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Questions and Answers
What is the quantitative definition of solubility?
What is the quantitative definition of solubility?
- The dissolved solute in a concentration below that necessary for complete saturation at a definite temperature
- The concentration of solute in a saturated solution at a certain temperature (correct)
- The solute in solution being in equilibrium with the solid phase
- The spontaneous interaction of two or more substances to form a homogeneous molecular dispersion
What type of solution is one containing the dissolved solute in a concentration below that necessary for complete saturation at a definite temperature?
What type of solution is one containing the dissolved solute in a concentration below that necessary for complete saturation at a definite temperature?
- Subsaturated solution
- Unsaturated solution (correct)
- Supersaturated solution
- Saturated solution
What happens if a mixture, initially containing 100 grams of dissolved glucose at 25 °C, is slowly cooled back to 25 °C?
What happens if a mixture, initially containing 100 grams of dissolved glucose at 25 °C, is slowly cooled back to 25 °C?
- Glucose precipitates after a long time (correct)
- Glucose remains dissolved indefinitely
- Glucose never precipitates
- Glucose precipitates immediately
What effect does the addition of electrolytes and non-electrolytes have on gaseous solutions?
What effect does the addition of electrolytes and non-electrolytes have on gaseous solutions?
In which type of solution do the components obey Raoult's law and have adhesive forces equal to cohesive forces?
In which type of solution do the components obey Raoult's law and have adhesive forces equal to cohesive forces?
What is the characteristic of a negative deviated solution?
What is the characteristic of a negative deviated solution?
Under what conditions do liquid-liquid systems show complete miscibility?
Under what conditions do liquid-liquid systems show complete miscibility?
Why is water able to dissolve NaCl but chloroform and benzene cannot?
Why is water able to dissolve NaCl but chloroform and benzene cannot?
Why are non polar solvents like benzene unable to dissolve ionic compounds?
Why are non polar solvents like benzene unable to dissolve ionic compounds?
Why is water capable of dissolving phenols, alcohols, and other oxygen & nitrogen containing compounds?
Why is water capable of dissolving phenols, alcohols, and other oxygen & nitrogen containing compounds?
Study Notes
Solubility
- Quantitative definition of solubility: Not explicitly stated, but implied to be the maximum amount of solute that can dissolve in a solvent at a given temperature.
Types of Solutions
- Solution containing dissolved solute in a concentration below that necessary for complete saturation at a definite temperature: Undersaturated solution.
Solution Behavior
- If a mixture, initially containing 100 grams of dissolved glucose at 25 °C, is slowly cooled back to 25 °C: Precipitation of glucose occurs, as the solubility of glucose decreases with decreasing temperature.
Effects of Electrolytes and Non-Electrolytes
- Addition of electrolytes and non-electrolytes to gaseous solutions: Increases the solubility of gases, particularly in aqueous solutions.
Ideal Solutions
- Components obey Raoult's law and have adhesive forces equal to cohesive forces: Ideal solutions, where the interactions between solute and solvent molecules are identical to those between solvent molecules.
Negative Deviation
- Characteristic of a negative deviated solution: Lower vapor pressure than expected, indicating stronger intermolecular forces between solute and solvent molecules.
Liquid-Liquid Miscibility
- Conditions for complete miscibility in liquid-liquid systems: Similar intermolecular forces between the two liquids.
Solvent Properties
- Water's ability to dissolve NaCl, but not chloroform and benzene: Polarity and high dielectric constant of water, allowing it to dissociate and solvate ionic compounds.
- Non-polar solvents like benzene unable to dissolve ionic compounds: Lack of polarity and low dielectric constant, making them unable to dissociate and solvate ionic compounds.
- Water's ability to dissolve phenols, alcohols, and other oxygen & nitrogen containing compounds: Hydrogen bonding between water molecules and the functional groups of these compounds.
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Description
Test your knowledge of solubility and distribution phenomena in physical pharmacy with this quiz. Explore concepts such as saturated solutions, spontaneous interactions, and molecular dispersion.
