Chemistry Chapter on Solutions and Mixtures
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Questions and Answers

Which of the following is NOT a general property of mixtures?

  • Components can be easily separated.
  • Each component retains its original properties.
  • Mixtures can be converted into component substances by physical processes.
  • The proportion of components is fixed. (correct)

    • Which of the following is true about the conversion between substances (compounds and elements)?

  • They are always converted through physical processes.
  • They are always converted through physical processes.
  • They are only converted through physical processes.
  • They are only converted through chemical processes. (correct)

    • A patient suffering from dehydration due to excessive diarrhea would likely benefit from which type of IV solution?

  • Isotonic (correct)
  • Hypotonic
  • Hypertonic
  • None of the above

    • Which of the following is a key factor that influences the rate of dissolution?

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

    A supersaturated solution is best described as a solution that:

    <p>Contains more solute than the maximum that can dissolve at a given temperature. (B)</p> Signup and view all the answers

    Which of the following is a unit commonly used to express the concentration of a solution?

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

    What is the main factor that governs the solubility of a gas in a liquid?

    <p>Pressure (B)</p> Signup and view all the answers

    In general, as the temperature of a solution increases, the solubility of a solid solute:

    <p>Increases (D)</p> Signup and view all the answers

    What is the dispersed phase in a colloid?

    <p>The component present in smaller proportion (C)</p> Signup and view all the answers

    What is the Tyndall effect?

    <p>The scattering of light by particles in a colloid (B)</p> Signup and view all the answers

    Which of the following is an example of a solid-solid solution?

    <p>Brass (D)</p> Signup and view all the answers

    Which of the following is NOT a characteristic of a colloid?

    <p>The particles are easily separated by filtration (B)</p> Signup and view all the answers

    Which of the following is an example of an aerosol?

    <p>Fog (C)</p> Signup and view all the answers

    What is the process by which the dispersed phase of a colloid is made to aggregate and separate from the continuous phase?

    <p>Coagulation (B)</p> Signup and view all the answers

    What is the main reason for the cleansing action of soap?

    <p>The nonpolar tail of soap dissolves in oil (D)</p> Signup and view all the answers

    What is the correct classification of a solution where a gas is dissolved in a liquid?

    <p>Gas-Liquid Solution (A)</p> Signup and view all the answers

    Which of the following is NOT a true solution?

    <p>Milk (A)</p> Signup and view all the answers

    What is the main difference between a colloid and a suspension?

    <p>Colloids cannot be separated by filtration, suspensions can (B)</p> Signup and view all the answers

    Why does the sky appear blue during the day?

    <p>Sunlight is scattered by the particles in the atmosphere (D)</p> Signup and view all the answers

    Which of the following is an example of an association colloid?

    <p>Soap in water (D)</p> Signup and view all the answers

    What is the term used to describe a mixture where the components are not uniformly distributed?

    <p>Heterogeneous mixture (B)</p> Signup and view all the answers

    Which of the following is NOT an example of a colloid?

    <p>Sugar dissolved in water (B)</p> Signup and view all the answers

    What is the dispersion medium in a foam?

    <p>Liquid (B)</p> Signup and view all the answers

    What is the dispersion medium in an emulsion?

    <p>Liquid (B)</p> Signup and view all the answers

    What is the name of the colloidal particle formed when a coronavirus-infected patient coughs or sneezes, dispersing fine droplets of respiratory fluid containing viral particles in the atmosphere?

    <p>Aerosol (D)</p> Signup and view all the answers

    Which of the following is NOT a colloid?

    <p>Honey (B)</p> Signup and view all the answers

    Which statement best describes the 'like dissolves like' rule?

    <p>Substances with similar intermolecular forces dissolve in each other. (A)</p> Signup and view all the answers

    Which of the following is a polar compound?

    <p>H2O (B)</p> Signup and view all the answers

    Which of the following is MOST effective in coagulating colloidal sulphur?

    <p>AlCl3 (C)</p> Signup and view all the answers

    Which of the following is an example of a homogeneous mixture?

    <p>Salt and water (C)</p> Signup and view all the answers

    Which of the following is an example of a suspension?

    <p>Muddy water (A)</p> Signup and view all the answers

    Which of the following is an example of a pure substance?

    <p>Gold (C)</p> Signup and view all the answers

    What is the correct order of steps involved in the solution process?

    <p>Breaking up solute-solute interactions, breaking up solvent-solvent interactions, forming solute-solvent interactions (B)</p> Signup and view all the answers

    Which of the following statements accurately describes the dissolution of an ionic compound in water?

    <p>The ionic compound dissolves because the water molecules attract the ions and break the ionic bonds. (B)</p> Signup and view all the answers

    Which of the following pairs of substances is MOST likely to dissolve in each other?

    <p>Ethanol (C2H5OH) and Water (H2O) (D)</p> Signup and view all the answers

    Which of the following intermolecular forces is strongest?

    <p>Hydrogen bonding (D)</p> Signup and view all the answers

    Which of the following statements is TRUE关于溶液？

    <p>溶液是一种物理变化，而不是化学变化。 (B)</p> Signup and view all the answers

    What is the enthalpy change when one mole of a substance is dissolved in water at constant pressure?

    <p>Molar heat of solution (B)</p> Signup and view all the answers

    What is the sign of the enthalpy change (ΔHsoln) for an exothermic dissolution process?

    <p>Negative (A)</p> Signup and view all the answers

    In which step of the solution process does the enthalpy change represent the energy required to separate solute particles from each other?

    <p>Solute-solute interactions (A)</p> Signup and view all the answers

    Which of the following is an example of an ideal solution?

    <p>A mixture of methanol and ethanol (B)</p> Signup and view all the answers

    What is the term used for the enthalpy change associated with the process of completely surrounding solute particles with solvent molecules?

    <p>Solvation energy (D)</p> Signup and view all the answers

    When water is used as the solvent, what specific term is used to describe the energy change of surrounding solute particles with solvent molecules?

    <p>Hydration energy (A)</p> Signup and view all the answers

    Which of the following factors influences lattice energy?

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

    How does lattice energy affect the solubility of ionic solids in water?

    <p>Higher lattice energy leads to lower solubility. (A)</p> Signup and view all the answers

    Why are instant cold packs often based on ammonium nitrate?

    <p>Ammonium nitrate absorbs heat when dissolved. (D)</p> Signup and view all the answers

    Which of the following salts is most likely to produce heat when dissolved in water?

    <p>Sodium hydroxide (NaOH) (B)</p> Signup and view all the answers

    Which of the following statements best describes the relationship between heat of solution (ΔHsoln) and the strength of interparticle forces?

    <p>Stronger interparticle forces lead to a more positive ΔHsoln. (A)</p> Signup and view all the answers

    Which of the following is true about the 'ideal' solution?

    <p>The solute-solute and solvent-solvent interactions are equal in strength. (D)</p> Signup and view all the answers

    What is the relationship between the magnitude of the lattice energy and the solubility of an ionic solid in water?

    <p>Inversely proportional (C)</p> Signup and view all the answers

    Which of the following ionic compounds would you expect to have the highest lattice energy?

    <p>AlCl3 (A)</p> Signup and view all the answers

    If the dissolving of a substance results in an increase in temperature, which of the following statements is true about the heat of solution?

    <p>It is negative. (C)</p> Signup and view all the answers

    In the equation ΔHsoln = ΔHsolute + ΔHsolvent + ΔHmix, which term represents the energy change associated with the formation of new solute-solvent interactions?

    <p>ΔHmix (C)</p> Signup and view all the answers

    A student adds 4.00 g of NaOH(s) to 100 g of water in a polystyrene foam cup. The temperature of the water rises by 10.0 °C. Assuming the polystyrene foam cup is well insulated and the specific heat capacity of water is 4.18 J/°C·g, what is the enthalpy change for the dissolution of NaOH in kJ/mol?

    <p>-43.5 kJ/mol (A)</p> Signup and view all the answers

    Which of the following pairs of ions has the greatest enthalpy of hydration?

    <p>Mg2+ or Cs+ (B)</p> Signup and view all the answers

    Why is the enthalpy of solution an important factor in determining the formation of solutions?

    <p>The enthalpy of solution determines whether the dissolution process is exothermic or endothermic. (D)</p> Signup and view all the answers

    Which of the following actions would likely lead to a supersaturated solution?

    <p>Cooling a saturated solution slowly. (A)</p> Signup and view all the answers

    What is the purpose of using a calorimeter in the determination of the enthalpy of solution?

    <p>To measure the temperature change of the solution. (A)</p> Signup and view all the answers

    A student is investigating the heat of solution of calcium chloride (CaCl2) and ammonium nitrate (NH4NO3). They accurately weigh 4 g of each salt and dissolve it in 40 mL of water. Which of the following is a reasonable assumption they can make about the heat exchange with the surroundings?

    <p>The heat exchange with the surroundings is negligible. (D)</p> Signup and view all the answers

    Which of the following accurately describes the purpose of Project 2.4 in the chemistry textbook?

    <p>To understand the usage and working principles of instant cold packs and hot packs in a real-world context. (A)</p> Signup and view all the answers

    What is the primary reason why a solution reaches equilibrium when no more solute will dissolve, even with continued stirring?

    <p>The rate of dissolution equals the rate of recrystallization. (D)</p> Signup and view all the answers

    When an ionic solid dissolves in water, what happens to the ions?

    <p>They break apart and become surrounded by water molecules. (C)</p> Signup and view all the answers

    Which of the following scenarios best illustrates the concept of a supersaturated solution?

    <p>Heating a saturated solution of sugar in water and then slowly cooling it down. (A)</p> Signup and view all the answers

    You are asked to prepare a supersaturated solution of sodium thiosulphate (Na2S2O3). Which of the following steps would be most crucial to ensure the successful preparation of a supersaturated solution?

    <p>Cooling the solution slowly and carefully after heating. (B)</p> Signup and view all the answers

    In the context of solutions, what is meant by the term "solution equilibrium"?

    <p>The state where the rate of dissolution equals the rate of recrystallization. (D)</p> Signup and view all the answers

    What is the primary factor that determines the solubility of a solid in a liquid?

    <p>The temperature of the solution. (D)</p> Signup and view all the answers

    A student is preparing a solution of sodium sulphate (Na2SO4). They add a small amount of Na2SO4 to water and observe that it dissolves completely. They continue adding more Na2SO4, and eventually, some solid remains undissolved at the bottom of the container. At this point, the solution is best described as:

    <p>Saturated (D)</p> Signup and view all the answers

    What is the primary difference between a saturated solution and a supersaturated solution?

    <p>A supersaturated solution contains more dissolved solute than a saturated solution at the same temperature. (C)</p> Signup and view all the answers

    What characterizes a saturated solution?

    <p>It contains the maximum amount of dissolved solute at equilibrium. (B)</p> Signup and view all the answers

    Which solution type allows for more solute to be dissolved without any undissolved particles present?

    <p>Unsaturated solution (D)</p> Signup and view all the answers

    What occurs when a seeding crystal is added to a supersaturated solution?

    <p>The excess solute will rapidly crystallize. (B)</p> Signup and view all the answers

    What factor significantly affects the solubility of gases in liquids?

    <p>Pressure (B)</p> Signup and view all the answers

    How does temperature affect the solubility of most solid solutes?

    <p>Solubility increases with higher temperatures. (B)</p> Signup and view all the answers

    In what case would you expect more than the initially added solid to precipitate?

    <p>In a supersaturated solution upon adding solute (D)</p> Signup and view all the answers

    What is typically required to create a supersaturated solution?

    <p>A heating process followed by cooling (B)</p> Signup and view all the answers

    Which of the following is a characteristic of an unsaturated solution?

    <p>Can dissolve additional solute (B)</p> Signup and view all the answers

    Which process occurs when forming sodium sulfate from its solute at higher temperatures?

    <p>Increased solubility (D)</p> Signup and view all the answers

    What is the term for the solution that stays dissolved despite having exceeded normal saturation?

    <p>Supersaturated solution (A)</p> Signup and view all the answers

    What will happen if a few crystals of salt are added to an unsaturated solution?

    <p>They will dissolve and not affect the solution. (C)</p> Signup and view all the answers

    When does the solubility of a gas generally decrease?

    <p>When temperature increases (D)</p> Signup and view all the answers

    How is solubility generally measured?

    <p>In grams of solute per 100 g of solvent (C)</p> Signup and view all the answers

    What happens to the solubility of a gas when external heat is added to the system?

    <p>The solubility of the gas decreases. (B)</p> Signup and view all the answers

    According to Henry's Law, what effect does increasing the partial pressure of a gas above a liquid have?

    <p>It increases the concentration of the gas in the liquid. (A)</p> Signup and view all the answers

    Which equation represents the relationship between solubility and partial pressure of a gas as stated by Henry's Law?

    <p>C = k * P (D)</p> Signup and view all the answers

    What is the expected effect on gas solubility if the temperature of the solution is increased while keeping pressure constant?

    <p>Gas solubility will decrease. (C)</p> Signup and view all the answers

    Which of the following gases would not typically obey Henry's Law due to its strong interaction with water?

    <p>HCl (A)</p> Signup and view all the answers

    If the concentration of CO2 in a solution is measured to be 0.1 M at a pressure of 4 atm, what is the molarity of CO2 when the pressure is decreased to 2 atm?

    <p>0.05 M (C)</p> Signup and view all the answers

    Which of the following factors does NOT affect the solubility of a gas in a liquid?

    <p>Presence of light (A)</p> Signup and view all the answers

    How is concentration often expressed in relation to a solute in a solution?

    <p>Molarity (B)</p> Signup and view all the answers

    What is the effect of pollution on aquatic life as nations shift from agriculture-led to industry-led economies?

    <p>It decreases biodiversity and productivity. (B)</p> Signup and view all the answers

    In the example given for the solubility of nitrogen gas, what is the concentration under atmospheric conditions?

    <p>5.3 x 10-4 mol/L (C)</p> Signup and view all the answers

    What additional precaution should be taken when disposing of personal hygiene materials to protect aquatic life?

    <p>Avoid disposing of them in water bodies. (D)</p> Signup and view all the answers

    What is indicated by the Henry’s law constant for a gas?

    <p>The concentration of dissolved gas at equilibrium. (C)</p> Signup and view all the answers

    What happens to the solubility of a gas when the partial pressure is reduced?

    <p>Solubility decreases. (A)</p> Signup and view all the answers

    Which intermolecular force is responsible for the solubility of HBr in water?

    <p>Dipole-dipole forces (C)</p> Signup and view all the answers

    Which intermolecular force is primarily responsible for the dissolution of NaCl in water?

    <p>Ion-dipole forces (A)</p> Signup and view all the answers

    Which intermolecular force is responsible for the solubility of atmospheric O2 in water?

    <p>Dipole-induced dipole forces (C)</p> Signup and view all the answers

    Which of the following intermolecular forces is considered the weakest?

    <p>Dispersion forces (B)</p> Signup and view all the answers

    Which of the following compounds is MOST likely to be soluble in water?

    <p>KCl (C)</p> Signup and view all the answers

    Which of the following is NOT a characteristic of hydrogen bonding?

    <p>It is a relatively weak intermolecular force. (B)</p> Signup and view all the answers

    Which of the following best describes the solubility of ionic compounds in water?

    <p>Most ionic compounds are soluble in water, but there are some exceptions. (A)</p> Signup and view all the answers

    Which of the following intermolecular forces is NOT considered a van der Waals force?

    <p>Ion-dipole forces (A)</p> Signup and view all the answers

    Which of the following statements about the relative strengths of intermolecular forces is TRUE?

    <p>Ion-dipole forces are weaker than hydrogen bonding. (A)</p> Signup and view all the answers

    Which of the following pairs of molecules is MOST likely to exhibit hydrogen bonding between them?

    <p>NH3 and H2O (D)</p> Signup and view all the answers

    Which type of intermolecular force is responsible for the attraction between the Fe2+ ion in hemoglobin and an O2 molecule?

    <p>Dipole-induced dipole forces (B)</p> Signup and view all the answers

    Which of the following statements accurately describes the solubility rules for ionic compounds?

    <p>Most hydroxide salts are soluble. (D)</p> Signup and view all the answers

    Which of the following is an example of a compound that is slightly soluble in water?

    <p>Ca(OH)2 (D)</p> Signup and view all the answers

    Which of the following intermolecular forces is primarily responsible for the dissolution of polar molecular solids in water?

    <p>Hydrogen bonding (B)</p> Signup and view all the answers

    Which of the following pairs of liquids would be considered miscible?

    <p>Water and grain alcohol (B)</p> Signup and view all the answers

    Which of the following compounds is classified as insoluble in water?

    <p>BaCO3 (A)</p> Signup and view all the answers

    Which of the following factors does NOT affect the rate of dissolution of a solid solute in a solvent?

    <p>Pressure of the solvent (C)</p> Signup and view all the answers

    Which of the following statements correctly describes the energy changes involved in the dissolution process?

    <p>Dissolution can be either exothermic or endothermic, depending on the relative strengths of the intermolecular forces involved. (B)</p> Signup and view all the answers

    Which of the following is the best explanation for why a flask containing ammonium chloride (NH4Cl) in water gets cold when the solution is formed?

    <p>The dissolution of NH4Cl is an endothermic process. (A)</p> Signup and view all the answers

    Why does increasing the surface area of a solid solute generally increase the rate of dissolution?

    <p>It increases the number of collisions between solute particles and solvent molecules. (D)</p> Signup and view all the answers

    Which of the following is TRUE about the solvation energy?

    <p>It represents the energy released when solute molecules are surrounded by solvent molecules. (D)</p> Signup and view all the answers

    Which of the following pairs exhibits the strongest intermolecular forces?

    <p>I2 and NO3- (C)</p> Signup and view all the answers

    Which of the following is the best explanation for why H2O is a liquid at room temperature while H2S is a gas?

    <p>H2O has stronger hydrogen bonds than H2S. (B)</p> Signup and view all the answers

    What is the main reason why quicklime (CaO) and slaked lime (Ca(OH)2) are used to remove excess fluoride from drinking water?

    <p>They react with fluoride ions to form insoluble precipitates. (B)</p> Signup and view all the answers

    Which of the following statements accurately describes the process of dissolution?

    <p>Dissolution is the process where a solute disperses uniformly throughout a solvent. (C)</p> Signup and view all the answers

    Which of the following is a correct example of a polar molecular solid?

    <p>Glucose (C6H12O6) (D)</p> Signup and view all the answers

    If a solution process is endothermic, what can be said about the relative amounts of energy involved in breaking solute-solute and solvent-solvent interactions versus forming solute-solvent interactions?

    <p>Less energy is released in forming solute-solvent interactions than is required to break solute-solute and solvent-solvent interactions. (A)</p> Signup and view all the answers

    Which of the following is NOT a factor that can affect the rate of dissolution of a solid solute?

    <p>The pressure of the system (D)</p> Signup and view all the answers

    Which of the following best describes the term "hydration" in the context of solution chemistry?

    <p>The process of surrounding solute molecules with water molecules. (C)</p> Signup and view all the answers

    What is the primary difference between a miscible and an immiscible pair of liquids?

    <p>Miscible liquids can mix in any proportion, while immiscible liquids cannot. (A)</p> Signup and view all the answers

    Study Notes

    Unit Outcomes

    • Solutions are homogeneous mixtures of a solute dissolved in a solvent.
    • Solution formation involves breaking solute-solute and solvent-solvent interactions and forming solute-solvent interactions.
    • Solubility depends on temperature and pressure.
    • Concentration is the relative quantity of solute compared to the total solution or solvent.

    Types of Mixtures

    • Mixtures combine two or more substances, maintaining their individual properties.
    • Homogeneous mixtures have uniform composition throughout (e.g., solutions).
    • Heterogeneous mixtures have physically distinct parts with non-uniform composition (e.g., suspensions).

    Solutions, Suspensions, and Colloids

    • Solutions are homogeneous, with solute particles in a size of individual atoms, molecules, or ions.
    • Suspensions are heterogeneous, with solid particles dispersed in a liquid without dissolving.
    • Colloids are heterogeneous with particle sizes between 1 nm and 100 nm, appearing homogenous but visibly scattering light (Tyndall effect).

    Types of Solutions

    • Gaseous solutions (gas-gas): The atmosphere is a major example
    • Liquid solutions (liquid-solid, liquid-liquid, or gas-liquid): Carbonated drinks, alcoholic beverages, and seawater.
    • Solid solutions (solid-solid): Alloys, dental filling

    Solubility Rules for Ionic Solids

    • Group 1A salts and ammonium salts are soluble.
    • Salts containing acetate, nitrate, perchlorate are usually soluble.
    • Chlorides, bromides, and iodides are generally soluble, except those containing silver, lead, copper, or mercury.
    • Most hydroxides are slightly soluble; Group 1 hydroxides are soluble.
    • Most sulfates are soluble except those with barium, strontium, lead, calcium, silver, or mercury.
    • Except for Group 1A and ammonium salts, carbonates, sulfides, oxides, and phosphates are generally insoluble in water.

    Solution Process

    • Dissolution is a physical process, not a chemical change.
    • "Like dissolves like": Substances with similar intermolecular forces dissolve in each other.
      • Polar substances dissolve in polar solvents.
      • Nonpolar substances dissolve in nonpolar solvents.

    Intermolecular Forces

    • Intermolecular forces influence solubility.
    • Types of intermolecular forces (weakest to strongest):
      • Dispersion forces
      • Dipole-induced dipole forces
      • Dipole-dipole forces
      • Hydrogen bonds
      • Ion-dipole forces

    Solubility as Equilibrium

    • A saturated solution contains the maximum amount of dissolved solute at a given temperature.
    • Unsaturated solutions have dissolved solute below the maximum.
    • Supersaturated solutions contain more solute than possible at a given temperature.

    Factors Affecting Solubility

    • Temperature (solids): Generally, increased temperature increases solubility.
    • Temperature (gases): Generally, increased temperature decreases solubility.
    • Pressure (gases): Increased pressure increases solubility (Henry's Law).

    Concentration Units

    • Concentration describes the relative amount of solute in a solution.
    • Ways to express solution concentration include mass percentage (%), parts per million (ppm), and parts per billion (ppb).

    Heat of Solution

    • Heat of solution is the amount of heat absorbed or released when a solute dissolves.
    • Endothermic dissolution absorbs heat; exothermic dissolution releases heat.
    • Molar heat of solution is the heat absorbed or released when one mole of solute dissolves.

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    Description

    Test your understanding of solutions, mixtures, and their properties with this quiz. You'll explore concepts like solubility, concentration, and the Tyndall effect, among others. Challenge yourself to recall key factors that affect dissolution rates and the characteristics of colloids.

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