Term
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Definition
| it is a homogenous mixture of two or more compounds in a single phase: liquid, solid and or gas |
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Term
| give an example of a solid solution |
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Definition
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Term
| what is an ideal solution |
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Definition
| solutions made from compounds that have similar properties-for instances: a solution of benzene and toluene-similar size and similar bonding properties |
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Term
| what is an ideally dilute solution |
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Definition
| the solute is completely seperated by the solvent, so there are no interactions between them |
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Term
give examples of a colloidal system
and
a brief description of it |
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Definition
aerosal, foam, an emulsion (milk or butter) & sol (paint)
so, this is a solution only the solute particles are usually too small to be extracted by filtration |
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Term
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Definition
| heating or introducing a solute into a colloidal system-the larger particles will settle out and then can be filtered out |
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Term
| how are ionic compounds dissolved |
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Definition
| solvation- ionic bonds are dissolved into a polar solvent, so that the cations and anions form bonds with their oppositely charged ends of the polar solvent |
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Term
| what does the compound nitrite look like |
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Definition
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Term
| what does the compound hypochlorite look like |
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Definition
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Term
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Definition
| moles of the compound divided by the volume of the solution |
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Term
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Definition
| moles of solute divided by kilograms of solvent |
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Term
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Definition
| the number of moles of solute divided by the total number of moles in solution |
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Term
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Definition
| mass of the solute divided by the total mass of the solution times 100 |
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Term
| what is parts per million |
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Definition
| mass of solute divided by total mass of solution times 10^6 |
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Term
context: acid-base reaction
what does is mean if H2SO4 is called a 2 normal solution |
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Definition
| it means that it can donate 2 protons for each H2SO4 |
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Term
| if given the specific gravity (1.006 kg) of a compound, how would you determine how many moles it had within it |
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Definition
| since water weighs 1 kg, subtract that form 1.006 kg and you get about 6 g. 6g/ the molecular weight of the compound to get moles |
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Term
| when determining solubility, what should you look for |
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Definition
look for very polar functional groups (N,O) something super electronegative
second, look for ionic bonding molecules
third, look for non polar (least soluble in water) |
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Term
| context: the air we breathe is approximately 21% O and 79% . if the partial pressure of nitrogen in air is 600 torr, what can you automatically exclude from this question |
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Definition
| partial pressure refers to number of particles not, the mass |
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Term
| at constant pressure, how can you determine the ethalpy of a reaction |
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Definition
| well, since at constant pressure the ethalpy of a reaction is equal to the change in heat-ethalpy can be equal to the change of heat in step 1: breaking of intermolecular bonds in the solute, change of heat in step 2: breaking of intermolecule bonds in the solvent, and change of heat in step 3: formation of intermolecular bonds between solvent and solute |
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Term
context: solution formation
the first two steps are:
the last step is: |
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Definition
| endothermic and the last step is exothermic |
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Term
| a negative heat of solution results in |
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Definition
| stronger intermolecular bonds and will give off heat |
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Term
| a positive heat of solution results in |
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Definition
| weaker intermolecular bonds |
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Term
| since separate pure substances are more orderly than a solution, the overall entropy of the solution what |
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Definition
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Term
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Definition
in an air tight seal, water molecules will break their intermolecular bonds to form water vapors molecules
once the molecules leaving the liquid equals the rate of molecules entering the liquid |
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Term
| how can you increase vapor pressure |
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Definition
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Term
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Definition
| when the vapor pressure of a solid equals the atmospheric pressure |
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Term
| what does Raoult's law for non volatile solutes say |
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Definition
| if 97% of the solution is solvent, then the vapor pressure will be 97% of the vapor pressure of a pure solvent |
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Term
| what does Raoult's law for volatile solvents say: |
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Definition
| if 97% of the solution is solvent, then the vapor pressure will be 97% of the vapor pressure of the pure solvent and 3% vapor pressure of pure solute |
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Term
| given a negative heat of solution, what can be said about that mechanisms vapor pressure |
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Definition
| negative heat of solution means stronger intermolecular bonds are formed and vapor pressure is lowered |
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Term
| the solubility product will only change with a change in |
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Definition
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Term
| according to le chatalier's principle, when a common ion effect is added to an already existing ion solution in equilibrium, what will happen |
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Definition
| since there is an added ion, it will push it back to the left and form more precipitate |
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Term
| pressure on liquids and solids has little effect, but pressure on a gas |
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Definition
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Term
| when the volatile solute concentration is low, each molecule is surrounded by solvent molecules creating deviation from the behavior of |
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Definition
pure volatile solute
thus its vapor partial pressure is not proportional to its pressure as a pure volatile solute |
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Term
| the solubility of salts tends to what with an increase in temeprature |
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Definition
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Term
| the solubility of gases tends to what when temperature is increased |
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Definition
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Term
| when a solution is saturated, what does this mean in terms of solute and solvent concentrations |
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Definition
| solute is maximized and solvent is minimized |
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