Physical Pharmacy II - Solutions Quiz
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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?

  • True solution
  • Suspension
  • Colloidal solution (correct)
  • Coarse dispersion

In a binary solution, what is generally designated as the solvent when a solid is dissolved in a liquid?

  • The solid, in all cases
  • The substance in lesser quantity
  • The liquid, regardless of amount (correct)
  • The substance with the higher boiling point

Which property of solutions is primarily influenced by the number of solute particles present?

  • Colligative Properties (correct)
  • Thermodynamic Properties
  • Constitutive Properties
  • Additive Properties

Which example can be classified as a true solution?

<p>Solution of sodium chloride in water (C)</p> Signup and view all the answers

In a two-phase heterogeneous system, which of the following is an example?

<p>Silver proteinate in water (A)</p> Signup and view all the answers

What type of solution is formed when substances do not agree to form distinct solute and solvent phases?

<p>Miscible solution (C)</p> Signup and view all the answers

What do additive properties of a solution depend on?

<p>The sum of properties of individual components (D)</p> Signup and view all the answers

Which of the following examples best describes a coarse dispersion?

<p>Dirt suspended in water (D)</p> Signup and view all the answers

Which of the following is an example of a gas-liquid solution?

<p>Carbonated water (A)</p> Signup and view all the answers

What characterizes an ideal solution during mixing?

<p>No change in the properties other than dilution (B)</p> Signup and view all the answers

Which of these mixtures is classified as a solid-liquid solution?

<p>Mineral oil in paraffin (B)</p> Signup and view all the answers

What happens to the volume of a non-ideal solution when mixing sulfuric acid and water?

<p>Volume increases beyond the sum of each component (B)</p> Signup and view all the answers

Which statement about solution concentration is true?

<p>The terms dilute and concentrated are relative and have no fixed meaning (C)</p> Signup and view all the answers

In ideal solutions, what governs the weighted averages of vapor pressure and viscosity?

<p>Pure individual constituents (A)</p> Signup and view all the answers

Which factor does NOT contribute to the non-ideality of a solution?

<p>Uniform attractive forces between solute and solvent (B)</p> Signup and view all the answers

Which is an example of a gas-solid solution?

<p>Hydrogen in palladium (B)</p> Signup and view all the answers

What is the definition of a concentrated solution?

<p>A solution with a relatively greater amount of solute per unit volume. (B)</p> Signup and view all the answers

How is mass percent of a solution calculated?

<p>Mass of solute divided by total mass of solution times 100. (B)</p> Signup and view all the answers

What does a 10% (w/v) NaCl solution imply?

<p>10 g NaCl dissolved in 100 cm³ of solution. (D)</p> Signup and view all the answers

Which of the following correctly defines molarity (M)?

<p>The number of moles of solute per liter of solution. (A)</p> Signup and view all the answers

What is the formula to calculate molality (m)?

<p>Moles of solute divided by kilograms of solvent. (A)</p> Signup and view all the answers

What does normality (N) refer to in solution chemistry?

<p>Gram equivalent weights of solute in one liter of solution. (A)</p> Signup and view all the answers

What does the mole fraction represent?

<p>The ratio of the number of moles of one component to the total number of moles in the solution. (D)</p> Signup and view all the answers

In calculating the mass percent of a solution, how much would a solution with 10 g of sugar in 100 g of water yield?

<p>9.09% (A)</p> Signup and view all the answers

Flashcards

Solution

A homogeneous mixture of two or more pure substances with a uniform composition throughout.

True solution

A homogeneous molecular dispersion (one phase system) of two or more components. The composition can vary over a wide range.

Colloidal solution

A system having a particle size intermediate between that of a true solution and a coarse dispersion, roughly 10 Angstroms to 5000 Angstroms.

Coarse dispersion

The diameter of the particles in emulsions and suspensions for the most part being larger than 0.1 µm (1000 Angstroms or 10-5 cm).

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Binary solution

A solution composed of only two substances: a solvent and a solute. The solvent is usually present in a greater amount and the solute in a lesser amount.

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Colligative properties (of solutions)

Properties that depend mainly on the number of particles in the solution.

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Additive properties (of solutions)

Properties that depend on the total contribution of atoms in a molecule or the sum of the properties of the constituents in the solution.

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Constitutive properties (of solutions)

Properties that depend on the arrangement and to a lesser extent on the number and kinds of atoms within the molecules.

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Mass Percent

The mass of solute present in 100 g of solution. It's also known as percent weight/weight.

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Percent Weight by Volume (w/v)

The amount of solute dissolved per 100 parts by volume of the solution (not the volume of the solvent).

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Percent Volume by Volume (v/v)

The volume of solute dissolved per 100 parts by volume of the solution. The volumes of solute and solvent might be equal to the solution's volume.

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Molarity (M)

The number of moles of solute dissolved per dm3 of solution. It's based on the solution's total volume, not just the solvent.

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Molality (m)

The number of moles of solute dissolved per kilogram of solvent.

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Normality (N)

A measure of the number of gram equivalent weights of solute in one liter of solution.

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Mole Fraction

The ratio of the number of moles of one component (solute or solvent) to the total number of moles in the solution.

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Ideal Solution

A solution where the solute and solvent have similar properties, resulting in no change in their individual properties upon mixing.

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Non-Ideal Solution

A solution formed by mixing substances with differing properties, resulting in changes in their individual properties upon mixing.

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Solution Concentration

The amount of solute present in a given amount of solvent or solution.

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Dilute Solution

A solution containing a relatively small amount of solute compared to its solvent.

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Concentrated Solution

A solution containing a relatively large amount of solute compared to its solvent.

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Solution Classification

The state of the solute and solvent in a solution, like gas, liquid, or solid.

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Homogeneous Solution

A type of solution where the solute is uniformly distributed throughout the solvent.

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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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Physical Pharmacy (II) - Solutions, Solubility, and Distribution Phenomena PDF

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.

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