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Questions and Answers
What are solutions?
Why are solutions important?
What 'drives' the dissolution process when a solid dissolves into a liquid?
What term defines the extent of ionization of a weak acid or base at different pH values?
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What do many drugs (APIs) behave as when dissolved in water?
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What do 50-65% of our body mass consist of?
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What is the process called when solvents are attracted to surface ions, forming a solvation shell around each ion?
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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?
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What theory defines acids as substances that can donate a proton and bases as substances that can accept a proton?
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What equation is used to calculate pH values based on the concentration of the base and its conjugate acid?
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What occurs when the addition of an ion to a solution lowers the concentration of the other ion to maintain the solubility constant?
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What does the enthalpy change of solution (DHsoln) represent?
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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?
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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?
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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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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.
