Name: solubility rules for ionic salts
Uploaded: 2020-09-03T13:38:26.000Z
Duration: 2 min 55 s
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Chemistry

Matter and its Interactions

PS.Chm.6.1

Solubility of Ionic Compounds

The solubility of a solute is its maximum possible concentration at solubility equilibrium in a given amount of solvent. Solubility is affected by temperature and other physical conditions.

Substances that dissolve in water are called water-soluble. A simple water-soluble ionic compound like sodium chloride dissolves in water by breaking up into monatomic ions. Here, it is more favorable for the water molecules and ions to interact in solution than it is for the ions to remain in the ordered solid.

A more complex water-soluble ionic compound like sodium nitrate contains ions that are composed of multiple atoms covalently bound together, or polyatomic ions. When sodium nitrate dissolves, the polyatomic nitrate ions do not split into nitrogen and oxygen. Instead, the ions disperse in solution as intact units.

Substances that do not dissolve in water are water-insoluble. For example, silver chloride is a water-insoluble ionic compound. In this case, it is more favorable for the ions to remain in the ordered solid than to interact with water and disperse in the solution.

The solubility of an ionic compound in water depends on the ion pair that makes up the compound. Chemists have formu

solubility of ionic compounds

Solubility is the measure of the maximum amount of solute that can be dissolved in a given quantity of solvent at a given temperature and pressure. Solubility is usually measured in molarity (M) or moles per liter (mol/L). A compound is termed soluble if it dissolves in water.

When soluble salts dissolve in water, the ions in the solid separate and disperse uniformly throughout the solution; this process represents a physical change known as dissociation. Potassium chloride (KCl) is an example of a soluble salt. When solid KCl is added to water, the positive (hydrogen) end of the polar water molecules is attracted to the negative chloride ions, and the negative (oxygen) ends of water are attracted to the positive potassium ions. The water molecules surround individual K+ and Cl&minus; ions, reducing the strong forces that bind the ions together and letting them move off into solution as solvated ions.&nbsp;

Another example of a soluble salt is silver nitrate, AgNO3, which dissolves in water as Ag+ and NO3- ions. Nitrate, NO3-, is a polyatomic ion, and in solution, it stays intact as a single whole unit. Unlike monatomic ions (K+, Cl-, Ag+), which contain only one atom, polyatomic ions are a group of atoms that carry a charge (NO3-, SO42-, NH4+). They remain such in solution and do not split into individual atoms.&nbsp;

A compound is termed insoluble if it does not dissolve in water. However, in reality, &ldquo;insoluble&rdquo; compounds dissolve to some extent, that is, less than 0.01 M.

In the case of insoluble salts, the strong interionic forces that bind the ions in the solid are stronger than the ion-dipole forces between individual ions and water molecules. As a result, the ions stay intact and do not separate. Thus, most of the compound remains undissolved in water. Silver chloride (AgCl) is an example of an insoluble salt. The water molecules cannot overcome the strong interionic forces that bind the Ag+ and Cl- &nbsp;ions together; hence, the solid remains undissolved.

<h4>Solubility Rules</h4>

The solubility of ionic compounds in water depends on the type of ions (cation and anion) that form the compounds. For example, AgNO3 is water-soluble, but AgCl is water-insoluble. The solubility of a salt can be predicted by following a set of empirical rules (listed below), developed based on the observations on many ionic compounds.

i) Compounds containing ammonium ions (NH4+) and alkali metal cations are soluble 
ii) All nitrates and acetates are always soluble. 
iii) Chloride, bromide, and iodide compounds are soluble with the exception of those of silver, lead, and mercury(I) 
iv) All sulfate salts are soluble except their salts with silver, lead, mercury(I), barium, strontium, and calcium 
v) All carbonates, sulfites, and phosphates are insoluble except their salts with ammonium and alkali metal cations. 
vi) Sulfides and hydroxides of all salts are insoluble, with the exception of their salts with alkali metal cations, ammonium ion, and calcium, strontium, and barium ions. 
vii) All oxide-containing compounds are insoluble except their compounds with calcium, barium, and alkali metal cations.

This text is adapted from <a href="https://openstax.org/books/chemistry-2e/pages/11-2-electrolytes">OpenStax Chemistry 2e, Section 11.2: Electrolytes.</a>

Solubility is the measure of the maximum amount of solute that can be dissolved in a given quantity of solvent at a given temperature and pressure. ...

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KEY TERMS AND CONCEPTS

solubility rules for ionic salts

Solubility rules help predict whether ionic salts will dissolve in water. Solubility is the maximum amount of solute that can dissolve in a given amount of solvent at a set temperature and pressure. It is often measured in molarity, or moles per liter (mol/L). A compound is soluble if it dissolves in water.

When a soluble salt dissolves, its ions separate and spread evenly through the solution. This physical change is called dissociation. Potassium chloride, KCl, is a simple example. Water molecules are polar, so the hydrogen end is attracted to chloride ions and the oxygen end is attracted to potassium ions. The water molecules surround the ions, weaken the forces holding the solid together, and let the ions move into solution as solvated ions.

Silver nitrate, AgNO3, also dissolves in water as Ag+ and NO3- ions. Nitrate is a polyatomic ion, which means it is a charged group of atoms. In solution, it stays together as one unit. This is different from monatomic ions such as K+, Cl-, and Ag+, which each contain only one atom.

A compound is insoluble if it does not dissolve in water. In practice, insoluble compounds still dissolve a little, but less than 0.01 M. For insoluble salts, the forces between the ions in the solid are stronger than the ion-dipole forces between the ions and water molecules. As a result, the ions stay together, and most of the solid remains undissolved. Silver chloride, AgCl, is an example. Water cannot overcome the attraction between Ag+ and Cl-, so the solid stays in place.

The solubility of ionic compounds depends on the cation and anion that form the salt. These patterns can be used to predict whether a salt will dissolve. Compounds with ammonium ions, NH4+, and alkali metal cations are soluble. All nitrates and acetates are also soluble. Chlorides, bromides, and iodides are soluble except when paired with silver, lead, or mercury(I).

Other rules apply to additional groups. All sulfate salts are soluble except those of silver, lead, mercury(I), barium, strontium, and calcium. Carbonates, sulfites, and phosphates are insoluble unless they contain ammonium or an alkali metal cation. Sulfides and hydroxides are usually insoluble, with exceptions for alkali metal cations, ammonium ion, and calcium, strontium, and barium ions. Oxide-containing compounds are also insoluble except when they contain calcium, barium, or an alkali metal cation.

Solubility Rules for Ionic Salts

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Solubility rules help predict whether ionic salts will dissolve in water. Solubility is the maximum amount of solute that can dissolve in a given amount of solvent at a set temperature and pressure. It is often measured in molarity, or moles per liter (mol/L). A compound is soluble if it dissolves in water. When a soluble salt dissolves, its ions separate and spread evenly through the solution. This physical change is called dissociation. Potassium chloride, KCl, is a simple example. Water...

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key terms and concepts

Learn how to predict whether ionic salts dissolve in water using solubility rules, with examples like KCl, AgNO3, and AgCl for grades 9–12.

Solubility Rules for Ionic Salts | JoVE K12

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Solubility Rules for Ionic Salts

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