Chemistry Chapter: Liquid Solutions
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Questions and Answers

What type of solution is formed when a solid solute is added to a liquid solvent?

A liquid solution

What are the main components of a homogeneous mixture?

Solvent and solute

Which of the following components is typically present in the largest quantity in a solution?

  • It depends on the specific solution
  • Both solute and solvent are present in equal quantities
  • Solvent (correct)
  • Solute

    • What type of solution refers to a solution that contains two components, namely, the solvent and the solute?

    <p>Binary solution</p> Signup and view all the answers

    The concentration of a solution can be described qualitatively and quantitatively.

    <p>True</p> Signup and view all the answers

    What does the mass percentage (w/w) of a component represent?

    <p>The mass of the component in the solution divided by the total mass of the solution, multiplied by 100</p> Signup and view all the answers

    What is the formula for volume percentage (V/V) of a component?

    <p>(Volume of component/Total volume of solution) × 100</p> Signup and view all the answers

    What does the mass by volume percentage (w/V) represent?

    <p>Mass of solute dissolved in 100 mL of the solution</p> Signup and view all the answers

    How is the concentration of a solute expressed when it is present in trace quantities?

    <p>Parts per million (ppm)</p> Signup and view all the answers

    What is the formula for calculating parts per million?

    <p>(Number of parts of component/Total number of parts of all components in solution) × 10⁶</p> Signup and view all the answers

    Concentration in parts per million can be expressed as mass to mass, volume to volume, and mass to volume.

    <p>True</p> Signup and view all the answers

    What is the symbol commonly used for mole fraction?

    <p>x</p> Signup and view all the answers

    What is the formula for calculating the mole fraction of a component?

    <p>(Number of moles of component / Total number of moles of all components)</p> Signup and view all the answers

    In a binary mixture, what is the formula for calculating the mole fraction of component A?

    <p>n_a / (n_a + n_b)</p> Signup and view all the answers

    The sum of all mole fractions in a given solution is equal to 1.

    <p>True</p> Signup and view all the answers

    What is the definition of molarity?

    <p>The number of moles of solute dissolved in one liter (or cubic decimeter) of the solution</p> Signup and view all the answers

    What is the formula for calculating molarity?

    <p>(Moles of solute / Volume of solution in liters)</p> Signup and view all the answers

    The solubility of a substance is its maximum amount that can be dissolved in a specified amount of solvent.

    <p>True</p> Signup and view all the answers

    What factors affect the solubility of a substance?

    <p>All of the above</p> Signup and view all the answers

    The solubility of solids in liquids is generally not significantly affected by pressure.

    <p>True</p> Signup and view all the answers

    What happens to the solubility of a solid in a liquid when the dissolution process is endothermic?

    <p>Solubility increases with increasing temperature</p> Signup and view all the answers

    Solubility of gases in liquids is significantly affected by pressure.

    <p>True</p> Signup and view all the answers

    What is the statement of Henry's law?

    <p>At a constant temperature, the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas present above the surface of the liquid.</p> Signup and view all the answers

    What is the mathematical expression of Henry's law?

    <p>p = KH * x</p> Signup and view all the answers

    What happens to the solubility of a gas in a liquid as the temperature increases?

    <p>Solubility decreases</p> Signup and view all the answers

    The solubility of liquids in liquids is not significantly affected by pressure.

    <p>True</p> Signup and view all the answers

    What is the definition of vapor pressure?

    <p>The pressure exerted by the vapor of a liquid over the liquid phase at equilibrium conditions.</p> Signup and view all the answers

    What are the two important properties of ideal solutions?

    <p>Both A and B</p> Signup and view all the answers

    Henry's law is a special case of Raoult's law.

    <p>True</p> Signup and view all the answers

    What is the definition of an ideal solution?

    <p>A solution that obeys Raoult's law over the entire range of concentration.</p> Signup and view all the answers

    What is Raoult's law?

    <p>The partial vapor pressure of each volatile component in a solution is directly proportional to its mole fraction.</p> Signup and view all the answers

    What type of deviation from Raoult's law is observed when the intermolecular forces between solute and solvent molecules are weaker than the intermolecular forces between solute-solute and solvent-solvent molecules?

    <p>Positive deviation</p> Signup and view all the answers

    What type of deviation from Raoult's law is observed when the intermolecular forces between solute and solvent molecules are stronger than the intermolecular forces between solute-solute and solvent-solvent molecules?

    <p>Negative deviation</p> Signup and view all the answers

    What is an azeotrope?

    <p>A binary mixture that has the same composition in both its liquid and vapor phases and boils at a constant temperature.</p> Signup and view all the answers

    What type of azeotrope is formed when a solution shows a large positive deviation from Raoult's law?

    <p>Minimum boiling azeotrope</p> Signup and view all the answers

    What are colligative properties?

    <p>Properties of solutions that depend only on the number of solute particles and are independent of their chemical identity.</p> Signup and view all the answers

    Colligative properties are useful for determining the molar mass of solutes.

    <p>True</p> Signup and view all the answers

    What is osmosis?

    <p>The movement of solvent molecules from a region of higher solvent concentration to a region of lower solvent concentration through a semipermeable membrane.</p> Signup and view all the answers

    What is osmotic pressure?

    <p>The excess pressure that must be applied to a solution to prevent osmosis.</p> Signup and view all the answers

    What is the formula for osmotic pressure for dilute solutions?

    <p>Π = CRT</p> Signup and view all the answers

    The osmotic pressure method is a useful technique for determining the molar masses of biomolecules.

    <p>True</p> Signup and view all the answers

    What are isotonic solutions?

    <p>Solutions having the same osmotic pressure at a given temperature.</p> Signup and view all the answers

    Reverse osmosis is a process where pure solvent flows out of the solution, through a semipermeable membrane, when pressure greater than osmotic pressure is applied to the solution side.

    <p>True</p> Signup and view all the answers

    Abnormal molar masses are observed when a solute dissociates into ions or associates into larger molecules.

    <p>True</p> Signup and view all the answers

    What is the van't Hoff factor?

    <p>A factor that accounts for the extent of dissociation or association of a solute.</p> Signup and view all the answers

    For strong electrolytes, the van't Hoff factor approaches the number of ions produced per formula unit as the solution becomes very dilute.

    <p>True</p> Signup and view all the answers

    Colligative properties can be used to determine the degree of association or dissociation of a solute.

    <p>True</p> Signup and view all the answers

    Study Notes

    Objectives

    • Students will be able to describe the formation of different types of solutions.
    • Students will be able to express solution concentration in various units.
    • Students will be able to state and explain Henry's Law and Raoult's Law.
    • Students will be able to differentiate between ideal and non-ideal solutions.
    • Students will be able to explain deviations of real solutions from Raoult's Law.
    • Students will be able to describe the colligative properties of solutions.
    • Students will be able to correlate colligative properties with molar masses of solutes.

    Solutions

    • Most processes in liquid solutions.
    • Mixtures of substances.
    • Composition affects utility/importance.
      • Example: Brass (copper+zinc) properties differ from those of German silver (copper+zinc+nickel) or bronze (copper+tin).
      • Fluoride in water prevents tooth decay (1 ppm) or causes discoloration (1.5ppm) and is toxic in higher concentrations.

    Types of Solutions

    • Homogeneous mixtures of 2 or more components.
    • Composition and properties uniform.
    • Component present in highest quantity is solvent.
    • Solvent determines solution's physical state.
      • Component other than solvent is solute.
    • Binary Solutions: only two components.

    Expressing Concentration of Solutions

    • Qualitative description: dilute/concentrated
    • Quantitative methods:
      • Mass percentage (w/w): (Mass of component/Total mass of solution) × 100
      • Volume percentage (V/V): (Volume of component/Total volume of solution) × 100
      • Mass by Volume (%) (w/V): (Mass of solute/100 mL solution) × 100
      • Parts per million (ppm): (Number of parts of component/Total number of parts of all components) × 10⁶
      • Mole fraction (x): (Moles of component/Total moles of all components)

    Solubility of a Solid in a Liquid

    • Not all solids dissolve in all liquids.
    • Polar solutes dissolve in polar solvents (like dissolves like).
    • Solubility varies with temperature and pressure (Le Chatelier's Principle).
      • Endothermic dissolution: solubility increases with temperature.
      • Exothermic dissolution: solubility decreases with temperature.
      • Pressure has little effect on most solutes.

    Solubility of a Gas in a Liquid

    • Solubility increases with pressure (Henry's Law).
    • p = KH x (partial pressure = Henry's Law constant x mole fraction).
    • Solubility decreases with temperature (exothermic).

    Ideal Solutions

    • Solutions that obey Raoult's Law throughout the entire concentration range.
    • Enthalpy of mixing is zero (ΔHmix = 0).
    • Volume of mixing is zero (ΔVmix = 0).

    Non-Ideal Solutions

    • Solutions that do not obey Raoult's Law.
    • Positive deviation: Vapour pressure is higher than expected.
    • Negative deviation: Vapour pressure is lower than expected.

    Colligative Properties

    • Properties that depend on the number of solute particles, not their nature.
    • Relative lowering of vapour pressure, elevation of boiling point, depression of freezing point, osmotic pressure.
    • Elevation of boiling point: change in boiling point = constant × molality.
    • Depression of freezing point: change in freezing point = constant × molality.

    Osmosis and Osmotic Pressure

    • Osmosis: flow of solvent from low to high solute concentration through a semipermeable membrane
    • Osmotic pressure: pressure needed to stop osmosis; directly proportional to molarity of the solution.
    • II = CRT (Osmotic pressure = molarity × gas constant × Temperature).

    Abnormal Molar Masses

    • Some solutes can associate or dissociate in solution
    • Van't Hoff factor (i): accounts for the extent of association or dissociation
    • Abnormal molar masses: calculated molar masses differ from true values due to association or dissociation.

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    Solutions PDF Chemistry Past Paper

    Description

    This quiz covers the formation and concentration of various types of liquid solutions. It will assess your understanding of key concepts such as Henry's Law, Raoult's Law, and colligative properties. Prepare to differentiate between ideal and non-ideal solutions and explore their impacts on substance properties.

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