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Chem Ch5

컨트롤 버튼이 '내비게이션' 모드로 변경되었습니다.
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이 집합의 용어 (27)

  • What is a solution?
    A solution is a homogeneous mixture where the majority component is the solvent and the minority component is the solute.
  • What defines an aqueous solution?
    An aqueous solution is a solution in which water is the solvent.
  • Difference between dilute and concentrated solutions
    Dilute solutions have a small amount of solute compared to solvent, while concentrated solutions have a large amount of solute compared to solvent.
  • How is molarity defined?
    Molarity (M) is the amount of solute in moles divided by the volume of solution in liters, expressed as \(M=\frac{moles\ solute}{liters\ solution}\).
  • How to prepare 1 L of 1.00 M NaCl solution?
    Weigh 1.00 mol of NaCl, dissolve it in water, and add water until the total volume reaches 1 liter.
  • Using molarity as a conversion factor
    Molarity can convert between moles of solute and liters of solution, e.g., 0.500 M NaCl means 0.500 mol NaCl per liter of solution.
  • What happens during solution dilution?
    Dilution involves adding solvent to a concentrated stock solution, increasing volume but keeping the amount of solute constant.
  • How to calculate moles from volume and molarity?
    Moles of solute = Molarity × Volume of solution (in liters).
  • What are electrolytes and nonelectrolytes?
    Electrolytes dissolve in water to form ions and conduct electricity; nonelectrolytes dissolve as molecules and do not conduct electricity.
  • Difference between strong and weak electrolytes
    Strong electrolytes completely dissociate into ions; weak electrolytes partially ionize in solution.
  • What causes a solute to dissolve in a solvent?
    Solute dissolves if the attraction between solute and solvent molecules is strong enough to overcome solute-solute and solvent-solvent attractions.
  • Charge distribution in a water molecule
    Water has a partial negative charge on oxygen and partial positive charges on hydrogens due to uneven electron distribution.
  • How do ionic compounds dissolve in water?
    Ions are pulled from the crystal lattice and surrounded by water molecules, allowing free movement and electrical conductivity.
  • What is a precipitation reaction?
    A reaction where two aqueous solutions mix and form an insoluble solid called a precipitate.
  • How to predict precipitation reactions?
    Identify ions in reactants, exchange ions to form products, use solubility rules to determine if products precipitate.
  • What is a molecular equation?
    A chemical equation showing complete, neutral formulas for all compounds as if they existed as molecules.
  • What is a complete ionic equation?
    An equation showing all strong electrolytes as ions, with insoluble substances and weak electrolytes as molecules.
  • What is a net ionic equation?
    An ionic equation with spectator ions removed, showing only species that change during the reaction.
  • What defines an acid and a base according to Arrhenius?
    An acid produces \(H^+\) ions in aqueous solution; a base produces \(OH^-\) ions.
  • What is a neutralization reaction?
    An acid-base reaction where an acid and base react to form water and a salt, neutralizing each other's properties.
  • What is a titration?
    A laboratory procedure where a solution of known concentration (titrant) is used to determine the concentration of an unknown solution (analyte).
  • What is the equivalence point in titration?
    The point where the moles of acid and base are stoichiometrically equal and completely reacted.
  • What are gas-evolution reactions?
    Reactions in aqueous solution that produce a gas, often accompanied by bubbling.
  • What is oxidation and reduction?
    Oxidation is the loss of electrons; reduction is the gain of electrons.
  • What is an oxidizing agent and reducing agent?
    The oxidizing agent causes oxidation and is itself reduced; the reducing agent causes reduction and is itself oxidized.
  • How are oxidation states assigned?
    Oxidation states are assigned based on rules considering element type, charge, and bonding, representing hypothetical charges.
  • What is the activity series of metals?
    A list of metals ranked by their tendency to lose electrons; metals higher in the series oxidize more easily.