Pharmacy Program: States of Matter (Lecture 6)
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Questions and Answers

Which of the following pairs of liquids are completely immiscible?

  • Phenol and water
  • Water and ether
  • Water and benzene (correct)
  • Water and alcohol

What happens when equal volumes of two partially miscible liquids, such as phenol and water, are mixed?

  • They completely mix to form a single layer.
  • They react and produce a gas.
  • They form two layers. (correct)
  • Only one liquid dissolves completely.

What best describes a substance in chemistry?

  • A mixture of different materials
  • A combination of solids and liquids
  • Matter with uniform and definite composition (correct)
  • Any physical property of a material

Which of the following is not a physical property of a substance?

<p>Reactivity with acid (B)</p> Signup and view all the answers

In which case would the degree of miscibility increase with temperature?

<p>Phenol-Water system (D)</p> Signup and view all the answers

How do liquids behave in terms of shape and volume?

<p>They take the shape of their container and have a constant volume (A)</p> Signup and view all the answers

What describes the graphical representation of the temperature versus composition relationship in miscible systems?

<p>Phase diagrams (A)</p> Signup and view all the answers

What is the outcome of adding excess phenol to a solution of phenol in water?

<p>Formation of a saturated solution (D)</p> Signup and view all the answers

Which state of matter is characterized by particles that are spaced far apart and easily compressed?

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

What is one of the two states of matter that is commonly not taught in high school physics?

<p>Bose-Einstein Condensate (A)</p> Signup and view all the answers

Which of the following correctly defines a saturated solution?

<p>Contains the maximum amount of solute that can dissolve in a solvent at a specific temperature. (B)</p> Signup and view all the answers

What is the term used for the component present in a smaller amount in a solution?

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

Which characteristic is true for solids?

<p>Are incompressible and have a definite shape (C)</p> Signup and view all the answers

When comparing solids, liquids, and gases, which statement is accurate?

<p>Gases occupy the volume of their container (C)</p> Signup and view all the answers

How can you describe a solution that contains less solute than it can dissolve?

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

Which of the following properties is observed without changing the substance’s composition?

<p>Melting point (B)</p> Signup and view all the answers

A solution with a concentration of 1 mole of solute in 1 liter of solution is referred to as what?

<p>Molarity (B)</p> Signup and view all the answers

Which of the following solutions involves a liquid solute in a solid solvent?

<p>Dental amalgam filling (B)</p> Signup and view all the answers

What is the relationship between the density of a solution and its mass and volume?

<p>Density = Mass / Volume (D)</p> Signup and view all the answers

Electrolytes in solutions are characterized by what key feature?

<p>They dissociate into ions when dissolved. (A)</p> Signup and view all the answers

Which method is NOT suitable for calculating the concentration of a solution?

<p>Title of substance (D)</p> Signup and view all the answers

What is the formula for calculating mass per volume percent (% W/V)?

<p>Mass of solute / Total volume of solution x 100 (D)</p> Signup and view all the answers

What does the sum of mole fractions in a solution equal?

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

How is molarity (M) defined?

<p>No. of moles of solute per liter of solution (C)</p> Signup and view all the answers

What is normality (N) primarily concerned with?

<p>Gram equivalents of solute per liter of solution (C)</p> Signup and view all the answers

What principle describes the total pressure in a mixture of non-reacting gases?

<p>Total pressure is the sum of partial pressures (A)</p> Signup and view all the answers

What does molality (m) measure?

<p>Moles of solute per kg of solvent (C)</p> Signup and view all the answers

In gaseous solutions, what happens when gases do not chemically react?

<p>They form a completely homogeneous solution (B)</p> Signup and view all the answers

What is the unit for molarity (M)?

<p>Mol/liter or M (B)</p> Signup and view all the answers

Flashcards

What is a substance?

A substance has a uniform and definite composition, meaning it is made of only one type of matter. All samples of a substance have the same physical properties.

What are physical properties?

Physical properties describe a substance's characteristics that can be observed or measured without changing the substance's composition.

What are some examples of physical properties?

Examples of physical properties include color, solubility, odor, hardness, density, melting point, and boiling point.

What are the three states of matter?

The three common states of matter are solid, liquid, and gas. These states are defined by how tightly packed the particles are and how much they move around.

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What is a solid?

A solid has a definite shape and volume. Its particles are tightly packed and almost incompressible. They expand slightly when heated.

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What is a liquid?

A liquid takes the shape of its container and flows. Its particles are close together but not rigid. It has a constant volume and expands slightly when heated.

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What is a gas?

A gas takes the shape and volume of its container and flows easily. Its particles are spread far apart and are easily compressed. It expands without limit to fill any space.

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What is plasma?

Plasma is a superheated gas where some electrons are stripped from the atoms, resulting in a very hot, electrically charged state.

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Miscibility

The ability of two liquids to dissolve in each other. Liquids can be completely miscible, partially miscible, or immiscible.

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Completely Miscible Liquids

Liquids that dissolve in each other in any proportion. They form a single homogeneous solution.

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Partially Miscible Liquids

Liquids that only dissolve in each other to a certain extent. They form two separate liquid layers when shaken together.

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Conjugate Solutions

The two separate liquid layers formed when partially miscible liquids are shaken together.

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Effect of Temperature on Miscibility

The degree of miscibility between liquids can be affected by temperature. Some liquid pairs become more miscible with increasing temperature, while others become less miscible.

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Mass per volume percent (% W/V)

The mass of solute divided by the total volume of the solution, multiplied by 100. It expresses the concentration of a solution by indicating the grams of solute per 100 mL of solution.

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Mole Fraction (XA)

The number of moles of a component (A) divided by the total number of moles of all components in the solution. It represents the fraction of the moles of a component in the mixture.

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Molarity (M)

The number of moles of solute per liter of solution. It measures the concentration of a solution in terms of the amount of solute dissolved in a specific volume.

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Molality (m)

The number of moles of solute per kilogram of solvent. It expresses the concentration of a solution in terms of the amount of solute dissolved in a specific mass of solvent.

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Normality (N)

The number of gram equivalents of solute per liter of solution. It represents the concentration of a solution in terms of the reactive capacity of the solute.

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Gram Equivalent

The weight of a substance that reacts with or replaces one mole of hydrogen ions (H+) or hydroxide ions (OH-) in a chemical reaction.

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Dalton's Law of Partial Pressures

The total pressure exerted by a mixture of non-reacting gases is equivalent to the sum of the partial pressures of the individual gases.

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Properties of Gaseous Solutions

Gaseous solutions are completely homogeneous (miscible), do not react chemically, and obey Dalton's Law of Partial Pressures. The properties of the mixture are the sum of the properties of the individual components.

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Liquid Crystals

Substances that exhibit properties of both liquids and solids, flowing like liquids but possessing optical and other characteristics of crystals.

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Solution

A homogeneous mixture of two or more substances, where one substance (solute) is dissolved in another (solvent).

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Solute

The component present in a smaller amount in a solution.

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Solvent

The component present in a larger amount in a solution, usually causing the solute to dissolve.

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Concentration

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

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Types of Solutions (Based on Saturation)

Solutions can be classified by their ability to dissolve more solute. Unsaturated solutions have room for more solute, saturated solutions are at their maximum solute capacity, and supersaturated solutions have exceeded that capacity and may precipitate.

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Electrolyte vs. Nonelectrolyte Solution

Electrolyte solutions conduct electricity because they contain dissolved ions. Nonelectrolyte solutions do not contain ions and cannot conduct electricity.

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Percent by Weight (% W/W)

A way to express concentration, defined as the weight of the solute divided by the total weight of the solution, multiplied by 100%.

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Study Notes

Field of Pharmacy Sciences

  • Bachelor of Pharmacy-PharmD (Clinical Pharmacy) Program
  • Pharmaceutical Inorganic & Physical Chemistry (PMC101)
  • Lecture 6: States of Matter and Solutions
  • Instructor: Dr. Amir Shaaban Farag
  • Date: Nov/20/2024

States of Matter

  • A substance has a uniform and definite composition
  • Substances contain only one kind of matter
  • All samples of a substance have the same physical properties

Physical Properties

  • Observable or measurable without changing composition
  • Examples: color, solubility, odor, hardness, density, melting point, boiling point
  • Help chemists identify substances based on characteristics

States of Matter: Properties

Property Solid Liquid Gas/Vapor
Shape Definite Indefinite Indefinite
Volume Definite Definite Indefinite
Expansion on heating Very slight Moderate Great
Compressibility Almost incompressible Almost incompressible Readily compressible

Solids, Liquids, and Gases

  • Solids*

  • Definite shape and volume

  • Shape independent of container

  • Particles tightly packed, almost incompressible

  • Expand slightly when heated

  • Liquids*

  • Take the shape of their container (flow)

  • Particles closely packed, but not rigidly

  • Volume constant, regardless of shape

  • Almost incompressible, tend to expand when heated

  • Gases*

  • Take the shape and form of their container (flowable)

  • Particles spaced far apart

  • Expand without limit to fill any space

  • Easily compressed

Some Characteristics of Solids, Liquids, and Gases

Property Gas Liquid Solid
Shape Assumes container Assumes container Definite
Volume Indefinite Definite Definite
Compressibility High Low Low
Flow Flows easily Flows easily Does not flow
Particle movement Particles move past each other Particles can move but also slide past each other Particles are in fixed positions

Phase Changes

  • Processes where matter transitions between solid, liquid, and gas states.
  • Melting, Freezing, Vaporization, Condensation, Sublimation, Deposition
  • Diagram showing phase changes and phase diagrams
  • Critical point
  • Triple point

Solutions

  • Mixtures of two or more chemically non-reactive substances
  • Most chemical reactions occur in solutions
  • Body fluids (like blood) are solutions
  • Homogenous or heterogenous
    • Homogenous - solute is uniformly distributed throughout solvent
    • Heterogenous- varies depending on size of particles

Classifying Solutions

  • Physical state: Based on the physical states of the solute and solvent (e.g., gas in a gas, liquid in liquid)
  • Unsaturated/Saturated/Supersaturated: (based on the ability of the solvent to dissolve more solute)
  • Concentration (dilute/concentrated): based on the ratio of solute to solvent
  • Miscible/Immiscible: Liquids that mix completely (miscible), or do not mix (immiscible)
  • Electrolyte/Nonelectrolyte: based on whether the solution conducts electricity (electrolyte) or not (nonelectrolyte)

Types of Solutions (1-Physical state)

  • Solutions are classified by the original state of the solute and the solvent (gas, liquid, or solid)
  • Several examples given in the slide

(2- Degree of saturation)

  • Unsaturated: Contains less solute than its capacity to dissolve
  • Saturated: Contains maximum solute at a specific temperature
  • Supersaturated: Contains more solute than a saturated solution

(3-Concentration)

  • Concentrated: High ratio of solute to solvent(e.g.,maple syrup, high salt solution)
  • Dilute: Low ratio of solute to solvent (e.g., a few sugar crystals in water)

(4-MISCIBILITY)

  • Miscible: liquids which are soluble in each other (e.g. ethanol and water)
  • Immiscible: liquids which are not soluble in each other (e.g. oil and water)

(5-Electrolytes and non electrolytes)

  • Electrolytes: dissolve in water to form solutions that conduct electricity
  • Nonelectrolytes: dissolve in water but do not conduct electricity
  • Examples of strong, weak, and non-electrolytes are given in the lecture

Different Units for Expressing Concentrations of Solutions

  • Percent by weight
  • Percent by volume
  • Mass per volume percent
  • Mole fraction
  • Molarity
  • Molality
  • Normality
  • equations for percent by weight, percent by volume

Solutions of Gases in Gases

  • Completely homogenous (miscible).
  • No chemical reaction between components.
  • Dalton's partial pressure law applies, where total pressure equals sum of partial pressures of the individual gases.

Solutions of Liquids in Liquids

  • Completely miscible: liquids which are soluble in each other at all proportions. Ex: alcohol and water.
  • Partially miscible: liquids which are soluble in each other, but only up to a limited concentration. Ex: water and ether
  • Completely immiscible: liquids which are insoluble in each other. Ex: water and benzene
  • Relationship between properties of liquids and miscibility

Effect of Temperature on Miscibility

  • Some systems show increased miscibility with rising temp
  • Some systems show decreased miscibility with rising temp
  • Some systems have upper and lower consolute temperatures.
  • Effects are shown using phase diagrams (graphs of Temperature vs Composition at constant pressure).

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States of Matters and Solutions Lecture Notes PDF

Description

This quiz focuses on the states of matter and solutions as part of the Pharmaceutical Inorganic & Physical Chemistry course. It covers key physical properties of substances, including their characteristics and how they help in identifying different types of matter. Ideal for students in the Bachelor of Pharmacy-PharmD program.

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