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Questions and Answers
What phenomenon is described when a solute is more soluble in a mixture of solvents than in one solvent alone?
What phenomenon is described when a solute is more soluble in a mixture of solvents than in one solvent alone?
- Deliquescence
- Hygroscopy
- Efflorescence
- Cosolvency (correct)
How does the addition of alcohol to a buffered aqueous solution of a weak electrolyte affect the solubility of the un-ionized species?
How does the addition of alcohol to a buffered aqueous solution of a weak electrolyte affect the solubility of the un-ionized species?
- Has no effect on its solubility
- Forms a precipitate
- Decreases its solubility by increasing dissociation
- Increases its solubility by adjusting solvent polarity (correct)
How does alcohol, when added to water, impact the dissociation of a weak electrolyte in a buffered solution?
How does alcohol, when added to water, impact the dissociation of a weak electrolyte in a buffered solution?
- Has no effect on dissociation or solubility
- Increases dissociation and raises solubility
- Decreases dissociation and lowers solubility (correct)
- Forms a chemical bond with the solute
What happens to the solubility of a weak base as the pH of the solution is increased?
What happens to the solubility of a weak base as the pH of the solution is increased?
How does the Henderson-Hasselbach equation relate pH and pKa to acid and its salt concentrations?
How does the Henderson-Hasselbach equation relate pH and pKa to acid and its salt concentrations?
How is the pHp defined in relation to the solubility of acids and bases?
How is the pHp defined in relation to the solubility of acids and bases?
What is the pH below which free phenobarbital will begin to separate from a solution?
What is the pH below which free phenobarbital will begin to separate from a solution?
In the context of drug solubility, what does a pH of 9.03 indicate?
In the context of drug solubility, what does a pH of 9.03 indicate?
How does a weak electrolyte behave in a solution where the pH makes the drug entirely ionic?
How does a weak electrolyte behave in a solution where the pH makes the drug entirely ionic?
What is the significance of pKa in determining the solubility behavior of weak acids or bases?
What is the significance of pKa in determining the solubility behavior of weak acids or bases?
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