Podcast
Questions and Answers
Which scenario best illustrates Henry's Law regarding gas solubility in liquids?
Which scenario best illustrates Henry's Law regarding gas solubility in liquids?
- Adding salt to a solution, causing a gas to be less soluble.
- Heating a carbonated beverage, causing it to lose fizz.
- Chemically reacting a gas with a solvent to increase its solubility through compound formation.
- Increasing the partial pressure of a gas above a liquid, resulting in more gas dissolving into the liquid. (correct)
In the context of gas solubility in liquids, how does increasing temperature typically affect the solubility of most gases, and why?
In the context of gas solubility in liquids, how does increasing temperature typically affect the solubility of most gases, and why?
- Causes a chemical reaction that binds the gas to the solvent, increasing solubility.
- Increases solubility due to enhanced kinetic energy facilitating dissolution.
- Decreases solubility because the gas has a greater tendency to expand, reducing interaction with the solvent. (correct)
- Has no effect as temperature only affects the solubility of solids in liquids.
How does the addition of electrolytes like NaCl to an aqueous solution containing a dissolved gas typically affect the gas's solubility, and what is this phenomenon called?
How does the addition of electrolytes like NaCl to an aqueous solution containing a dissolved gas typically affect the gas's solubility, and what is this phenomenon called?
- Increases solubility due to enhanced polarity of the solvent.
- Decreases solubility, known as 'salting out'. (correct)
- Has no effect due to the inert nature of electrolytes.
- Increases solubility, known as 'salting in'.
Under what conditions is Henry's Law most accurately applied regarding the solubility of gases in solvents?
Under what conditions is Henry's Law most accurately applied regarding the solubility of gases in solvents?
If the concentration of CO2 dissolved in sparkling water in a closed soda can is 0.150 m at 25°C, and Henry's constant for CO2 in water at 25°C is 0.034 mol/kg·bar, what is the partial pressure of CO2 (g) in the can?
If the concentration of CO2 dissolved in sparkling water in a closed soda can is 0.150 m at 25°C, and Henry's constant for CO2 in water at 25°C is 0.034 mol/kg·bar, what is the partial pressure of CO2 (g) in the can?
A tank is filled with H₂O(g) and H₂ (g). The total pressure in the tank is 10 bar at 0 °C, and the partial pressure of H₂O(g) is 0.15 bar. If Henry's constant for H₂ (g) at 0 °C is 7.8 x 10⁻⁴ mol/kg·bar, what is the concentration of H₂ (g) in the water?
A tank is filled with H₂O(g) and H₂ (g). The total pressure in the tank is 10 bar at 0 °C, and the partial pressure of H₂O(g) is 0.15 bar. If Henry's constant for H₂ (g) at 0 °C is 7.8 x 10⁻⁴ mol/kg·bar, what is the concentration of H₂ (g) in the water?
Which of the following statements accurately describes the concept of 'salting out' in the context of gas solubility?
Which of the following statements accurately describes the concept of 'salting out' in the context of gas solubility?
What fundamental criterion must be met for a solution to be considered 'ideal' according to Raoult's Law?
What fundamental criterion must be met for a solution to be considered 'ideal' according to Raoult's Law?
Which of the following is a correct characteristic of an ideal solution regarding its thermodynamic properties upon mixing?
Which of the following is a correct characteristic of an ideal solution regarding its thermodynamic properties upon mixing?
When mixing 100 ml of methanol with 100 ml of ethanol, the resulting volume is nearly 200 ml. According to this observation, how would you categorize this mixture?
When mixing 100 ml of methanol with 100 ml of ethanol, the resulting volume is nearly 200 ml. According to this observation, how would you categorize this mixture?
How does the partial pressure of a component in an ideal liquid mixture relate to its mole fraction and vapor pressure in the pure state, according to Raoult's Law?
How does the partial pressure of a component in an ideal liquid mixture relate to its mole fraction and vapor pressure in the pure state, according to Raoult's Law?
In ideal solutions, what determines the total vapor pressure above a mixture of volatile components?
In ideal solutions, what determines the total vapor pressure above a mixture of volatile components?
What is the primary distinction between solutions that exhibit 'positive deviation' and those with 'negative deviation' from Raoult's Law?
What is the primary distinction between solutions that exhibit 'positive deviation' and those with 'negative deviation' from Raoult's Law?
Which scenario exemplifies a negative deviation from Raoult's Law?
Which scenario exemplifies a negative deviation from Raoult's Law?
How do adhesion forces compare in mixtures that exhibit a negative deviation from Raoult's Law, relative to cohesion forces?
How do adhesion forces compare in mixtures that exhibit a negative deviation from Raoult's Law, relative to cohesion forces?
Consider a mixture of two substances where the partial vapor pressure of the constituents is higher than expected based on Raoult's Law. What type of deviation does this mixture exhibit, and what is its effect on solubility?
Consider a mixture of two substances where the partial vapor pressure of the constituents is higher than expected based on Raoult's Law. What type of deviation does this mixture exhibit, and what is its effect on solubility?
What is the partial vapor pressure of benzene and ethylene chloride in a solution with a mole fraction of benzene of 0.6, given that the vapor pressure of pure benzene at 50 °C is 286 mmHg and that of ethylene chloride is 236 mmHg? Also, what is the total vapor pressure?
What is the partial vapor pressure of benzene and ethylene chloride in a solution with a mole fraction of benzene of 0.6, given that the vapor pressure of pure benzene at 50 °C is 286 mmHg and that of ethylene chloride is 236 mmHg? Also, what is the total vapor pressure?
If 2 moles of substance A are mixed with 3 moles of substance B, and the vapor pressures of substances A and B are 500 torr and 200 torr, respectively, and the observed vapor pressure of the solution is 294 torr, is this solution ideal? If not, what type of deviation is observed?
If 2 moles of substance A are mixed with 3 moles of substance B, and the vapor pressures of substances A and B are 500 torr and 200 torr, respectively, and the observed vapor pressure of the solution is 294 torr, is this solution ideal? If not, what type of deviation is observed?
What characterizes a system of two liquids that are considered 'completely miscible'?
What characterizes a system of two liquids that are considered 'completely miscible'?
What are 'conjugate liquid phases' in the context of liquid-liquid systems?
What are 'conjugate liquid phases' in the context of liquid-liquid systems?
How does temperature affect the mutual solubility of two partially miscible liquids?
How does temperature affect the mutual solubility of two partially miscible liquids?
What is the significance of the 'Critical Solution Temperature' (CST) in a system of two partially miscible liquids?
What is the significance of the 'Critical Solution Temperature' (CST) in a system of two partially miscible liquids?
For a phenol/water system, what occurs at the upper Critical Solution Temperature (CST)?
For a phenol/water system, what occurs at the upper Critical Solution Temperature (CST)?
How does temperature affect the miscibility of triethylamine in water, and what characterizes this system?
How does temperature affect the miscibility of triethylamine in water, and what characterizes this system?
What unique miscibility characteristic does the nicotine/water system exhibit compared to phenol/water and triethylamine/water systems?
What unique miscibility characteristic does the nicotine/water system exhibit compared to phenol/water and triethylamine/water systems?
In the context of ternary systems, what happens when a third component is added to a pair of partially miscible liquids, and that component is soluble in only one of the two liquids?
In the context of ternary systems, what happens when a third component is added to a pair of partially miscible liquids, and that component is soluble in only one of the two liquids?
What is the likely effect on the mutual solubility of two partially miscible liquids when a third component, soluble in both of those liquids, is added to the system?
What is the likely effect on the mutual solubility of two partially miscible liquids when a third component, soluble in both of those liquids, is added to the system?
Flashcards
Gas solubility in a liquid
Gas solubility in a liquid
The concentration of dissolved gas in a liquid when it's at equilibrium with the pure gas above.
Henry's Law
Henry's Law
In a dilute solution, the concentration of a gas that dissolves in a liquid is directly proportional to the partial pressure of the gas
Temperature impact on gas solubility
Temperature impact on gas solubility
Raising temperature usually decrease gas solubility because of the greater tendency of the gases to expand.
Salting out
Salting out
Signup and view all the flashcards
Effect of Reaction on Gas Solubility
Effect of Reaction on Gas Solubility
Signup and view all the flashcards
Ideal solution
Ideal solution
Signup and view all the flashcards
Ideal solution characteristics
Ideal solution characteristics
Signup and view all the flashcards
Raoult's Law
Raoult's Law
Signup and view all the flashcards
Real Solutions
Real Solutions
Signup and view all the flashcards
Negative deviation
Negative deviation
Signup and view all the flashcards
Positive deviation
Positive deviation
Signup and view all the flashcards
Complete Miscibility
Complete Miscibility
Signup and view all the flashcards
Partial Miscibility
Partial Miscibility
Signup and view all the flashcards
Critical Solution Temperature (CST)
Critical Solution Temperature (CST)
Signup and view all the flashcards
Ternary Systems.
Ternary Systems.
Signup and view all the flashcards
Study Notes
Solubility of Gases in Liquids
- Refers to a gas's concentration when in equilibrium with its pure form above a solution.
- Effervescent preparations, ammonia water, hydrochloric acid (HCl gas in water), and carbonated water are examples of pharmaceutical solutions with dissolved gases.
Factors Affecting the Solubility of a Gas
- Pressure, temperature, and presence of electrolytes/non-electrolytes influences the solubility of a gas in a solvent.
Effect of Pressure
- Henry's Law describes the effect of pressure on gas solubility.
- Henry's Law is given by: C = K * P(gas)
- C represents the dissolved gas concentration in gm/liter, and P represents the partial pressure in mmHg or torr.
- An increased solubility of gases is observed with increased pressure, gases escape when the pressure decreases.
Effect of Temperature
- The solubility of most gases decreases as temperature increases due to the gases' greater tendency to expand relative to the solvent.
Effect of Electrolytes and Non-Electrolytes
- Electrolytes such as NaCl and non-electrolytes decrease gas solubility in a solution, an effect known as "salting out."
- "Salting out" happens because of a higher affinity between the solvent and the electrolyte or non-electrolyte than between the solvent and the gas.
Effect of Chemical Reaction
- Henry's Law only applies to slightly soluble gases that do not react with the solvent.
- Chemical reactions between the gas and solvent increases solubility.
- Ex: HCl gas dissolves in water due to hydrogen bonding.
Solubility of Liquids in Liquids
- Hydroalcoholic solutions, peppermint water, and medicated oils are examples of liquids soluble in liquids
Ideal Solutions
- Follow Raoult's law across all compositions and temperatures.
- Benzene/Toluene, Methanol/Ethanol, and Hexane/Heptane are examples of ideal solutions.
Ideal Solutions vs Non-Ideal Solutions
- Ideal Solutions: Exhibit no changes in properties other than dilution of the component. This means the mixing process does not involve evolved or absorbed heat.
- Non-Ideal/Real Solutions: Changes in the properties of the components as well as the evolution or absorption of heat when they are mixed.
- Ideal Solutions obey Raoult's Law across all temperatures, and non-ideal solutions typically do not obey Raoult's law.
Raoult's Law
- States the partial pressure of a component A in a liquid mixture is equal to the vapor pressure in its pure state, multiplied by the mole fraction of the component in the solution (represented by PA = PAo * XA)
- Raoult's Law, describes that the pressure (Psolvent) is equal to the vapor pressure multiplied by the mole fraction.
- The total vapor pressure is the sum of the partial vapor pressures of each component.
Non Ideal Solutions
- Solutions include deviations from Raoult's Law, and deviations include negative deviations and positive deviations.
- Negative Deviation: Solubility increases due to hydrogen bonding between polar components.
- Positive Deviation: Solubility decreases because molecules of one component associate to form polymers.
Negative vs Positive Deviations
- Negative Deviation: Greater adhesive forces.
- Positive Deviation: Lesser adhesive forces.
- Negative Deviation: The dilution of chloroform with acetone reduces the vapor pressure of chloroform
- Positive Deviation: The dilution of benzene with ethyl alcohol increases the vapor pressure of benzene.
- Negative Deviation: The partial vapor pressure of the constituents is less than expected from Raoult's Law, with a minimum value showcased on the total vapor pressure curve.
- Positive Deviation: The partial vapor pressure of the constituents is greater than expected from Raoult's Law, with a maximum value showcased on the total vapor pressure curve.
- Negative Deviation: For example, chloroform is mixed with acetone.
- Positive Deviation: For example, benzene is added to ethyl alcohol.
- Negative Deviation: Leads to an increase in solubility and is frequently associated with hydrogen bonding between polar components.
- Positive Deviation: This leads to a decrease in solubility due to the association of one of the constituents to form double molecules (dimers) or polymers of high order.
Categories of Liquid-Liquid Systems
- Liquid-liquid systems can be characterized by complete miscibility and partial miscibility.
Complete Miscible
- Systems are mixed in any proportion without any solubility issues.
- Includes polar and semipolar liquids such as alcohol, glycerin, and alcohol
- Nonpolar solvents are completely miscible when mixed, such as benzene and carbon tetrachloride.
Partial Miscible
- These systems form two immiscible layers, each forming a saturated solution of one liquid in the other, that are conjugate liquid phases.
- A mutual solubility of one in the other is reached, such as water/ether or water/phenol systems.
- Temperature significantly affects the mutual solubility.
Phenol/Water System
- As temperature increases, the solubility increases.
- The critical solution temperature (CST) is about 66.8 degrees celcius in all proportions.
Triethylamine/Water System
- As temperature decreases there is an increased solubility of liquids.
- The system has a lower C.S.T at 18.5°C
Nicotine/Water System
- There is an upper C.S.T at 208°C as well as a lower C.S.T at 60.8°C.
- Between 60.8 and 208°C nicotine and water are partially miscible.
Ternary Systems
- Created by introducing a third component to a pair of partially miscible liquids.
- If the added component is soluble in any of the other two, or its solubility isn't the same the solubility decreases of the liquids.
- If the added component is miscible, the solubility of two liquids is increased.
Studying That Suits You
Use AI to generate personalized quizzes and flashcards to suit your learning preferences.
