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Questions and Answers
What type of solution is characterized by having particle sizes between that of true solutions and coarse dispersions?
What type of solution is characterized by having particle sizes between that of true solutions and coarse dispersions?
In a binary solution, what is generally designated as the solvent when a solid is dissolved in a liquid?
In a binary solution, what is generally designated as the solvent when a solid is dissolved in a liquid?
Which property of solutions is primarily influenced by the number of solute particles present?
Which property of solutions is primarily influenced by the number of solute particles present?
Which example can be classified as a true solution?
Which example can be classified as a true solution?
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In a two-phase heterogeneous system, which of the following is an example?
In a two-phase heterogeneous system, which of the following is an example?
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What type of solution is formed when substances do not agree to form distinct solute and solvent phases?
What type of solution is formed when substances do not agree to form distinct solute and solvent phases?
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What do additive properties of a solution depend on?
What do additive properties of a solution depend on?
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Which of the following examples best describes a coarse dispersion?
Which of the following examples best describes a coarse dispersion?
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Which of the following is an example of a gas-liquid solution?
Which of the following is an example of a gas-liquid solution?
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What characterizes an ideal solution during mixing?
What characterizes an ideal solution during mixing?
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Which of these mixtures is classified as a solid-liquid solution?
Which of these mixtures is classified as a solid-liquid solution?
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What happens to the volume of a non-ideal solution when mixing sulfuric acid and water?
What happens to the volume of a non-ideal solution when mixing sulfuric acid and water?
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Which statement about solution concentration is true?
Which statement about solution concentration is true?
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In ideal solutions, what governs the weighted averages of vapor pressure and viscosity?
In ideal solutions, what governs the weighted averages of vapor pressure and viscosity?
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Which factor does NOT contribute to the non-ideality of a solution?
Which factor does NOT contribute to the non-ideality of a solution?
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Which is an example of a gas-solid solution?
Which is an example of a gas-solid solution?
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What is the definition of a concentrated solution?
What is the definition of a concentrated solution?
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How is mass percent of a solution calculated?
How is mass percent of a solution calculated?
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What does a 10% (w/v) NaCl solution imply?
What does a 10% (w/v) NaCl solution imply?
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Which of the following correctly defines molarity (M)?
Which of the following correctly defines molarity (M)?
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What is the formula to calculate molality (m)?
What is the formula to calculate molality (m)?
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What does normality (N) refer to in solution chemistry?
What does normality (N) refer to in solution chemistry?
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What does the mole fraction represent?
What does the mole fraction represent?
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In calculating the mass percent of a solution, how much would a solution with 10 g of sugar in 100 g of water yield?
In calculating the mass percent of a solution, how much would a solution with 10 g of sugar in 100 g of water yield?
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Study Notes
Physical Pharmacy (II) - Solutions
- Solutions are homogeneous mixtures of two or more pure substances, with uniform composition.
- Solutions can be true solutions, colloidal solutions, or coarse dispersions.
- A true solution is a homogeneous molecular dispersion (one phase).
- The composition of a true solution can vary widely.
Phases
- A phase is a homogeneous part of a system separated by definite boundaries.
- Colloidal dispersions have particle sizes between true solutions and coarse dispersions (roughly 10 Å to 5000 Å).
- Coarse dispersions have larger particle sizes (greater than 0.1 µm or 10⁻⁵ cm).
Binary Solutions
- A binary solution is composed of two substances: a solvent (usually present in greater amount) and a solute.
- When a solid dissolves in a liquid, the liquid is typically considered the solvent.
- Water is often taken as the solvent in mixtures.
- Determining solute and solvent in some liquid mixtures can be difficult (e.g., alcohol and water).
Types of Solutions
- Heterogeneous: Two-phase system. Example: Silver Proteinate in water.
- Homogeneous: Single-phase system, like solutions of acacia in water or sodium carboxymethylcellulose in water. These may also be true solutions.
Properties of Solutions
- Colligative Properties: Depend on the number of particles in solution. Examples are osmotic pressure, vapor pressure lowering, freezing point depression, and boiling point elevation.
- Additive Properties: Depend on the sum of the properties of the constituents. Examples include molecular weight and the total mass of components.
- Constitutive Properties: Depend on the arrangement of atoms within molecules. Examples include refraction of light, electrical properties, surface characteristics, and solubility.
Ideal and Real Solutions
- Ideal Solutions: Formed by mixing substances with similar properties. No heat is evolved or absorbed during mixing. Example: Mixing 100 mL methanol with 100 mL ethanol results in a 200 mL mixture with no heat change. The properties of the constituents change only by dilution.
- Real Solutions (Non-ideal): Do not always adhere to Raoult's Law and interactions between constituents are more complex. Example: 100 mL sulfuric acid + 100 mL water does not equal 200 mL.
Solution Concentration
- Dilute Solution: Contains a small amount of solute per unit volume.
- Concentrated Solution: Contains a relatively large amount of solute per unit volume. Various expressions exist for solution concentrations.
Concentration Expressions
- Mass percent (w/w): Mass of solute per 100 g of solution
- Percent weight by volume (w/v): Mass of solute per 100 parts (volume) of solution (when solvent volume isn't exactly known).
- Volume by volume (v/v): Volume of solute per 100 parts (volume) of solution (volumes are often assumed as equal).
Other Concentration Expressions
- Molarity (M): Number of moles of solute per liter of solution
- Molality (m): Number of moles of solute per kilogram of solvent
- Normality (N): Gram equivalent weights of solute in 1 liter of solution
- Mole Fraction: Expresses the moles of a component relative to the total moles of the solution.
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Description
Test your knowledge of solutions in physical pharmacy with this comprehensive quiz. Explore concepts such as true solutions, colloidal dispersions, and binary solutions. Understand the definitions and characteristics that differentiate these types of mixtures.
