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Questions and Answers
Which of the following is an example of a heterogeneous mixture?
Which of the following is an example of a heterogeneous mixture?
A concentrated solution has a low concentration of solute.
A concentrated solution has a low concentration of solute.
False (B)
What is the term for the component present in lesser quantity in a solution?
What is the term for the component present in lesser quantity in a solution?
solute
In a solution of salt and water, the salt is the ______ and the water is the ______.
In a solution of salt and water, the salt is the ______ and the water is the ______.
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Which type of solution is characterized by having no more solute that can be dissolved at a given temperature?
Which type of solution is characterized by having no more solute that can be dissolved at a given temperature?
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Match the following types of solutions with their definitions:
Match the following types of solutions with their definitions:
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Aqueous solutions use substances other than water as the solvent.
Aqueous solutions use substances other than water as the solvent.
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Give one example of a gas dissolved in a liquid.
Give one example of a gas dissolved in a liquid.
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What is the effect of temperature on the solubility of solids in liquids?
What is the effect of temperature on the solubility of solids in liquids?
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Pressure has a significant effect on the solubility of solids in liquids.
Pressure has a significant effect on the solubility of solids in liquids.
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What is Henry's Law?
What is Henry's Law?
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Gases that easily liquefy, such as ______, tend to be more soluble in liquids.
Gases that easily liquefy, such as ______, tend to be more soluble in liquids.
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Which of the following conditions increase the risk of nitrogen narcosis for deep-sea divers?
Which of the following conditions increase the risk of nitrogen narcosis for deep-sea divers?
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Match the following gases with their solubility characteristics:
Match the following gases with their solubility characteristics:
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The solubility of gases in liquids decreases with increasing pressure.
The solubility of gases in liquids decreases with increasing pressure.
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According to Raoult's Law, the partial vapor pressure of a component in a solution is directly proportional to its _______ fraction.
According to Raoult's Law, the partial vapor pressure of a component in a solution is directly proportional to its _______ fraction.
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What happens to the vapor pressure of a liquid as temperature increases?
What happens to the vapor pressure of a liquid as temperature increases?
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What is the main characteristic of ideal solutions?
What is the main characteristic of ideal solutions?
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What is defined as the number of moles of solute per liter of solution?
What is defined as the number of moles of solute per liter of solution?
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Molality is affected by temperature changes.
Molality is affected by temperature changes.
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Define mole fraction.
Define mole fraction.
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The volume of solution is expressed in ________ when calculating molarity.
The volume of solution is expressed in ________ when calculating molarity.
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Match the following types of solutions with their characteristics:
Match the following types of solutions with their characteristics:
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Which of the following best describes molality?
Which of the following best describes molality?
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A 1 molar solution of sugar is less concentrated than a 1 molal solution of sugar.
A 1 molar solution of sugar is less concentrated than a 1 molal solution of sugar.
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Explain how temperature affects the solubility of solids in liquids.
Explain how temperature affects the solubility of solids in liquids.
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The formula for molarity is M = ________ / Volume of solution (in liters).
The formula for molarity is M = ________ / Volume of solution (in liters).
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What does the assertion and reason analysis indicate if the assertion is correct but the reason is incorrect?
What does the assertion and reason analysis indicate if the assertion is correct but the reason is incorrect?
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Volume percentage is defined as the volume of the component divided by the mass of the solution.
Volume percentage is defined as the volume of the component divided by the mass of the solution.
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List two factors that affect solubility.
List two factors that affect solubility.
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The mole fraction of the solution is always equal to ________.
The mole fraction of the solution is always equal to ________.
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Match the concentration terms with their definitions:
Match the concentration terms with their definitions:
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Study Notes
Introduction to Solutions
- A solution is a homogeneous mixture of two or more substances.
- Homogeneous mixtures have a uniform composition throughout.
- Heterogeneous mixtures have a non-uniform composition.
- Common examples include sugar dissolved in water, salt dissolved in water, and lemonade.
Components of Solutions
- Solute: The component present in lesser quantity.
- Solvent: The component present in greater quantity.
- Examples of solute/solvent combinations include sugar and water (sugar is the solute, water is the solvent).
Types of Solutions
- Binary Solutions: Solutions made of two components.
- Ternary Solutions: Solutions made of three components.
- Quaternary Solutions: Solutions made of four components.
- Poly Solutions: Solutions made of multiple components.
- Diluted Solutions: Solutions with a low concentration of solute.
- Concentrated Solutions: Solutions with a high concentration of solute.
- Unsaturated Solutions: Solutions where more solute can be dissolved at a given temperature.
- Saturated Solutions: Solutions where no more solute can be dissolved at a given temperature.
- Aqueous Solutions: Solutions where water is the solvent.
- Non-Aqueous Solutions: Solutions where water is not the solvent.
Classifying Solutions: Solute and Solvent States
- Solid in Liquid: A solid solute dissolved in a liquid solvent. Examples include sugar in water and salt in water.
- Liquid in Liquid: A liquid solute dissolved in a liquid solvent. Examples include alcohol in water and vinegar.
- Gas in Liquid: A gaseous solute dissolved in a liquid solvent. Examples include carbon dioxide in water (soda) and oxygen in water (aquatic life).
- Solid in Gas: A solid solute dissolved in a gaseous solvent. Examples include smoke.
- Liquid in Gas: A liquid solute dissolved in a gaseous solvent. Examples include fog and clouds.
- Gas in Gas: A gaseous solute dissolved in a gaseous solvent. Example: Air.
- Solid in Solid: A solid solute dissolved in a solid solvent. Examples include alloys, such as brass and bronze (brass is an alloy of copper and zinc).
- Liquid in Solid: A liquid solute dissolved in a solid solvent. Examples include amalgams, such as mercury in sodium.
- Gas in Solid: A gaseous solute dissolved in a solid solvent. Examples include hydrogen dissolved in palladium.
Expressing Concentration Qualitatively
- Qualitative: Describing a solution's concentration based on visual observations.
- Quantitative: Describing a solution's concentration with numerical values, units, and formulas.
Expressing Concentration Quantitatively
- Mass Percentage: The mass of the component divided by the mass of the solution, multiplied by 100.
- Volume Percentage: The volume of the component divided by the volume of the solution, multiplied by 100.
Concentration Terms
- Volume by Volume Concentration (v/v): Expressed as the volume of solute per 100 mL of solution. Example: 15 mL of solute in 100 mL of solution.
- Mass by Volume Concentration (m/v): Represents the mass of solute (in grams) per 100 mL of solution. Example: 20 g of solute in 100 mL of solution.
- Volume by Mass Concentration (v/m): Indicates the volume of solute (in mL) per 100 g of the solution. Example: 20 mL of solute in 100 g of solution.
Mole Fraction
- Defined as the ratio of the number of moles of a component to the total number of moles in the solution.
- Represented by the symbol 'χ'.
- Formula: χA = Number of moles of A / Total number of moles in the solution.
- Key Properties:
- Unitless (moles cancel out in the ratio).
- The mole fraction of the solution is always equal to one (sum of mole fractions of each component).
- Independent of temperature (as it's a mass-by-mass concept).
Molarity
- Defined as the number of moles of solute dissolved per liter of solution.
- Represented by the symbol 'M'.
- Formula: Molarity (M) = Number of moles of solute / Volume of solution (in liters)
- Unit: Moles per liter (mol/L).
- Memorization Tip: "Washing Machine 1000 Milliliter" (W = mass of solute, M = molar mass of solute, 1000 = conversion factor).
- Dilution Equation: m1v1 = m2v2 (initial molarity & volume vs. final molarity & volume)
- Addition Equation: m1v1 + m2v2 = m3(v1 + v2) (molarities of solutions and their volumes)
Molality
- Defined as the number of moles of solute dissolved per kilogram of solvent.
- Represented by the symbol 'm'.
- Formula: Molality (m) = Number of moles of solute / Mass of solvent (in kilograms).
- Unit: Moles per kilogram (mol/kg).
- Memorization Tip: "Washing Machine 1000 Washing Ton" (mass of solute, molar mass of solute, conversion factor, mass of solvent, grams to kg conversion).
- Key Properties:
- A mass-by-mass concept and hence independent of temperature.
Key Differences between Molarity and Molality
- Definition: Molarity considers the volume of the solution, while molality focuses on the mass of the solvent.
- Units: Molarity is expressed in mol/L, while molality is in mol/kg.
- Temperature Dependence: Molarity varies with temperature due to changes in volume, while molality remains unchanged.
Types of Solutions (Solid Solution)
- Solid Solution: A homogeneous mixture where the solvent is a solid. Examples include alloys like brass (copper and zinc).
Assertion and Reason
- Assertion: A statement proposed to be true.
- Reason: A statement providing explanation for the assertion.
Analyzing Assertion and Reason Questions:
- A: Both assertion and reason correct; reason is correct explanation of assertion.
- B: Both assertion and reason correct; reason is not the correct explanation of assertion.
- C: Assertion correct, reason incorrect.
- D: Assertion incorrect, reason correct.
Molality and Temperature
- Molality of a substance does not change with temperature.
Volume of Solution and Temperature
- Volume of solution changes with temperature.
Defining Key Terms
- Molality: Number of moles of solute dissolved in 1 kilogram of solvent.
- Mole Fraction: Ratio of moles of a component to the total moles in the solution.
- Binary Solution: Contains two components; water may be solvent.
- Molarity: Number of moles of solute dissolved in 1 liter of solution.
Distinguishing between Molarity and Molality
- Molarity: moles of solute per liter of solution. Molality: moles of solute per kilogram of solvent.
- Molarity is affected by temperature, molality is not.
Converting Molarity to Molality
- Formula: M = (d * m * B) / (1 + (m * MB))
- M = Molarity
- d = Density
- m = Molality
- MB = Molar Mass of the solute in kilograms
Comparing Molar and Molal Solutions
- 1 molar sugar solution has 1 mole of sugar in 1 liter of solution.
- 1 molal sugar solution has 1 mole of sugar in 1 kilogram of solvent.
- Molar solutions typically more concentrated than molal solutions due to temperature insensitivity.
Defining Solubility
- Solubility is the maximum amount of solute that can dissolve in 100 grams of solvent at a given temperature.
Factors Affecting Solubility
- Nature of Solute and Solvent: "Like dissolves like." Polar solutes dissolve in polar solvents, and nonpolar solutes dissolve in nonpolar solvents. Example: Salt (NaCl) dissolves in water (H₂O) due to polarity but not in oil.
- Temperature: Solubility of solids in liquids generally increases with increasing temperature. Endothermic reactions increase solubility with temperature, exothermic reactions decrease.
- Pressure: Pressure has a negligible effect on the solubility of solids in liquids.
Solubility of Gases in Liquids
- Nature of the Gas: Gases easily liquefied (e.g., CO₂, NH₃, SO₂) tend to be more soluble than gases that don't easily liquefy.
-
Pressure: The solubility of gases in liquids increases with increasing pressure (Henry's Law).
- Henry's Law: Solubility of a gas is proportional to its partial pressure above the liquid.
-
Formula: P = kC
- P = partial pressure of the gas.
- k = Henry's Law constant.
- C = concentration of the dissolved gas.
- Temperature: Solubility of gases in liquids generally decreases with increasing temperature.
Applications of Henry's Law
- High pressure in soda bottles increases CO₂ solubility. Opening a soda releases pressure, reducing CO₂ solubility and releasing bubbles.
- Deep-sea divers use gas mixtures without nitrogen to avoid nitrogen narcosis (excessive nitrogen solubility in blood).
Pressure and Solubility
- Solubility of gases decreases with decreasing pressure.
- Scuba divers experience increased gas solubility at higher pressures and rapid release at lower pressures.
- Use of helium in scuba diving equipment reduces blood nitrogen solubility, preventing decompression sickness (the bends).
High Altitude Affects
- Lower atmospheric pressure leads to lower oxygen intake & results in anoxia (lack of oxygen).
- Symptoms such as fatigue, impaired cognitive function, and difficulty breathing.
Vapor Pressure
- Vapor pressure is the pressure exerted by the vapor of a liquid in equilibrium with its liquid phase.
- Factors Affecting Vapor Pressure:
- Intermolecular interactions (weaker = higher vapor pressure)
- Temperature (higher = higher vapor pressure)
- Boiling point (higher = lower vapor pressure)
- Volatile solutes (increase vapor pressure)
- Non-volatile solutes (decrease vapor pressure)
Raoult's Law
- Raoult's Law states that the partial vapor pressure of a component in a solution is directly proportional to its mole fraction.
-
Partial Vapor Pressure of Component A:
(P_A = P^o_A \times X_A)
- (P_A) = Partial vapor pressure of component A in the solution.
- (P^o_A) = Vapor pressure of pure component A.
- (X_A) = Mole fraction of component A in the solution.
Types of Solutions
- Ideal Solutions: Obey Raoult's Law at all concentrations and temperatures; similar intermolecular interactions; no volume/enthalpy change upon mixing. Examples: Hexane and Heptane, Benzene and Toluene.
- Non-Ideal Solutions: Deviate from Raoult's Law; different intermolecular forces; volume/enthalpy change upon mixing. Examples: Water and Ethanol, Chloroform and Acetone.
Positive Deviation From Raoult's Law
- Solute-solvent interactions weaker than solute-solute and solvent-solvent interactions. Higher vapor pressure than predicted by Raoult's Law. Volume increases, enthalpy positive (endothermic). Example: Water and Ethanol.
Negative Deviation From Raoult's Law
- Solute-solvent interactions stronger than solute-solute and solvent-solvent interactions. Lower vapor pressure than predicted. Volume decreases, enthalpy negative (exothermic). Example: Acetone and Chloroform.
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Description
This quiz covers the fundamental concepts of solutions, including definitions, components, and types of mixtures. Understand the difference between solutes and solvents, as well as the characteristics of various solution types such as binary, ternary, and concentrated solutions. Test your knowledge on these essential chemistry concepts.
