗比例为5:2.Na2C2O4为0.2262克,0.0169mol.对应高锰酸钾的物质的量为0.000675mol.消耗量为41.5毫升, …

大专 33.求0.1000mol·L-1 NaOH标准溶液对 H2C2O4的滴定 … 滴定度:是指每毫升标准滴定溶液相当于被测物质的质量（g 或mg）.也可以理解为每毫升标准滴定溶液恰好能与多少g被测物质完全反应. 2NaOH + H2C2O4==Na2C2O4+2H2O 2mol 90.04(g) …

用Na2C2O4（A）标定KMnO4（B）时,其反应系数之间的关系为（ Na2C2O4标定KMnO4时,为什么要加热到70摄氏度到80摄氏度?溶液温度过高或过低有何影 1年前 1个回答 用Na2C2O4作基准物质标定KMnO4的浓度时,应该用什么酸控制酸度,滴定温度应控制在什 …

Na2C2O4热分解反应方程式为：. - 雨露学习互助 向na2c2o4溶液中滴加过量的甲酸溶液,离子反应为,c2o4ˉ+hcooh=Hc2o4ˉ+Hcooˉ 为什么不是H2c 1年前 4个回答 置换反应、分解反应、化合反应、复分解反应的方程式

化学ki中加入fecl3再加入na2c2o4 - 雨露学习互助 2KI+2FeCl3=I2+2FeCl2+2KCl,现象：溶液由无色变为棕黄色（亚铁离子和碘的水溶液颜色） 加入草酸钠：I2+Na2C2O4=2NaI+2CO2,现象：溶液变成绿色（上一步生成亚铁离子的颜色）

请问KHC2O4.H2C2O4.2H2O和NaOH反应的化学反应方程式是什么, … 草酸三氢钾和氢氧化钠反应,视比例不同可得不同的产物. khc2o4·h2c2o4 + naoh = khc2o4 + nahc2o4 + h2o khc2o4·h2c2o4 + 2naoh = khc2o4 + na2c2o4 + 2h2o 2khc2o4 ·h2c2o4 + 6naoh = …

在滴定草酸钠时为什么高锰酸钾开始褪色慢之后比较快 - 雨露学习互助 草酸钠与KMnO4的反应是一个自催化反应. 5 Na2C2O4 + 2 KMnO4 + 8 H2SO4 = K2SO4 + 2 MnSO4 + 5 Na2SO4 + 10 CO2↑ + 8 H2O 反应生成的Mn2+会催化反应进行. 刚开始的时候,Mn2+浓度很低, …

用Na2C2O4标准溶液标定KnMO4时 应该注意控制哪些条件? - 雨露 … 用Na2C2O4作基准物质标定HCl时,是将准确称取的Na2C2O4灼烧为Na2CO3后再用HCl滴定至甲基橙终点 1年前 3个回答 用Zn2+标准溶液标定EDTA及测定水硬度时为什么要再加入氨性缓冲溶液后 …

由甲乙丙三瓶同体积同浓度的Na2C2O4,H2C2O4,NaHC2O4溶液,若 … 由甲乙丙三瓶同体积同浓度的na2c2o4,h2c2o4,nahc2o4溶液,若用naoh或hcl调节至同样的ph,最后补 as46451639 1年前 已收到1个回答 举报 赞

H2C2O4.2H2O与NaOH的反应式是? - 雨露学习互助 h2c2o4.2h2o+2naoh=na2c2o4+4h2o 如氢氧化钠过量生成草酸钠和水、 h2c2o4.2h2o+naoh=nahc2o4+3h2o 如晶体草酸过量则生成草酸氢钠和水