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Solubility Product Ksp ↔ Solubility

· Last updated：2026-09-03

Ksp ↔ molar solubility in either direction for 1:1, 1:2, 1:3 and 2:3 salts, with optional g/L output.

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Tool usage guide

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Key facts

Category
Science & Education
Input types
select, number
Output type
text
Sample coverage
4
API ready
Yes

Overview

The Solubility Product Ksp ↔ Solubility tool converts between solubility product constants (Ksp) and molar solubility across common ionic salt stoichiometries, including 1:1, 1:2, 1:3, and 2:3 compounds. It supports bidirectional calculation, customizable solubility units (M, mM, and µM), and optional molar mass input to compute mass solubility in g/L.

When to use

  • Determining molar solubility and saturated ion concentrations from an experimental or tabulated Ksp value.
  • Calculating the solubility product constant Ksp from known molar solubility measurements in M, mM, or µM.
  • Converting molar solubility into mass concentration (g/L) using a compound's molar mass.

How it works

  1. 1Select the calculation direction: Ksp → molar solubility (s) or molar solubility (s) → Ksp.
  2. 2Choose the salt stoichiometry: AB (1:1), AB₂/A₂B (1:2), AB₃/A₃B (1:3), or A₂B₃/A₃B₂ (2:3).
  3. 3Enter the known Ksp or molar solubility value with its corresponding concentration unit.
  4. 4Optionally enter the molar mass (g/mol) to calculate equilibrium mass solubility in g/L.

Use cases

  • Chemistry students verifying homework problems involving equilibrium expressions and saturated solution concentrations.
  • Laboratory researchers checking precipitation thresholds and dissolution limits of sparingly soluble salts.
  • Environmental scientists calculating aqueous metal ion saturation levels from standard solubility constants.

Examples

1. Calculating AgCl Molar and Mass Solubility from Ksp

Chemistry Student

Background

Working on analytical chemistry coursework calculating saturated silver ion concentrations in pure water.

Problem

Determine the molar solubility and mass solubility in g/L for Silver Chloride (AgCl) with Ksp = 1.8e-10 and molar mass = 143.32 g/mol.

How to use

Set direction to 'Ksp → molar solubility s', select 'AB — 1:1', input 1.8e-10 as Ksp, select 'M' as the solubility unit, and enter 143.32 in the molar mass field.

Direction: ksp-to-s, Salt: ab, Ksp: 1.8e-10, Unit: M, Molar Mass: 143.32 g/mol

Outcome

Returns molar solubility s = 1.34164e-5 mol/L, individual ion concentrations [Ag⁺] = [Cl⁻] = 1.34164e-5 mol/L, and mass solubility = 1.92284e-3 g/L.

2. Deriving Ksp for Calcium Fluoride from Measured Solubility

Lab Technician

Background

Testing fluoride salt dissolution in water where calcium fluoride (CaF₂) reaches saturation at 0.25 mM.

Problem

Calculate the solubility product constant Ksp for a 1:2 salt given a solubility of 0.25 mmol/L and molar mass of 78.08 g/mol.

FAQ

What salt stoichiometries are supported by this calculator?

The calculator supports AB (1:1, Ksp = s²), AB₂ or A₂B (1:2/2:1, Ksp = 4s³), AB₃ or A₃B (1:3/3:1, Ksp = 27s⁴), and A₂B₃ or A₃B₂ (2:3/3:2, Ksp = 108s⁵).

Can I input molar solubility in units other than mol/L?

Yes, you can enter or receive molar solubility in Molarity (M, mol/L), Millimolarity (mM, mmol/L), or Micromolarity (µM, µmol/L).

How does the tool calculate mass solubility in g/L?

When an optional molar mass (g/mol) is provided, the tool multiplies the molar solubility (in mol/L) by the molar mass.

Does this calculation account for common-ion effects or complex ion formation?

No, it computes standard equilibrium solubility in pure water based on the stoichiometric dissolution equilibrium.

How do I enter scientific notation for very small Ksp values?

You can use standard exponential notation directly in the numeric input, such as 1.8e-10 for 1.8 × 10⁻¹⁰.

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How to use

Set direction to 'Molar solubility s → Ksp', select 'AB₂ / A₂B — 1:2 or 2:1', input 0.25 as solubility, set unit to 'mM', and provide 78.08 for molar mass.

Direction: s-to-ksp, Salt: ab2, Solubility: 0.25, Unit: mM, Molar Mass: 78.08 g/mol

Outcome

Yields Ksp = 6.25000e-11 using the 4s³ relationship, with equilibrium ion concentrations [Ca²⁺] = 2.50000e-4 mol/L and [F⁻] = 5.00000e-4 mol/L, plus mass solubility = 0.01952 g/L.