Chemistry Chapter on Solubility and Distribution
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Questions and Answers

What is defined as the concentration of solute in a saturated solution at a certain temperature?

  • Dispersion
  • Solubility (correct)
  • Saturation limit
  • Dissolution rate

    • Which component in a solution is typically present in the largest proportion?

  • Colloid
  • Solvent (correct)
  • Solute
  • Suspension

    • What term describes the amount of solute that dissolves per unit of time?

  • Solubility
  • Dissolution rate (correct)
  • Equilibrium concentration
  • Saturation concentration

    • Which factor does NOT influence the solubility of a compound?

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

    What type of solution contains more dissolved solute than is normally expected at a specific temperature?

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

    In what kind of mixture is gas dispersed in liquid?

    <p>Gas-liquid mixture</p> Signup and view all the answers

    Which type of solution is in equilibrium with excess undissolved solid of the solute?

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

    Which of the following is NOT a type of solution classification?

    <p>Solid in solid</p> Signup and view all the answers

    Which method can convert a supersaturated solution to a stable saturated solution?

    <p>Seeding the solution with a crystal of solute</p> Signup and view all the answers

    What is the term for a solubility range where less than 1 part of solvent is required for one part of solute?

    <p>Very soluble</p> Signup and view all the answers

    Which solvent would most likely dissolve ionic solutes effectively?

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

    What is the significance of the dielectric constant in solvents?

    <p>It measures the ability of a solvent to separate oppositely charged bodies</p> Signup and view all the answers

    Why is the statement 'like dissolves like' relevant in solubility?

    <p>It indicates that similar polarities in solute and solvent ensure solubility</p> Signup and view all the answers

    Which of the following terms describes a substance that requires more than 10,000 parts of solvent for one part of solute?

    <p>Practically insoluble</p> Signup and view all the answers

    What primarily affects the solubility of polar substances in water?

    <p>The ability to form hydrogen bonds with the solvent</p> Signup and view all the answers

    What would be the best description of a solvent with a dielectric constant of greater than 50?

    <p>Polar solvent</p> Signup and view all the answers

    What is Henry's Law primarily concerned with?

    <p>The relationship between pressure and gas solubility</p> Signup and view all the answers

    What primarily affects the solubility of alcohols in water?

    <p>The presence of non-polar groups</p> Signup and view all the answers

    How does an increase in temperature generally affect the solubility of most gases?

    <p>Decreases solubility due to gas expansion</p> Signup and view all the answers

    Which factor contributes most to the higher water solubility of glycerin compared to long-chain alcohols?

    <p>The presence of additional polar groups</p> Signup and view all the answers

    What does the term 'salting out' refer to?

    <p>The liberation of gases from solutions by adding electrolytes</p> Signup and view all the answers

    How does the dielectric constant of water influence ionic solubility?

    <p>It decreases the attraction between ions</p> Signup and view all the answers

    Which gas is known to show significant increase in solubility in water due to a chemical reaction?

    <p>Hydrogen chloride</p> Signup and view all the answers

    What happens to hydrogen bonds when ethyl alcohol is mixed with water?

    <p>They are partly replaced by new bonds with alcohol</p> Signup and view all the answers

    In what scenario would gas solubility likely decrease?

    <p>With an increase in temperature</p> Signup and view all the answers

    Which of the following statements is true regarding non-polar solvents?

    <p>They cannot effectively dissolve ionic salts</p> Signup and view all the answers

    What is the term used for the proportionality constant in the equation of Henry's Law?

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

    Which of the following solutions is likely to require the use of a propellant gas?

    <p>Aerosol products</p> Signup and view all the answers

    What is the primary role of polar solvents like water in the context of solubility?

    <p>They facilitate ionization and hydrogen bonding</p> Signup and view all the answers

    The attraction of salt ions for water molecules leads to which phenomenon regarding gas solubility?

    <p>Liberation of gases from solution</p> Signup and view all the answers

    Why do straight-chain monohydroxy alcohols with longer carbon chains have limited solubility in water?

    <p>They are unable to participate in hydrogen bonding with water</p> Signup and view all the answers

    What distinguishes tertiary butyl alcohol's solubility in water from that of n-butyl alcohol?

    <p>Its branched structure reduces non-polar effects</p> Signup and view all the answers

    What effect do non polar solvents have on polar solutes?

    <p>They cannot dissolve polar solutes effectively.</p> Signup and view all the answers

    Which of the following solvents can dissolve non polar solutes due to induced dipole interactions?

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

    How do semipolar solvents affect the miscibility of polar and non polar liquids?

    <p>They act as intermediates to facilitate miscibility.</p> Signup and view all the answers

    What must be taken into account when determining the solubility of a substance?

    <p>Purity of the substance and solvent.</p> Signup and view all the answers

    Which of the following best describes the process for determining solubility?

    <p>Agitating the solute and solvent mix continuously at constant temperature.</p> Signup and view all the answers

    What role does propylene glycol serve in a mixture with water and peppermint oil?

    <p>It enhances the mutual solubility.</p> Signup and view all the answers

    What is one of the best methods for determining the purity of a substance?

    <p>Accurate determination of solubility.</p> Signup and view all the answers

    What type of forces keep solute molecules in solution in non polar solvents?

    <p>Van der Waals-London forces</p> Signup and view all the answers

    Study Notes

    Solubility and Distribution

    • A solution is a mixture of two or more components forming a single phase that is homogeneous at the molecular level.
    • The solvent is the component determining the solution's phase, usually the largest proportion. Other components are solutes, dispersed throughout the solvent as molecules or ions.
    • Solubility is defined quantitatively as the concentration of solute in a saturated solution at a certain temperature. It can also be defined qualitatively as the spontaneous interaction of substances to form a homogeneous dispersion.
    • Factors affecting solubility include:
      • Physical and chemical properties of the solute and solvent
      • Temperature
      • Pressure
      • State of subdivision of the solute
    • Types of mixtures include: gases in liquids, liquids in liquids, and solids in liquids.
    • Types of solutions include saturated (equilibrium with excess undissolved solute), unsaturated (less solute than necessary for saturation at a given temperature), and supersaturated (more solute than normally soluble at a given temperature).

    Solubility Expressions (Quantitative)

    • USP expression: milliliters of solvent needed to dissolve 1 gram of solute.
    • Molarity: number of moles of solute per liter of solution.
    • Molality: number of moles of solute per kilogram of solvent.
    • Mole fraction: mole fraction of A = (moles of A) / (total number of moles)
    • Percent by weight (w/w): grams of solute per 100 grams of solution.
    • Percent weight/volume (w/v): grams of solute per 100 mL of solution.
    • Percent by volume (v/v): milliliters of solute per 100 mL of solution.

    Qualitative Terms of Solubility

    • Table (1): Terms of Approximate Solubility (A table is not presented, but terms for solubility are given)
      • Very soluble
      • Freely soluble
      • Soluble
      • Sparingly soluble
      • Slightly soluble
      • Very slightly soluble
      • Practically insoluble

    Solvent-Solute Interactions

    • "Like dissolves like": A general guideline stating that polar solvents dissolve polar solutes, and nonpolar solvents dissolve nonpolar solutes.
    • Water is a good solvent for salts, sugars, and similar polar compounds. Mineral oil and benzene are good solvents for nonpolar substances.
    • Solubility is influenced by the polarity of the solvent (dipole moment), solvation, ionization, and hydration.
    • Hildebrand's work showed that dipole moments are insufficient to fully explain solubility, emphasizing the importance of hydrogen bonding interactions.

    Dielectric Constant

    • A measure of a solvent's ability to separate oppositely charged bodies.

    Polar Solvents

    • Water (DEC > 50) can dissolve ionic solutes due to its ability to oppose electrostatic attractions between positive and negative ions via the dielectric constant mechanism. Water also dissolves polar compounds via hydrogen bond formation.

    Nonpolar Solvents

    • Nonpolar solvents cannot reduce attractions between ions, meaning they have low dielectric constants.
    • They don't break covalent bonds to create ionic compounds and cannot form hydrogen bonds to dissolve ionic or polar solutes.
    • Nonpolar solvents dissolve other nonpolar compounds through induced dipole interactions and Van der Waals forces (London Dispersion forces).

    Semipolar Solvents

    • Act as intermediate solvents for mixing polar and nonpolar liquids; examples include ketones and alcohols.
    • Induce polarity in nonpolar solvents.

    Solubility of Gases in Liquids

    • Solubility of a gas in a liquid depends on the concentration of the dissolved gas, in equilibrium with the pure gas above the solution.

    Effect of Pressure on Gas Solubility (Henry's Law)

    • The concentration of a dissolved gas is directly proportional to its partial pressure above the solution at a constant temperature.

    Effect of Temperature on Gas Solubility

    • As temperature increases, the solubility of most gases decreases.

    Salting Out

    • Gases can be removed from solution by the introduction of an electrolyte (e.g., sodium chloride) or non-electrolyte (e.g., sucrose), due to attraction between the solute ions/molecules and water molecules.

    Effect of Chemical Reaction on Gas Solubility

    • Some gases (e.g., hydrogen chloride, ammonia, carbon dioxide) undergo chemical reactions with the solvent leading to increased solubility.

    Solubility of Liquids in Liquids

    • Frequently, two or more liquids are mixed together in the production of pharmaceutical solutions.
    • The mixing of liquids can lead to ideal or real solutions. Ideal solutions follow Raoult's Law (partial pressure of a component is equal to the vapor pressure of the pure component multiplied by its mole fraction in the solution), however, real solutions may exhibit deviations from Raoult's Law (positive or negative deviations).
    • The interaction of the solvent with the solute is known as solvation.
    • Cohesion forces between molecules of one constituent influence whether the mixture is ideal or shows deviations. Polar liquids tend to dissolve similar-nature compounds.
    • Complete miscibility means that two liquids can mix in any proportion.
    • Partial miscibility means two liquids mix only to certain maximum extent. They form distinct liquid layers that each contain some of the other liquid at their interface

    Influence of Foreign Substances on Solubility of Liquids

    • The addition of a third substance to a binary liquid mixture can either increase or decrease the solubility of each liquid in the other depending on the relative solubility of the third substance in each of the liquids of the original binary system. Also, the introduction of a third substance may change the liquid's critical solution temperature.
    • Factors like the mutual solubility and solubility coefficient must be considered when deciding whether the addition of a third substance will increase or decrease solubility of the liquid pair.

    Solubility of Solids in Liquids

    • The majority of pharmaceutical solutions involve solids dissolved in liquids and these solutions may be ideal or real.
    • Ideal solutions follow Raoult's law, while real solutions may not. The solubility of a solid in an ideal solution depends on the temperature, melting point of the solid, and molar heat of fusion.

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    Solubility and Distribution PDF

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    Explore the fascinating concepts of solubility and distribution in this chemistry quiz. Learn about solutions, the roles of solutes and solvents, and the factors affecting solubility. Test your understanding of different types of mixtures and their properties.

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