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What type of solution is one that contains the dissolved solute in a concentration below that necessary for complete saturation at a definite temperature?
What type of solution is one that contains the dissolved solute in a concentration below that necessary for complete saturation at a definite temperature?
- Saturated solution
- Homogeneous molecular dispersion
- Supersaturated solution
- Unsaturated or subsaturated solution (correct)
What is solubility defined as in quantitative terms?
What is solubility defined as in quantitative terms?
- The interaction of solute and solvent to form a heterogeneous mixture
- The interaction of two or more substances to form a homogeneous molecular dispersion
- The concentration of solute in a saturated solution at a certain temperature (correct)
- The concentration of solute in an unsaturated solution
What happens when a supersaturated solution contains more of the dissolved solute than it would normally contain at a definite temperature?
What happens when a supersaturated solution contains more of the dissolved solute than it would normally contain at a definite temperature?
- The solute crystallizes out of the solution (correct)
- The solute fully precipitates from the solution
- The solute remains in solution without any change
- The solute forms a heterogeneous mixture with the solvent
What happens to the system between the cooling of the solution and the formation of glucose crystals when there is a higher amount of dissolved glucose than predicted by the solubility limit at 25 °C?
What happens to the system between the cooling of the solution and the formation of glucose crystals when there is a higher amount of dissolved glucose than predicted by the solubility limit at 25 °C?
What term is used to describe a solution that contains more dissolved solute than is predicted by the solubility limit?
What term is used to describe a solution that contains more dissolved solute than is predicted by the solubility limit?
What factor can affect the solubility of a substance?
What factor can affect the solubility of a substance?
What is the significance of the dielectric constant (Ԑ) of a solvent?
What is the significance of the dielectric constant (Ԑ) of a solvent?
Based on the principle of 'like dissolves like', in which type of solvent would a polar solute dissolve best?
Based on the principle of 'like dissolves like', in which type of solvent would a polar solute dissolve best?
What type of solvents dissolve ionic solutes and other polar substances?
What type of solvents dissolve ionic solutes and other polar substances?
What does a series of solvents of increasing polarity show?
What does a series of solvents of increasing polarity show?
What effect does a high dielectric constant in polar solvents have on the force of attraction between oppositely charged ions in crystals?
What effect does a high dielectric constant in polar solvents have on the force of attraction between oppositely charged ions in crystals?
In which type of solvent would ionic compounds be practically insoluble?
In which type of solvent would ionic compounds be practically insoluble?
What type of interaction allows polar solvents to solvate molecules and ions?
What type of interaction allows polar solvents to solvate molecules and ions?
Which type of compounds can water dissolve due to hydrogen bond formation?
Which type of compounds can water dissolve due to hydrogen bond formation?
How do polar solvents break the covalent bonds of strong electrolytes?
How do polar solvents break the covalent bonds of strong electrolytes?
Why are non polar solvents unable to reduce the attraction between ions?
Why are non polar solvents unable to reduce the attraction between ions?
In what way can semipolar solvents bring about miscibility of polar and non polar liquids?
In what way can semipolar solvents bring about miscibility of polar and non polar liquids?
What factor does the solubility of a gas in a liquid depend on according to Henry’s law?
What factor does the solubility of a gas in a liquid depend on according to Henry’s law?
According to Henry’s law, what happens to the solubility of a gas when the pressure above the solution is decreased?
According to Henry’s law, what happens to the solubility of a gas when the pressure above the solution is decreased?
What law states that the concentration of dissolved gas is proportional to the partial pressure of the gas above the solution at equilibrium?
What law states that the concentration of dissolved gas is proportional to the partial pressure of the gas above the solution at equilibrium?
What is the formula for calculating the concentration (C2) of dissolved gas according to Henry’s law?
What is the formula for calculating the concentration (C2) of dissolved gas according to Henry’s law?
What is the quantitative definition of solubility?
What is the quantitative definition of solubility?
What happens to a supersaturated solution when it contains more of the dissolved solute than it would normally contain at a definite temperature?
What happens to a supersaturated solution when it contains more of the dissolved solute than it would normally contain at a definite temperature?
What happens to the system between the cooling of the solution and the formation of glucose crystals when there is a higher amount of dissolved glucose than predicted by the solubility limit at 25 °C?
What happens to the system between the cooling of the solution and the formation of glucose crystals when there is a higher amount of dissolved glucose than predicted by the solubility limit at 25 °C?
What term is used to describe a solution that contains more dissolved solute than is predicted by the solubility limit?
What term is used to describe a solution that contains more dissolved solute than is predicted by the solubility limit?
What affects the solubility of substances in polar solvents?
What affects the solubility of substances in polar solvents?
In what type of solvent would nonpolar solutes dissolve best?
In what type of solvent would nonpolar solutes dissolve best?
What is the United States Pharmacopeia (USP) listing for expressing drug solubility?
What is the United States Pharmacopeia (USP) listing for expressing drug solubility?
What factor largely determines the solubility of a drug in a given solvent?
What factor largely determines the solubility of a drug in a given solvent?
What does a series of solvents of increasing polarity indicate?
What does a series of solvents of increasing polarity indicate?
How does branching of the carbon chain in aliphatic alcohols affect water solubility?
How does branching of the carbon chain in aliphatic alcohols affect water solubility?
Which of the following compounds can water dissolve due to hydrogen bond formation?
Which of the following compounds can water dissolve due to hydrogen bond formation?
What type of interaction forces does a polar solvent use to solvate molecules and ions?
What type of interaction forces does a polar solvent use to solvate molecules and ions?
What is the effect of a high dielectric constant in polar solvents on the force of attraction between oppositely charged ions in crystals?
What is the effect of a high dielectric constant in polar solvents on the force of attraction between oppositely charged ions in crystals?
What type of solvents are practically unable to dissolve ionic compounds?
What type of solvents are practically unable to dissolve ionic compounds?
What type of solution includes the solute in a concentration below that necessary for complete saturation at a definite temperature?
What type of solution includes the solute in a concentration below that necessary for complete saturation at a definite temperature?
What happens to the solubility of a gas in a liquid when the pressure above the solution is decreased?
What happens to the solubility of a gas in a liquid when the pressure above the solution is decreased?
What does Henry’s law state about the concentration of dissolved gas in a liquid?
What does Henry’s law state about the concentration of dissolved gas in a liquid?
In which type of solvent would ionic compounds be practically insoluble?
In which type of solvent would ionic compounds be practically insoluble?
What factor does the solubility of a gas in a liquid depend on according to Henry’s law?
What factor does the solubility of a gas in a liquid depend on according to Henry’s law?
What type of interaction forces do non polar solvents use to dissolve non polar solutes?
What type of interaction forces do non polar solvents use to dissolve non polar solutes?
What do semipolar solvents induce in non polar solvent molecules?
What do semipolar solvents induce in non polar solvent molecules?
What type of solution includes gases dissolved in liquids?
What type of solution includes gases dissolved in liquids?
What happens to the solubility of gases as the temperature increases?
What happens to the solubility of gases as the temperature increases?
What is the purpose of immersing a container with a gaseous solution in ice or cold water before opening it in warm climates?
What is the purpose of immersing a container with a gaseous solution in ice or cold water before opening it in warm climates?
What happens when electrolytes are added to gaseous solutions such as carbonated solutions?
What happens when electrolytes are added to gaseous solutions such as carbonated solutions?
What is an ideal solution according to Raoult's law?
What is an ideal solution according to Raoult's law?
In which type of liquid-liquid systems does complete miscibility occur?
In which type of liquid-liquid systems does complete miscibility occur?
What is the term used to describe the mutual solubility of the components in liquid-liquid systems?
What is the term used to describe the mutual solubility of the components in liquid-liquid systems?
How does the addition of a material soluble in only one of the two liquid components affect their mutual solubility?
How does the addition of a material soluble in only one of the two liquid components affect their mutual solubility?
What term is used to refer to the increase in mutual solubility of two partially miscible solvents by another agent?
What term is used to refer to the increase in mutual solubility of two partially miscible solvents by another agent?
What type of systems include the most important type of pharmaceutical solutions?
What type of systems include the most important type of pharmaceutical solutions?
What is an effect of temperature increase on the solubility of gases?
What is an effect of temperature increase on the solubility of gases?
How do complete miscibility occur in liquid-liquid systems?
How do complete miscibility occur in liquid-liquid systems?
What is the quantitative definition of solubility?
What is the quantitative definition of solubility?
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?
What happens to the system between the cooling of the solution and the formation of glucose crystals when there is a higher amount of dissolved glucose than predicted by the solubility limit at 25 °C?
What happens to the system between the cooling of the solution and the formation of glucose crystals when there is a higher amount of dissolved glucose than predicted by the solubility limit at 25 °C?
What is a saturated solution?
What is a saturated solution?
What is the effect of high dielectric constant in polar solvents on the force of attraction between oppositely charged ions in crystals?
What is the effect of high dielectric constant in polar solvents on the force of attraction between oppositely charged ions in crystals?
What type of solvents are unable to form hydrogen bonds with non-electrolytes?
What type of solvents are unable to form hydrogen bonds with non-electrolytes?
How do polar solvents break the covalent bonds of strong electrolytes?
How do polar solvents break the covalent bonds of strong electrolytes?
What allows polar solvents to solvate molecules and ions?
What allows polar solvents to solvate molecules and ions?
Which type of compounds can water dissolve due to hydrogen bond formation?
Which type of compounds can water dissolve due to hydrogen bond formation?
What type of solvents are practically unable to dissolve ionic compounds?
What type of solvents are practically unable to dissolve ionic compounds?
What is the effect of pressure on the concentration of dissolved gas in a liquid according to Henry's law?
What is the effect of pressure on the concentration of dissolved gas in a liquid according to Henry's law?
What does Henry’s law state about the concentration of dissolved gas in a liquid?
What does Henry’s law state about the concentration of dissolved gas in a liquid?
How do semipolar solvents induce a certain degree of polarity in non-polar solvent molecules?
How do semipolar solvents induce a certain degree of polarity in non-polar solvent molecules?
What type of solutions include gases dissolved in liquids?
What type of solutions include gases dissolved in liquids?
What type of compounds can non-polar solvents dissolve through weak van der Waals forces?
What type of compounds can non-polar solvents dissolve through weak van der Waals forces?
What factor does the solubility of a gas in a liquid depend on according to Henry’s law?
What factor does the solubility of a gas in a liquid depend on according to Henry’s law?
What type of solvents are practically unable to dissolve ionic compounds?
What type of solvents are practically unable to dissolve ionic compounds?
How does the branching of the carbon chain in aliphatic alcohols affect water solubility?
How does the branching of the carbon chain in aliphatic alcohols affect water solubility?
What effect does a high dielectric constant in polar solvents have on the force of attraction between oppositely charged ions in crystals?
What effect does a high dielectric constant in polar solvents have on the force of attraction between oppositely charged ions in crystals?
What factor largely determines the solubility of a drug in a given solvent?
What factor largely determines the solubility of a drug in a given solvent?
What does a series of solvents of increasing polarity show?
What does a series of solvents of increasing polarity show?
What type of compounds can water dissolve due to hydrogen bond formation?
What type of compounds can water dissolve due to hydrogen bond formation?
What term is used to describe a solution that contains more dissolved solute than is predicted by the solubility limit?
What term is used to describe a solution that contains more dissolved solute than is predicted by the solubility limit?
What happens when electrolytes are added to gaseous solutions such as carbonated solutions?
What happens when electrolytes are added to gaseous solutions such as carbonated solutions?
What factor does the solubility of a gas in a liquid depend on according to Henry’s law?
What factor does the solubility of a gas in a liquid depend on according to Henry’s law?
What happens to a supersaturated solution when it contains more of the dissolved solute than it would normally contain at a definite temperature?
What happens to a supersaturated solution when it contains more of the dissolved solute than it would normally contain at a definite temperature?
What term is used to refer to the increase in mutual solubility of two partially miscible solvents by another agent?
What term is used to refer to the increase in mutual solubility of two partially miscible solvents by another agent?
What do semipolar solvents induce in nonpolar solvent molecules?
What do semipolar solvents induce in nonpolar solvent molecules?
What effect does an increase in temperature have on the solubility of gases?
What effect does an increase in temperature have on the solubility of gases?
When adding electrolytes to gaseous solutions, what happens to the gases in the solution?
When adding electrolytes to gaseous solutions, what happens to the gases in the solution?
In liquid-liquid systems, when do complete miscibility occur?
In liquid-liquid systems, when do complete miscibility occur?
What is the term used to describe the mutual solubility of components in liquid-liquid systems?
What is the term used to describe the mutual solubility of components in liquid-liquid systems?
How does the addition of a material soluble in only one of the two liquid components affect their mutual solubility?
How does the addition of a material soluble in only one of the two liquid components affect their mutual solubility?
What type of interaction forces allow polar solvents to solvate molecules and ions?
What type of interaction forces allow polar solvents to solvate molecules and ions?
What happens to the mutual solubility of a liquid pair when a material soluble in both liquids is added?
What happens to the mutual solubility of a liquid pair when a material soluble in both liquids is added?
What is the term used to refer to the increase in mutual solubility of two partially miscible solvents by another agent?
What is the term used to refer to the increase in mutual solubility of two partially miscible solvents by another agent?
What is an effect of temperature increase on the solubility of gases?
What is an effect of temperature increase on the solubility of gases?
What happens to a supersaturated solution when it contains more of the dissolved solute than it would normally contain at a definite temperature?
What happens to a supersaturated solution when it contains more of the dissolved solute than it would normally contain at a definite temperature?
In which type of liquid-liquid systems does complete miscibility occur?
In which type of liquid-liquid systems does complete miscibility occur?
What happens when added material is soluble in only one of the two liquid components?
What happens when added material is soluble in only one of the two liquid components?
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Study Notes
Solution Definitions
- A solution that contains the dissolved solute in a concentration below that necessary for complete saturation at a definite temperature is an unsaturated solution.
- A solution that contains more dissolved solute than is predicted by the solubility limit is a supersaturated solution.
Solubility
- Solubility is the maximum amount of a substance that can dissolve in a solvent at a definite temperature.
- Solubility is affected by factors such as temperature and the dielectric constant of the solvent.
Polar Solvents
- Polar solvents dissolve polar solutes and ionic compounds.
- The dielectric constant (Ԑ) of a solvent affects the force of attraction between oppositely charged ions in crystals.
- A high dielectric constant in polar solvents reduces the force of attraction between oppositely charged ions in crystals, allowing for better solubility.
Non-Polar Solvents
- Non-polar solvents dissolve non-polar solutes through weak van der Waals forces.
- Non-polar solvents are unable to form hydrogen bonds with non-electrolytes.
Henry's Law
- Henry's law states that the concentration of dissolved gas is proportional to the partial pressure of the gas above the solution at equilibrium.
- The formula for calculating the concentration (C2) of dissolved gas according to Henry's law is C2 = k * P2.
- The solubility of a gas in a liquid depends on the pressure above the solution according to Henry's law.
Liquid-Liquid Systems
- Complete miscibility occurs in liquid-liquid systems when the components are mutually soluble.
- The term used to describe the mutual solubility of components in liquid-liquid systems is miscibility.
- The addition of a material soluble in only one of the two liquid components affects their mutual solubility.
Temperature Effects
- An increase in temperature increases the solubility of gases.
- Temperature increase affects the solubility of gases, especially in gaseous solutions such as carbonated solutions.
Pharmaceuticals
- The United States Pharmacopeia (USP) listing for expressing drug solubility is important in pharmaceuticals.
- The solubility of a drug in a given solvent is largely determined by the dielectric constant of the solvent.
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