Predict whether each of the following ionic compounds is soluble in water: c. BaCO₃

Verified step by step guidance

1. Identify the ions involved in the compound BaCO_3. The compound consists of Ba^{2+} (barium ion) and CO_3^{2-} (carbonate ion).
2. Consult the solubility rules for ionic compounds in water.
3. According to the solubility rules, most carbonate (CO_3^{2-}) salts are insoluble in water, except those of alkali metals (such as Na^+, K^+) and ammonium (NH_4^+).
4. Since Ba^{2+} is not an alkali metal ion or ammonium ion, BaCO_3 is expected to be insoluble in water.
5. Conclude that BaCO_3 is not soluble in water based on the solubility rules.

Key Concepts

Ionic Compounds

Ionic compounds are formed from the electrostatic attraction between positively charged cations and negatively charged anions. They typically consist of a metal and a non-metal, and their properties include high melting and boiling points, as well as electrical conductivity when dissolved in water. Understanding the structure of ionic compounds is essential for predicting their solubility.

Solubility Rules

Solubility rules are guidelines that help predict whether an ionic compound will dissolve in water. These rules indicate that certain ions, such as alkali metals and nitrates, are generally soluble, while others, like carbonates and phosphates, are often insoluble. Familiarity with these rules is crucial for determining the solubility of specific compounds like BaCO₃.

Barium Carbonate (BaCO₃)

Barium carbonate (BaCO₃) is an ionic compound composed of barium cations and carbonate anions. According to solubility rules, most carbonates are insoluble in water, with exceptions for those containing alkali metals or ammonium. Therefore, BaCO₃ is generally considered insoluble, which is important for predicting its behavior in aqueous solutions.