Decide whether each of the following is watersoluble. If...

Decide whether each of the following is watersoluble. If soluble, tell what ions are produced when the compound dissolves in water.
(a) $\mathrm{NiCl}_{2}$
(b) $\operatorname{Cr}\left(\mathrm{NO}_{3}\right)_{3}$
(c) $\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}$
(d) $\mathrm{BaSO}_{4}$

Labs

Want to see this concept in action?

NEW

Explore this concept interactively to see how it behaves as you change inputs.

View Labs

Key Concepts

Water Solubility Rules

This concept involves using a set of guidelines to predict whether an ionic compound will dissolve in water. Common rules include that nitrates, most chlorides, and alkali metal salts are generally soluble, while many sulfates and other compounds may have limited solubility due to specific exceptions. Understanding these guidelines helps predict if a substance will form a homogeneous aqueous solution or precipitate out of solution.

Ionic Dissociation in Aqueous Solutions

When ionic compounds dissolve in water, they separate into their constituent positive and negative ions—a process known as dissociation. This concept is crucial because it explains how electrolytes in solution conduct electricity and participate in chemical reactions. The extent of dissociation depends on the compound's solubility, where soluble salts fully dissociate into ions while insoluble ones remain largely intact.

Transcript

Please give Ace some feedback