Solubility Rule Guidelines Ionic Soluble Insoluble Salt

Overview

Engineering reference data for Solubility Rule Guidelines Ionic Soluble Insoluble Salt in chemistry.

Key Formulas

Ideal Gas Law

$PV = nRT$

Pressure × Volume = moles × gas constant × temperature.

Molarity

$M = \frac{n}{V}$

Moles of solute per liter of solution.

pH

$pH = -\log_{10}[H^+]$

Measure of acidity.

Variables

Symbol	Description	Unit
$P$	Pressure	Pa
$V$	Volume	m³
$n$	Moles	mol
$R$	Gas constant	8.314 J/(mol·K)

Solubility Rules Summary

The following tables summarize the general solubility rules for ionic compounds in water at room temperature.

Practical Application: Predicting Precipitation

These rules are fundamental in predicting the outcome of double displacement (metathesis) reactions in aqueous solution. To predict if a precipitate forms:

1. Identify all ions present in the two reactant solutions.
2. Consider all possible new cation-anion pairs (the potential products).
3. Apply the solubility rules to each potential product.
4. If any potential product is insoluble (or only slightly soluble) according to the rules, a precipitation reaction will occur, and the insoluble salt will form as the precipitate.

Example: Mixing silver nitrate (AgNO₃) and sodium chloride (NaCl) solutions produces Ag⁺, NO₃⁻, Na⁺, and Cl⁻ ions. The potential products are AgCl and NaNO₃. According to the rules, NaNO₃ is soluble (Group 1 cation), but AgCl is insoluble. Therefore, a white precipitate of AgCl will form: $\text{Ag}^+(\text{aq}) + \text{Cl}^-(\text{aq}) \rightarrow \text{AgCl}(\text{s})$

References

• Original Source