Predict whether each of the following ionic compounds is soluble in water:
b. Kl

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Identify the ions that make up the compound Kl. Potassium iodide (Kl) consists of potassium ions (K⁺) and iodide ions (I⁻).

Refer to the solubility rules for ionic compounds in water. According to these rules, compounds containing alkali metal cations (such as K⁺) are generally soluble in water.

Additionally, compounds containing halide ions (such as I⁻) are typically soluble, except when paired with certain cations like Ag⁺, Pb²⁺, or Hg₂²⁺. Since K⁺ is not one of these exceptions, the compound remains soluble.

Combine the information from the solubility rules to conclude that Kl is soluble in water.

To confirm, you can write the dissociation equation for Kl in water:

K I (s) \to K ⁺ (aq) + I ⁻ (aq)

. This shows that Kl dissociates completely, confirming its solubility.

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Ionic Compounds

Ionic compounds are formed when atoms transfer electrons, resulting in the formation of positively and negatively charged ions. These compounds 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.

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Naming Ionic Compounds

Solubility Rules

Solubility rules are guidelines that help predict whether an ionic compound will dissolve in water. Common rules include that most alkali metal salts and nitrates are soluble, while many carbonates and phosphates are not. Understanding these rules is essential for determining the solubility of specific compounds.

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Solubility Rules

Potassium Iodide (KI)

Potassium iodide (KI) is an ionic compound composed of potassium ions (K+) and iodide ions (I-). According to solubility rules, KI is soluble in water due to the presence of the alkali metal potassium, which typically forms soluble compounds. This property makes KI useful in various applications, including medical and nutritional contexts.

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