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Introduction to Chemical Solutions and Equilibria, Exams of Chemistry

Miami University - MiddletownChemistry

A comprehensive overview of various concepts related to chemical solutions and equilibria, including the properties of solutions, colligative properties, chemical kinetics, chemical equilibrium, acid-base chemistry, and coordination compounds. It covers key topics such as the characteristics of solutions (solvent, solute, solubility), factors affecting reaction rates, the laws of mass action, le chatelier's principle, acid-base theories, and the properties of transition metals and their complexes. The document aims to equip students with a solid understanding of these fundamental chemical principles, which are essential for success in chemistry courses and related fields.

Typology: Exams

2023/2024

Available from 10/22/2024

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CHM 142 final exam with correct solution 2024/2025
solution - **- evenly spread or "homogenous" mixture of two or more substances
- Can have a combo of 3 phases of matter
solvent - **Substance present in the largest amount
solute - **Any substance in a smaller amount
solubility - **Degree to which a substance can dissolve in a given solvent
unsaturated - **- Contains less solute than it has the capacity to dissolve
- Stable when disturbed
saturated - **- Contains maximum amount of a solute that can dissolve
supersaturated - **- Contains more dissolved solute
- Small disturbance causes solute to crystalize
instantaneous dipole - **- Inducing a nearby nonpolar molecule
- Larger molecules generate larger dipole when they are induced
- Solutes more soluble in a solvent if they have greater IMFS
like dissolves like - **- Substances with similar types and magnitudes of
intermolecular forces in their pure forms will be the most soluble in solution
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CHM 142 final exam with correct solution 2024/

solution - **- evenly spread or "homogenous" mixture of two or more substances

  • Can have a combo of 3 phases of matter solvent - **Substance present in the largest amount solute - **Any substance in a smaller amount solubility - **Degree to which a substance can dissolve in a given solvent unsaturated - **- Contains less solute than it has the capacity to dissolve
  • Stable when disturbed saturated - **- Contains maximum amount of a solute that can dissolve supersaturated - **- Contains more dissolved solute
  • Small disturbance causes solute to crystalize instantaneous dipole - **- Inducing a nearby nonpolar molecule
  • Larger molecules generate larger dipole when they are induced
  • Solutes more soluble in a solvent if they have greater IMFS like dissolves like - **- Substances with similar types and magnitudes of intermolecular forces in their pure forms will be the most soluble in solution

what will form a solution - **- Two polar molecules

  • A nonpolar molecule and a polar molecule what will not form a solution - **- A polar and nonpolar molecule colligative properties - **- Depends on the number of solute particles
  • Do not depend on the nature of the solute particles vapor pressure - **- Pressure exerted by the molecules that have escaped to the gas phase, once pressure has stopped increasing
  • Reduced by presence of a solute semipermeable membrane - **- Allows the passage of solvent molecules but blocks the passage of solute molecules chemical kinetics - **- Study of how fast reactions take place what causes a chemical reaction slow down - **as reactants are consumed secant line - **- Line which intersects two points on the curve
  • Correspond to the "average rate" tangent line - **- Intersects curve at a single point perpendicular to normal line
  • Correspond to "instantaneous rate"

Boltzmann distribution - **Distribution widens at higher temperatures elementary reaction - **- Reaction that describes an individual collision or single molecule decomposition

  • Each step as a rate law chemical reaction - **Reaction that describes the chemical conversion of reactants to products that are both observable at the macroscopic level enzyme kinetics - **Predicts the saturation concentration indicating when all active sites are occupied by substrate chemical equilibrium - **- State in which forward and reverse processes are occurring at the same rate
  • Results in unchanging concentrations of reactants and products at the macro scale
  • Forward and reverse reactions are still taking place at equilibrium laws of mass action - **Build Qc or Kc from an overall reaction Qc - **- Changed throughout a chemical reaction
  • Moves toward Kc as time goes on Kc > 1 - **reaction goes to completion Kc is not large - **reaction occurs but does not go to completion Kc < 1 - **reaction does not occur to a significant amount

Qc < Kc - **There are more reactants and less product than at equilibrium Qc = Kc - **There are reactants and products with concentration at equilibrium conditions Qc > Kc - **There are more products than reactants homogeneous equilibrium - **All reactants and products involved in an equilibrium have the same phase Le Chatelier's principle - **- When a stress is applied to a system at equilibrium, the system will respond by shifting in the direction that minimizes the effect a stress - **- Addition of a reactant or product

  • Removal of a reactant or product
  • Change in volume that impacts concentration or partial pressure
  • Change in temp
  • Causes changes to Qc Delta n > 0 - **- Compression: shift towards reactant
  • Expansion: shift towards products Delta n < 0 - **- Compression: shift towards product
  • Expansion: shift towards reactants

Amphoteric - **Chemical species that may behave as either a bronsted acid or base Autoionization of water - **Water can react with itself weak acids - **- Only partially ionize in water

  • strong conjugate base Weak base - **- Only partially accept a proton in water
  • strong conjugate acid If X and Y are both inert - **Solution is neutral Lewis acid - **a species that can accept a pair of electrons Lewis base - **species that can donate a pair of electrons Curly arrow notation - **- A common notation in organic chemistry that depicts the movement of electrons in a chemical reaction
  • Double headed: electron pair moving
  • Single headed: one electron moving Coordination compounds - **- Have coordinate covalent bonds formed by the reactions of metal ions with groups of anions or polar molecules
  • Can be geometric or optical

Coordinate covalent bond - **Covalent bond in which one of the atoms donates both of the electrons that add to the bond Complex ion - **- What a coordination compound consists of

  • One or more counter ions Incompletely filled d subshells - **- Distinctive colors
  • Formation of paramagnetic compounds
  • Catalytic activity
  • Tendency to form complex ions Transition metals have - **- Higher densities
  • Higher melting points and boiling points
  • Higher heats of fusion and vaporization than the main group and group 12 Ligands - **- Molecules or ions that surround the metal in a complex ion
  • Must have at least one unpaired valence electrons
  • Act as a lewis base
  • Transition metal acts as a lewis acid First coordination sphere - **Species with a secondary valence Second coordination sphere - **Species with a primary valence Donor atom - **Atom in a ligand that is bound directly to the metal atom
  • Always rotate the plane of polarization by the same amount, but in opposite directions Racemic mixture - **- Equimolar mixture of two enantiomers
  • Net rotation is zero Small "K' - **slightly soluble or insoluble Solubility - **degree to which a substance can dissolve in a given Common ion effect - **when a cation or anion is present between 2 soluble compounds, when combined in a solution, it pushes the equilibrium towards the neutral (reactants) An insoluble or slightly soluble salt with a SCB or OH- (with a metal cation) will be more soluble in - **acidic solutions Buffer - **- solution that contains significant concentrations of both members of a conjugate pair
  • Resist change to pH when small amounts are added Equivalence point - **- when moles H+ = moles OH-
  • pH is 7 because it is neutralized Weak acid- strong base curve - **- Point before equivalence point is the buffer region
  • pH above 7
  • Half equivalence point: pH = pKa ways to make a buffer - **- Method 1: add an acid or base and conjugate base or acid in similar amounts
  • Method 2: add a strong acid or base and a weak base or acid. The added amounts are not equal amounts but can't exceed the buffer region Spontaneous - **- process that occurs under a specific set of conditions
  • Positive Nonspontaneous - **doesn't occur under a specific set of conditions Entropy - **is a state function that describes how dispersed a systems energy is Microstates - **number of different ways a molecule in a system that can be arranged with its current energy Entropy increases as W increases - **- Creating new states in the system which can be accessed
    • Phase change to gas
    • Increase in volume
    • Mixing ideal gasses and solution
    • Increases particles
    • Increase in molecular complexity
  • Making states in the system accessible that were not originally
    • Increase temperature