Enter a Cation (Positive Ion) and Anion (Negative Ion) to find out whether the resulting compound is soluble, insoluble, or slightly soluble — the calculator returns the Compound Formula, the Solubility Rule Applied, and any Exceptions, with optional Temperature adjustment factored in.
Solubility
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Compound Formula
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Rule Applied
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Exceptions
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Solubility is the ability of a substance to dissolve in a solvent, typically water. It's measured as the maximum amount of solute that can dissolve in a given amount of solvent at a specific temperature and pressure.
Focus on the general patterns: all nitrates and acetates are soluble, most chlorides are soluble except silver and lead, and most carbonates and phosphates are insoluble except Group 1 metals and ammonium. Practice with common examples to reinforce the patterns.
No, barium sulfate (BaSO4) is insoluble in water. While most sulfates are soluble, barium sulfate is one of the notable exceptions along with calcium, strontium, mercury, lead, and silver sulfates.
When silver nitrate (AgNO3) is mixed with sodium chloride (NaCl), a precipitation reaction occurs forming insoluble silver chloride (AgCl) and soluble sodium nitrate (NaNO3). The reaction is: AgNO3 + NaCl → AgCl↓ + NaNO3.
All nitrates (NO3⁻), acetates (CH3COO⁻), and compounds containing Group 1 metals (Li⁺, Na⁺, K⁺) or ammonium (NH4⁺) are always soluble in water with no exceptions.
Most ionic solids become more soluble as temperature increases, though the solubility rules remain the same. Temperature primarily affects the degree of solubility rather than whether a compound is classified as soluble or insoluble.
While most chlorides are soluble, the main exceptions are silver chloride (AgCl), lead chloride (PbCl2), and mercury(I) chloride (Hg2Cl2), which are all insoluble in water.
Solubility rules help predict precipitation reactions, determine which compounds will dissolve in solution, and are essential for understanding acid-base reactions, qualitative analysis, and industrial chemical processes.