Term
| Solubility rules for aqueous solutions |
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Definition
1. All salts containing ammonium and alkali metal (group 1) cations are water-soluble
2. All nitrate salts (NO3-) and acetate anions are water-soluble
Other rules need familiarity but only memorize these two |
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Term
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Definition
| moles of substance of interest divided by the total moles of all species |
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Term
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Definition
| moles of solute divided by kilograms of solvent |
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Term
| Equation for determining solubility product constant |
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Definition
Ksp = [An+]m[Bm-]n
A and B are the concentrations of the ions in solution |
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Term
| What is the common ion effect? |
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Definition
| This is observed when the molar solubility of a compound is reduced because one of its constituent ions is already dissolved into the solution at some concentration |
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Term
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Definition
Accounts for vapor pressure depression caused by solutes in solution. As solute is added to a solvent, the vapor pressure of the solvent decreases.
PA = XAPoA
X is the mol fraction of solvent A
Po is the vapor pressure of solvent A in its pure state
P is the new vapor pressure with solute dissolved in it |
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Term
| What is the equation for determining if a solute is saturated or unsaturated? |
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Definition
IP = [An+]m[Bm-]n
IP is the ion product.
IP > Ksp supersaturation → precipitation
IP < Ksp unsaturated → nothing
IP = Ksp saturated → solution at equilibrium |
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Term
| Osmotic pressure equation |
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Definition
Π = iMRT
Π is the osmotic pressure
i is the van't Hoff factor
M is molarity of the solution
R is the ideal gas consant
T is temperature |
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