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Questions and Answers
What is the defining characteristic of a saturated solution?
What is the defining characteristic of a saturated solution?
- Contains solute at a concentration equal to its solubility (correct)
- Contains solute at a concentration below its solubility
- Contains solute at a concentration above its solubility
- Contains no solute
What is a supersaturated solution?
What is a supersaturated solution?
- A solution with a concentration equal to its solubility
- A solution with a lower concentration than its solubility
- A solution with no solute present
- A nonequilibrium condition where the solute's concentration exceeds its solubility (correct)
How do the solubilities of gaseous solutes change with increasing temperature?
How do the solubilities of gaseous solutes change with increasing temperature?
- They increase
- They become immiscible
- They remain constant
- They decrease (correct)
What is the relation known as Henry’s law in relation to gaseous solutes?
What is the relation known as Henry’s law in relation to gaseous solutes?
What are colligative properties of a solution dependent on?
What are colligative properties of a solution dependent on?
What does the total concentration of solute particles in a solution determine?
What does the total concentration of solute particles in a solution determine?
How does the solubility of most solids in water change with temperature?
How does the solubility of most solids in water change with temperature?
What happens when a solution saturated at an elevated temperature is cooled to a lower temperature without precipitating the solute?
What happens when a solution saturated at an elevated temperature is cooled to a lower temperature without precipitating the solute?
How can precipitation of excess solute in a supersaturated solution be initiated?
How can precipitation of excess solute in a supersaturated solution be initiated?
What is the main advantage of using some hand warmers based on supersaturated solutions?
What is the main advantage of using some hand warmers based on supersaturated solutions?
What is the result of a solution being supersaturated?
What is the result of a solution being supersaturated?
In what way can the temperature dependence of solubility be exploited to prepare supersaturated solutions?
In what way can the temperature dependence of solubility be exploited to prepare supersaturated solutions?
What is a solution with a relatively low concentration of solute called?
What is a solution with a relatively low concentration of solute called?
In a supersaturated solution, the solute concentration exceeds its:
In a supersaturated solution, the solute concentration exceeds its:
What is the opposite of a concentrated solution?
What is the opposite of a concentrated solution?
What happens to the CO2 concentration in a supersaturated carbonated beverage over time?
What happens to the CO2 concentration in a supersaturated carbonated beverage over time?
In a supersaturated solution, what is the sole energetic factor affecting solubility?
In a supersaturated solution, what is the sole energetic factor affecting solubility?
What type of intermolecular attraction needs to be overcome when a gaseous solute dissolves in a liquid solvent?
What type of intermolecular attraction needs to be overcome when a gaseous solute dissolves in a liquid solvent?
What happens to cells when a hypertonic solution is injected?
What happens to cells when a hypertonic solution is injected?
What is the term used to describe the process when cells lose water and shrivel in a hypertonic solution?
What is the term used to describe the process when cells lose water and shrivel in a hypertonic solution?
Which property is directly proportional to the number of solute species present in a given amount of solution?
Which property is directly proportional to the number of solute species present in a given amount of solution?
What property permits determination of a solute’s molar mass when measured for a solution prepared using a known mass of solute?
What property permits determination of a solute’s molar mass when measured for a solution prepared using a known mass of solute?
In which type of solution do cells swell and possibly rupture?
In which type of solution do cells swell and possibly rupture?
What is the term used to describe the process when cells swell and possibly rupture in a hypotonic solution?
What is the term used to describe the process when cells swell and possibly rupture in a hypotonic solution?
Why are supersaturated solutions of most solids in water prepared by cooling saturated solutions?
Why are supersaturated solutions of most solids in water prepared by cooling saturated solutions?
Why are supersaturated solutions of most gases in water prepared by heating saturated solutions?
Why are supersaturated solutions of most gases in water prepared by heating saturated solutions?
What is the likely reason for ethanol (C2H5OH) being completely miscible with water?
What is the likely reason for ethanol (C2H5OH) being completely miscible with water?
Why is ethanethiol (C2H5SH) only soluble to the extent of 1.5 g per 100 mL of water?
Why is ethanethiol (C2H5SH) only soluble to the extent of 1.5 g per 100 mL of water?
Which of the following gases is expected to be most soluble in water?
Which of the following gases is expected to be most soluble in water?
At 0 °C and 4.00 atm, how many grams of O2 dissolve in 1 L of water?
At 0 °C and 4.00 atm, how many grams of O2 dissolve in 1 L of water?
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Study Notes
Solution Characteristics
- A saturated solution is defined as one that contains the maximum amount of solute that can be dissolved under a given set of conditions.
- A supersaturated solution is a solution that contains more solute than it can theoretically hold at a given temperature, often prepared by slowly cooling a saturated solution.
Gaseous Solutes
- The solubility of gaseous solutes generally decreases with increasing temperature.
- Henry's law states that the solubility of a gas in a liquid is directly proportional to the pressure of the gas above the solution.
Colligative Properties
- Colligative properties of a solution are dependent on the total concentration of solute particles, not the type of solute.
- The total concentration of solute particles in a solution determines the osmotic pressure, boiling point elevation, and freezing point depression.
Solubility and Temperature
- The solubility of most solids in water increases with temperature.
- When a solution saturated at an elevated temperature is cooled to a lower temperature without precipitating the solute, it becomes supersaturated.
- Supersaturated solutions can be prepared by exploiting the temperature dependence of solubility.
Supersaturated Solutions
- A solution with a relatively low concentration of solute is called a dilute solution.
- In a supersaturated solution, the solute concentration exceeds its equilibrium value, and the solution is unstable.
- The main advantage of using some hand warmers based on supersaturated solutions is that they can release heat energy when the excess solute precipitates.
Biological Effects
- When a hypertonic solution is injected into cells, the cells lose water and shrivel, a process called crenation.
- In a hypotonic solution, cells swell and possibly rupture, a process called hemolysis.
- Osmotic pressure is directly proportional to the number of solute species present in a given amount of solution.
Solubility and Intermolecular Forces
- The sole energetic factor affecting solubility in a supersaturated solution is the intermolecular attraction between the solute and solvent.
- The type of intermolecular attraction that needs to be overcome when a gaseous solute dissolves in a liquid solvent is London dispersion forces.
Solubility of Specific Substances
- Ethanol (C2H5OH) is completely miscible with water due to its ability to form hydrogen bonds with water.
- Ethanethiol (C2H5SH) is only soluble to the extent of 1.5 g per 100 mL of water because it is a larger and more polar molecule than ethanol.
- Oxygen is expected to be the most soluble of the following gases in water at 0 °C and 4.00 atm, with 1.38 g dissolving in 1 L of water.
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