Barium acetate is an inorganic salt that exhibits high solubility in water. When introduced into an aqueous solution, it readily dissolves, forming a clear solution. This characteristic places it among highly soluble salts, meaning a significant amount can be dispersed throughout a volume of water. Its easy dissolution makes it useful in various chemical and industrial applications.
Chemical Identity and Characteristics
Barium acetate is formally known as the barium(II) salt of acetic acid. The chemical formula is Ba(C2H3O2)2, indicating one barium atom bonded to two acetate groups. It exists as a white, crystalline solid or powder, sometimes found in a hydrated form where water molecules are incorporated into its crystal structure.
The compound is categorized as an ionic salt, held together by strong electrostatic forces between positively and negatively charged ions. Its molecular weight is approximately 255.42 grams per mole. At 20 degrees Celsius, its solubility is high, allowing approximately 59 to 72 grams of the solid to dissolve in 100 milliliters of water.
The Mechanism of Dissolution in Water
The dissolution of barium acetate is governed by ionic dissociation in a polar solvent. Water molecules are polar, possessing slight negative and positive charges. This polarity allows water to effectively separate the ions in the solid crystal structure.
When barium acetate is placed in water, polar water molecules surround the solid, pulling the constituent ions away from the crystal lattice. The ionic compound then dissociates completely into its component parts: one barium cation (Ba\(^{2+}\)) and two acetate anions (C2H3O2\(^-\)).
The newly separated ions are stabilized by the water molecules through a process called hydration. The negatively charged acetate ions are surrounded by the positive ends of the water molecules, while the positively charged barium ion is surrounded by the negative ends. This interaction overcomes the strong attractive forces holding the ions together in the solid form, resulting in a stable solution.
General solubility rules confirm this behavior, as virtually all salts containing the acetate ion are soluble in water. The combination of the acetate ion with the large, low-charge-density barium cation results in a salt that dissolves freely. This complete dissociation into ions is the reason why barium acetate is highly soluble.
Common Uses Related to Solubility
High solubility dictates many practical applications of barium acetate. Because it dissolves easily, it is frequently used as a precursor chemical in the synthesis of other barium compounds. For instance, a dissolved solution of barium acetate can be reacted to produce materials like barium titanate, which is important in electronics and ceramics.
The dissolved form is utilized extensively in analytical chemistry applications. One specific use involves the quantitative determination of sulfate ions in a sample. When a solution of barium acetate is added to a sample containing sulfate ions, the insoluble compound barium sulfate precipitates out of the solution. This precipitation reaction allows chemists to accurately measure the amount of sulfate present.
Its solubility is exploited in the textile industry, where barium acetate functions as a mordant. A mordant is a substance that dissolves and helps fix dyes onto fabrics, ensuring the color remains durable. The dissolved barium ions react with both the dye and the fiber to form an insoluble complex permanently bonded to the material.