At temperature, a number of solute grams can dissolve in 100 milliliters of solvent {solubility}|. If solubility is greater than one percent, solute can dissolve well in solvent {soluble}.
water solubility
Compounds have solubility in water {aqueous solubility}. Nitrates, acetates, chlorides, bromides, most iodides, most sulfates, sodium salts, potassium salts, and ammonium salts are soluble in water.
Hydroxides except sodium hydroxide and potassium hydroxide; sulfides except sodium sulfide, magnesium sulfide, and aluminum sulfide; arsenates except sodium arsenate and potassium arsenate; carbonates except sodium carbonate and potassium carbonate; and phosphates except sodium phosphate and potassium phosphate are insoluble in water.
precipitation
Solubility is maximum concentration before precipitation from solvent. For precipitation, concentration product {solubility product} must be greater than equilibrium constant.
factors
Solute solubility in solvent depends on solute polarity, size, and surroundableness and solvent polarity, size, and surroundability.
factors: temperature
Higher temperature increases solubility, because increased random motion breaks up and mixes solute and solvent more.
factors: concentration
Low concentration increases solubility, because solvent molecules can better surround solute molecules, with less solute molecules near other solute molecules.
factors: stirring
Stirring increases solubility, because more motion mixes solute and solvent more.
factors: ions
More hydrogen ion increases solubility in polar solvent, by increasing polarity. More ions increase solubility in polar solvent, by increasing polarity.
Ionic solutes with large ions and large charges are harder to dissolve. Ionic solutes with small ions and charges of +1 or -1 are easier to dissolve. Large ions with charge +1 or -1 dissolve better than small ions with charge +2, -2, +3, -3, or greater. Salts with small volume, especially hydrogen ions and acids, increase solubility by allowing more shielding. Higher-charge salts increase solubility more, because they shield better. Salts that form metal-ion complexes increase solubility, by more shielding.
factors: common ion
Low concentration of ion common to two solutes increases solubility, because solvent molecules can better surround solute molecules, with less solute molecules near other solute molecules. Common ion provides more molecules for collision. Solubility decreases if common ion is present in large amounts, because the other ion must then be at low concentration to equal solubility product.
factors: diverse ion
Solubility increases if diverse ion is present, because charges have more shielding and polarity increases.
factors: polarity
Similar-polarity molecules dissolve each other best, because electrical attractions for similar molecules are stronger.
factors: size
Small molecules dissolve better, because solvent molecules can better surround solute molecules.
factors: shape
Spherical molecules dissolve better than elongated ones, because solvent molecules can better surround spherical molecules.
When water molecules surround ions, energy {energy of hydration} {hydration energy}| releases. Small atoms have more hydration than large ones, because water surrounds them better.
Solvent molecules can surround other-substance {solute} molecules.
Solubility can decrease by adding salt with common ion and higher solubility, to make higher concentration and force solute out of solution {common ion effect}.
Ions in solution increase polarity and increase solubility {Debye-Hückel law}.
5-Chemistry-Inorganic-Phase-Solution
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Date Modified: 2022.0225