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Intro to Solubility - Coggle Diagram
Intro to Solubility
Saturated
Occurs during the production of a solution, when a substance can no further be dissolved in a solvent and there are visible amounts of the substance in a separate phase.
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Precipitate
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Example: KCl + AgNO3 -> AgCl + KNO3, AgCl is a precipitate
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Solvent
A substance that dissolves a solute, resulting in a solution.
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Unsaturated
Occurs during the production of a solution, when a substance continues to dissolve in a solvent with no visible amounts of the substance appearing in a separate phase.
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Molarity
Molarity (M) is calculated by taking the moles of solute and dividing it by the volume of solution in litres - mol/L
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Conductivity
Conductivity of a substance can be measured by the ease at which heat or an electrical charge can pass through the substance.
Electrolyte
A solution that easily conducts electricity is considered an electrolyte solution. A solution that has a weak conduction of electricity does not conduct electricity well. A non-electrolyte solution cannot conduct electricity at all.
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Compounds
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Ionic Compounds
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Ionization
Example: 2H2O -> H3O(+) + OH(-). The hydronium is a cation, and the hydroxide is an anion.
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Cation
An ion with fewer electrons than protons, giving it a positive charge.
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Anion
An ion with fewer protons than electrons, giving it a negative charge.
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Solubility
Solubility is determined by a production of a saturated solution by dissolving a substance in a solvent at specified temperature and pressure.
