Gen Chem 4 solutions.txt

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• Def solution, solvent, solute
• Solution: Is a homogenous mixture of two or more compounds in a single phase
• Solvent: the compound of which there is more
• Solute: compound of which there is less

• Ideal solutions: compounds with similar properties. Changing the amount of either compounds will not change spacial arrangement or I enter molecular interaction between molecules.
• Ideal dilute: solute molecules are completely separated by solvent ,molecules so the solvent molecules do not interact with each other
• Non ideal: violate both conditions

Colloid: like a solution, but particles are larger. Too small for filtration, but large enough to seperatd by a membrane. Aerosols are an example, also detract light

Solvation: ionic compounds breaking apart into cations and anion constituents in solvent

• Hydration: a type of solvation done in water. Water molecules surround ions.
• Aqueous phase: when hydration occurs, the compound is said to be in aqueous phase

Electrolyte: a found which forms an ion in aqueous phase giving the water electrical conductivity is a electrolyte

NO2-

NO3-

SO3 2-

SO4 2-

ClO-

ClO2 -

ClO3 -

ClO4 -

CO3 2-

HCO3 -

PO4 3-

M=moles solute/vol solution

m=moles solute/kg solvent

X=moles of solute/(total moles of solution)

Mass %= [(mass solute)/(total solution mass)]x100

ppm= (mass solute/total mass solution) x10^6

• 1: breaking intermolecular bonds in solute
• 2: breaking intermolecular bonds in solvent
• 3: formation of intermolecular bands between solvent and solute

Heat of solution: summation of enthalpy after each step of forming a solution. The heat of solution will be (+) endothermic or (-) exothermic

• Raoult's law: describes vapor pressure of a solution.
• Pv= XaPa
• Vapor pressure = mole fraction of the
• Liquid times vapor pressure of a pure liquid

• Nonvolatile solutes lower Pv. This means the vapor pressure will some percentage of the pure liquid vapor pressure
• Volatile solutes add to vapor pressure. This means vapor pressure will be a fraction of the pure vapor pressure plus the present fraction of the volatile substance vapor pressure

Positive heat of formation means the energy was added to the system so the bonds are weaker than before. Therefore the vapor pressure increases. Negative heats of formation are opposite and lower vapor pressure

• Solubility: a solvents tendency to dissolve solvent
• Precipitation: reverse of dissolving
• Saturated: dissolution and precipitation rates are in equuilibrium

Ksp=[products]\[reactants] solids and pure liquids are excluded

• Solubility: max number of moles that can dissolve in a solvent. Changes with temperature and ions
• Solubility product: a constant from a book and changes with temp only

• Spectator ions: is an ion not part of the equilibrium expression and has no effect equilibrium
• Common ion effect: is an ion in the equilibrium expression. Addition to a saturated solution will change equilibrium

Solubility of a gas is proportional to its vapor partial pressure. Vapor pressure decrease = solubility decrease. Think opening a soda can

Ideally dilute solution obeys raoults law, solute obeys Henrys law