Solubility Rule Guidelines Ionic Soluble Insoluble Salt

Reference data and engineering information about solubility rule guidelines ionic soluble insoluble salt for chemistry applications.

Solubilityruleguidelinesionic

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.

15 rows

Table 1: Ions and Compounds that are Usually Soluble in Water
Ion / Compound	Typical Formula	Solubility / Exceptions
Acetates	CH₃COO⁻	Usually soluble
		Exception: AgCH₃COO is moderately soluble
Ammonium	NH₄⁺	Usually soluble
Chlorates	ClO₃⁻	Usually soluble
Perchlorates	ClO₄⁻	Usually soluble
Group 1 Cations	Li⁺, Na⁺, K⁺, Rb⁺, Cs⁺	Usually soluble
Halides	F⁻	Usually soluble
		Exceptions: MgF₂, CaF₂, SrF₂, BaF₂, PbF₂ are insoluble
	Cl⁻, Br⁻, I⁻	Usually soluble
		Exceptions: AgCl, Hg₂Cl₂, PbCl₂, AgBr, Hg₂Br₂, PbBr₂, AgI, Hg₂I₂, PbI₂ are insoluble
Nitrates	NO₃⁻	Usually soluble
Nitrites	NO₂⁻	Usually soluble
		Exception: AgNO₂ is moderately soluble
Sulfates	SO₄²⁻	Usually soluble
		Exceptions: CaSO₄, SrSO₄, Ag₂SO₄ are moderately soluble; BaSO₄, PbSO₄ are insoluble

Source: Derived from extracted chemistry reference data

8 rows

Table 2: Ions and Compounds that are Usually Insoluble in Water
Ion / Compound	Typical Formula	Solubility / Exceptions
Carbonates	CO₃²⁻	Usually insoluble
		Exceptions: (NH₄)₂CO₃, Na₂CO₃, K₂CO₃ are soluble
Hydroxides	OH⁻	Usually insoluble
		Exceptions: LiOH, NaOH, KOH, Ba(OH)₂ are soluble; Ca(OH)₂, Sr(OH)₂ are moderately soluble
Phosphates	PO₄³⁻	Usually insoluble
		Exceptions: (NH₄)₃PO₄, Na₃PO₄, K₃PO₄ are soluble
Sulfides	S²⁻	Usually insoluble
		Exceptions: (NH₄)₂S, Na₂S, K₂S, MgS, CaS are soluble

Source: Derived from extracted chemistry reference data

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:

Identify all ions present in the two reactant solutions.
Consider all possible new cation-anion pairs (the potential products).
Apply the solubility rules to each potential product.
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

Source: engineeringtoolbox.com