Chem Lec Exam 3

• Solution: a homogenous mixture of two or more substances such as alloys and air
• Aqueous Solution: A solution where water is the solvent.
• Solute: the component of a solution that is present in lesser quantity
• Solvent: the solution component present in the largest quantity
• Solubility: how much of a particular solute can dissolve in a certain solvent at a specified temperature
• Saturated solution: a solution that contains all the solute that can be dissolved at a particular temperature
• Supersaturated: contains more solute than can be dissolved at the current temperature
• Concentration: amount of solute dissolved in a given amount of solution.
• 1,000 mL = 1 L
• Mass/Volume percent or %(m/v) = g of solute / mL of solution x 100%
• Molarity: defined as the number of moles of solute per liter of solution
• Molarity= mol of solute / L of solution
• moles of solute = (M) (L of solution)
• Dilution is required to prepare a less concentrated solution from a concentrated solution
• Dilution equation: M1V1=M1V2
• Colligative properties are properties of solution that depend on the concentration of the solute particles, rather than the identity of the solute
• Colligative properties are vapor pressure lowering, boiling point elevation, freezing point depression, and osmotic pressure
• Raoult's law: when a nonvolatile solute is added to a solvent, the vapor pressure of the solvent decreases in proportion to the concentration of the solute
• Molality: moles of solute per kg of solvent
• Molality = mol solute / kg of solvent
• Diffusion involves the movement of solvent molecules
• Osmosis is the movement of solvent from a dilute solution to a more concentrated solution through a semipermeable membrane. It stops when both concentrations are the same.
• Osmolarity is the molarity of particles in solution. Osmolarity = i x M (i = # of mole particles/ mole solute, M = molar concentration of solute)
• Osmotic pressure (π) is the amount of pressure required to stop the flow across a semipermeable membrane. π = iMRT (i = # of mol particles/ mol solute, M= molar concentration of solute, R= ideal gas constant, T= solution temperature (K) )
• Amphiprotic is a substance possesing both acid and base properties
• Arrhenius theory: 1) Acid is a substance that when dissolved in water dissociates to produce hydrogen ions 2) Base is a substance that when dissolved in water dissociates to produce hydroxide ions
• Hydrogen ion is also known as proton and is responsible for acidity
• OH- is responsible for basicity
• Bronsted-Lowry theory: 1) Acid is a proton (H+) donor 2) Base is a proton (H+) acceptor
• 1 - Meth, 2- Eth, 3- Prop, 4- But, 5- Pent, 6- Hex, 7- Hept, 8- Oct, 9- Non, 10- Dec
• Prefixes for ethyl groups: di, tri, tetra. ex: 4,4,6- triethyl
• Conjugate acid: what the base becomes after it accepts a proton
• Conjugate base: what the acid becomes after it donates its proton
• Conjugate acid-base pair: The acid and base on the opposites sides of the equation
• Strong acids include: hydrochloric acid (HCl), Nitric acid (HNO3), Sulfuric acid (H2SO4)
• Weak acids and bases do not dissociate completely
• H3O+ is called a hydronium ion.
• Carbon can form up to 4 covalent bonds and form double or triple bonds
• A hydrocarbon is a molecule that contains only hydrogen and carbon atoms
• Hydrocarbons are classified into aromatic and aliphatic