W2-Solutions I
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Questions and Answers

What are solutions?

  • Mixtures of a solute and a solvent
  • Pure substances with no mixture
  • Homogeneous mixtures of two or more pure substances (correct)
  • Heterogeneous mixtures of two or more pure substances

    • Why are solutions important?

  • To separate pure substances
  • To prevent the absorption of drugs
  • In order to be absorbed and exert an action, a drug must be in solution (correct)
  • To create heterogeneous mixtures

    • What 'drives' the dissolution process when a solid dissolves into a liquid?

  • Decrease in temperature
  • Increase in temperature (correct)
  • Increase in pressure
  • Decrease in pressure

    • What term defines the extent of ionization of a weak acid or base at different pH values?

    <p>$Ka$</p> Signup and view all the answers

    What do many drugs (APIs) behave as when dissolved in water?

    <p>Partially ionized molecules</p> Signup and view all the answers

    What do 50-65% of our body mass consist of?

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

    What is the process called when solvents are attracted to surface ions, forming a solvation shell around each ion?

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

    What is the term for the maximum amount of a solid that can dissolve in a liquid at a given temperature in dynamic equilibrium with undissolved solid?

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

    What theory defines acids as substances that can donate a proton and bases as substances that can accept a proton?

    <p>Lowery-Brønsted theory</p> Signup and view all the answers

    What equation is used to calculate pH values based on the concentration of the base and its conjugate acid?

    <p>$pH = pKa + ext{log} [A^-]:[HA]$</p> Signup and view all the answers

    What occurs when the addition of an ion to a solution lowers the concentration of the other ion to maintain the solubility constant?

    <p>Common ion effect</p> Signup and view all the answers

    What does the enthalpy change of solution (DHsoln) represent?

    <p>The sum of enthalpies of three processes involving the separation of solute and solvent particles, formation of new interactions, and enthalpy changes.</p> Signup and view all the answers

    What is the term for the equilibrium term describing the maximum amount of a gas that can dissolve in a liquid at a given temperature?

    <p>Gaseous solubility</p> Signup and view all the answers

    What is formed when a weak acid or base and its salt are combined to resist changes in pH upon addition of acid or base?

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

    Study Notes

    • Solvents are attracted to surface ions, forming a solvation shell around each ion.
    • Each ion is surrounded by solvent molecules, a process called solvation or hydration when the solvent is water.
    • Ionic solids dissolve in water through a process involving the separation of solute and solvent particles, formation of new interactions, and enthalpy changes.
    • The enthalpy change of solution (DHsoln) can be calculated as the sum of the enthalpies of the three processes.
    • The enthalpy of solution can be either positive or negative, depending on the energy required to separate the particles and form new interactions.
    • Solubility is an equilibrium term describing the maximum amount of a solid that can dissolve in a liquid at a given temperature in dynamic equilibrium with undissolved solid.
    • The solubility of solid solutes in liquid solvents generally increases with temperature, while the solubility of gases decreases.
    • The common ion effect occurs when the addition of an ion to a solution lowers the concentration of the other ion to maintain the solubility constant.
    • Water dissociates into ions in a process called autoprotolysis, with the concentration of hydronium and hydroxide ions influencing the pH of the solution.
    • The Lowery-Brønsted theory defines acids as substances that can donate a proton and bases as substances that can accept a proton.
    • The pH of a solution is related to the concentration of hydrogen ions through the logarithmic scale of pH.
    • Buffer solutions, made from a weak acid or base and its salt, can resist changes in pH upon the addition of acid or base.
    • Aspirin has a pKa of 3.5 and a pH of 7.4 in the human body, with a large ratio of [A-]:[HA] indicating a solution that is predominantly the base form of aspirin.
    • pH values can be calculated using the equation pH = pKa + log [A-]:[HA].
    • References and further reading suggested include "Aulton's Pharmaceutics" and "Physicochemical Principles of Pharmacy."

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    Pharmaceutics Solutions Week 2 PDF

    Description

    Test your knowledge on aqueous solutions, solubility, solubility constants, common ion effect, pKw, Ka, Kb, pH, pOH, Henderson-Hasselbalch equation, weak acids and bases, and buffers.

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