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Chemistry Unit 10

QuestionAnswer
Solution Homogeneous mixture of two or more substances in a single physical state
Solute Substance being dissolved (less of this)
Solvent Substance doing the dissolving (more of this)
Aqueous (aq) Solutions with water as solvent. Universal solvent because it dissolves so many substances. When water is the solvent the solute particles are hydrated
Alloys Solid solution of 2 or more metals
Air All gas mixtures are homogeneous solutions
Gas/Liquid Soda/pop: CO2 dissolved in water
Liquid/Liquid antifreeze: ethylene glycol in water, gasoline
Solid/Liquid Salt dissolved in water: aqueous
Rate of solution How fast a solute dissolves in solvent
Temperature (solids & liquids) As temp increases, rate of solution increases (dissolves faster). Increased temp= increased KE and motion of molecules
Stirring As stirring increases, rate of dissolving (solution) increases. Brings solute into contact with fresh solvent
Particle Size (surface area) As particle size decreases, rate of dissolving (solution) increases. Brings more of the solute into contact with solvent
Solubility How many grams of a substance can be dissolved in a given quantity of solvent at a specific temperature and pressure
Solids and Liquids Increasing temperature results in increased solubility. direct relationship
Gases As temp increases the amount of gas to that can be dissolved decreases. inverse relationship
Pressure As pressure increases, solubility of a gas increases. Keep soda bottle closed to maintain pressure and keep gas in solution. Solids and liquids not affected by pressure
Nature of the solvent/solute "like dissolves like". Polar solvent dissolves polar solute
Water Polar; grease = non-polar; soap: polar and non-polar end allows grease removal
NaCl Ionic (ionic substances are the extreme of polarity) so it can be dissolved in water
Qualitative Desprictive observation without numbers; more general; nit a specified amount.
Dilute Only a little solute is dissolved
Concentrated A lot of solute is dissolved
Saturated Contains the maximum amount of solute at a given temperature. No more can be dissolved. On line
Unsaturated Contains less than the max amount of solute at a given temperature. More can be dissolved. Below line
Supersaturated Holds more than the maximum amount at given temp and pressure. Above Line
Quantitative Describes the numerical concentration of a solution
Making Dilutions equation M1 V1 = M2 V2
%Mass Mass of solute/mass of solution x 100%
Parts Per Million Used when tiny amounts of solute are dissolved in a solvent
Colligative Properties The presence of dissolved particles and the amount of dissolved particles affects some solvent properties: (more solute, greater effect). Boiling point: increases Freezing point: decreases Vapor pressure: decreases (harder to evaporate)
Boiling Point Elevation The presence of a nonvolatile (won't evaporate away) solute always increases the boiling point
Freezing Point Depression The presence of a solute always decreases the freezing point of a solvent
Ionic Compounds (metal + nonmetal) Break apart (dissociate) into for form particles. Electrolytes conduct electricity
Covalent Compounds Do not break apart into particles when dissolved on a solvent. Non electrolytes do not conduct electricity
Vapor When a solid or liquid enters the gas phases through evaporation
Vapor pressure Pressure exerted by particles in the gas phases. The easier it is to evaporate the higher the vapor pressure
Normal Boiling Points A liquid boils when vapor pressure equals atmospheric pressure
Lower than standard pressure Liquids boil at a temperature lower than normal. High elevation = lower pressure
Higher than standard pressure Liquids boil at a temperature higher than normal
Created by: user-1866784
 

 



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