Exp 12 FP depression
•Download as PPTX, PDF•
1 like•9,335 views
This document discusses freezing point depression and colligative properties. It defines key terms like molality, freezing point depression constant, and Van't Hoff factor. The goals are to determine the freezing point depression constant of water, examine the relationship between concentration and freezing point, and explore the effect of electrolytes. Students will prepare sugar solutions of varying concentration and one salt solution to compare the freezing point depression.
Report
Share
Report
Share
Recommended
Chapter 14.2 : Colligative Properties
Colligative properties depend on the concentration of solute particles but not their identity. The four main colligative properties are vapor pressure lowering, freezing point depression, boiling point elevation, and osmotic pressure. Freezing point depression and boiling point elevation are directly proportional to the molal concentration of the solution. Electrolytes enhance colligative properties because they dissociate into multiple ions in solution, effectively increasing the number of solute particles compared to nonelectrolytes of the same molar concentration.
colligative property ,made by-chinmay jagadev pattanayak
What is colligative property?
Types of colligative property
Lowering Vapour Pressure (∆P) of solutions.
Boiling point elevation.
Freezing point depression
Osmotic pressure of the solution
Chapter 13 Lecture on Solutions & Colligative Properties
The document summarizes key concepts about solutions from chapters 11-13, including:
- Solutions are homogeneous mixtures of two or more substances where the solute is uniformly dispersed in the solvent.
- Solubility is affected by intermolecular forces - "like dissolves like" with polar substances dissolving in polar solvents.
- Temperature and pressure can impact solubility, with solubility generally increasing with temperature and gas solubility directly proportional to pressure.
- There are various ways to express concentration, including molarity, molality, mole fraction, ppm, and mass percentage.
Colligative Properties Of Solutions
A presentation discussing the main colligative properties of solutions, applicable for high school chemistry or AP Chemistry
Solution of non electrolyte full
This document provides information on solutions of non-electrolytes. It defines key terms like solute, solvent, saturated solution, and supersaturated solution. It explains how a solution forms via a 3 step process of solute separation, solvent separation, and solute-solvent interaction. Various methods of expressing concentration are described, including mass percentage, parts per million/billion, mole fraction, molarity, molality, and normality. Raoult's law and its limitations are discussed. Real solutions that deviate positively or negatively from Raoult's law are explained. Henry's law relating gas solubility to partial pressure is also summarized.
Colligative properties, sifat koligatif
This document discusses colligative properties of solutions, specifically molality and mole fraction. Molality is defined as the number of moles of solute per kg of solvent. Mole fraction is the ratio of moles of solute or solvent to the total moles of solution. Several examples are provided to demonstrate how to calculate molality and mole fraction for different solutions. Practice problems are also included at the end to help reinforce understanding of these concepts.
Colligative properties ppt ssc,amt
Colligative properties of dilute solution is important topic of physical chemistry. mainly cover types with application of it day to day life... must to watch and share
Colligative Properties
Colligative properties depend only on the number of dissolved particles in solution and not on their identity. The key colligative properties are vapor pressure lowering, boiling point elevation, and freezing point depression. Vapor pressure lowering occurs because solute particles decrease the number of solvent particles that can evaporate from the surface. Boiling point elevation and freezing point depression occur because adding solute particles lowers the vapor pressure of the solvent, requiring more energy for evaporation or freezing. The degree of change in boiling point or freezing point depends on the molality of the solution.
Recommended
Chapter 14.2 : Colligative Properties
Colligative properties depend on the concentration of solute particles but not their identity. The four main colligative properties are vapor pressure lowering, freezing point depression, boiling point elevation, and osmotic pressure. Freezing point depression and boiling point elevation are directly proportional to the molal concentration of the solution. Electrolytes enhance colligative properties because they dissociate into multiple ions in solution, effectively increasing the number of solute particles compared to nonelectrolytes of the same molar concentration.
colligative property ,made by-chinmay jagadev pattanayak
What is colligative property?
Types of colligative property
Lowering Vapour Pressure (∆P) of solutions.
Boiling point elevation.
Freezing point depression
Osmotic pressure of the solution
Chapter 13 Lecture on Solutions & Colligative Properties
The document summarizes key concepts about solutions from chapters 11-13, including:
- Solutions are homogeneous mixtures of two or more substances where the solute is uniformly dispersed in the solvent.
- Solubility is affected by intermolecular forces - "like dissolves like" with polar substances dissolving in polar solvents.
- Temperature and pressure can impact solubility, with solubility generally increasing with temperature and gas solubility directly proportional to pressure.
- There are various ways to express concentration, including molarity, molality, mole fraction, ppm, and mass percentage.
Colligative Properties Of Solutions
A presentation discussing the main colligative properties of solutions, applicable for high school chemistry or AP Chemistry
Solution of non electrolyte full
This document provides information on solutions of non-electrolytes. It defines key terms like solute, solvent, saturated solution, and supersaturated solution. It explains how a solution forms via a 3 step process of solute separation, solvent separation, and solute-solvent interaction. Various methods of expressing concentration are described, including mass percentage, parts per million/billion, mole fraction, molarity, molality, and normality. Raoult's law and its limitations are discussed. Real solutions that deviate positively or negatively from Raoult's law are explained. Henry's law relating gas solubility to partial pressure is also summarized.
Colligative properties, sifat koligatif
This document discusses colligative properties of solutions, specifically molality and mole fraction. Molality is defined as the number of moles of solute per kg of solvent. Mole fraction is the ratio of moles of solute or solvent to the total moles of solution. Several examples are provided to demonstrate how to calculate molality and mole fraction for different solutions. Practice problems are also included at the end to help reinforce understanding of these concepts.
Colligative properties ppt ssc,amt
Colligative properties of dilute solution is important topic of physical chemistry. mainly cover types with application of it day to day life... must to watch and share
Colligative Properties
Colligative properties depend only on the number of dissolved particles in solution and not on their identity. The key colligative properties are vapor pressure lowering, boiling point elevation, and freezing point depression. Vapor pressure lowering occurs because solute particles decrease the number of solvent particles that can evaporate from the surface. Boiling point elevation and freezing point depression occur because adding solute particles lowers the vapor pressure of the solvent, requiring more energy for evaporation or freezing. The degree of change in boiling point or freezing point depends on the molality of the solution.
Solutions
Solutions are homogeneous mixtures formed when a solute dissolves in a solvent. For a solution to form, the solute and solvent molecules must interact favorably through intermolecular forces like ion-dipole interactions, hydrogen bonding, or dispersion forces. The solubility of a substance is affected by temperature, pressure, and how well the solute and solvent "like" each other. Solutions exhibit colligative properties like lowering of vapor pressure, boiling point elevation, and freezing point depression that depend only on the number of solute particles and not their identity. Osmosis occurs when a semipermeable membrane separates solutions of different solute concentrations, causing net water movement from the lower to higher concentration side.
Lecture 16.3- Colligative Properties
The document discusses colligative properties of solutions, including vapor pressure lowering, boiling point elevation, and freezing point depression. It explains that these properties depend on the number of dissolved particles in solution, regardless of particle type. Specifically, it states that the decrease in vapor pressure and increase in boiling point or freezing point depression is proportional to the number of particles formed by the solute in solution.
Chemistry project
This document provides information about solutions and their properties. It discusses several topics:
1. Electrolytes and non-electrolytes - Solutions that conduct electricity, like those containing ions, are electrolytes. Vinegar contains acetic acid which is only partially dissociated.
2. Electrolysis - Passing electricity through a solution can cause a chemical change, in a process called electrolysis. Electrolytic cells use an external energy source to drive nonspontaneous reactions.
3. Colligative properties - Properties like boiling point elevation and freezing point depression depend only on the amount of solute, not its identity. These include vapor pressure lowering, boiling point increase, freezing point depression, and
3 colligative properties
1. A solution is a homogeneous mixture of one or more solutes dissolved in a solvent. Solubility refers to the ability of a solute to dissolve in a solvent.
2. Henry's law states that the amount of gas that dissolves in a liquid is directly proportional to the partial pressure of the gas above the liquid at a constant temperature.
3. Colligative properties depend on the number of solute particles in solution, not their identity, and include vapor pressure lowering, boiling point elevation, freezing point depression, and osmotic pressure.
Raoults law 2nd assignment
Raoult's law states that the vapor pressure of a solution is directly proportional to the mole fraction of the solvent. It applies to ideal solutions and describes how the vapor pressure of a solution changes as the composition of the liquid changes. For ideal solutions, the vapor pressure decreases linearly as the mole fraction of the solvent decreases. However, real solutions often deviate from Raoult's law due to intermolecular forces. Colligative properties, such as lowering of vapor pressure, boiling point elevation, and freezing point depression, depend only on the number of solute particles and not their identity. These properties are used to determine molar masses of unknown solutes.
Solution%20presentation%20(1)[1]
This document discusses properties of solutions including:
- Types of solutions defined by the states of the solute and solvent.
- Terms used to describe solution composition such as dilute, concentrated, molarity, mass percent, mole fraction, and molality.
- Calculations showing how to determine the molarity, mass percent, mole fraction, and molality of a solution.
- The relationship between molarity and normality for acids and bases.
- Factors that influence solubility including entropy and the heat of solution formation.
colligative Properties MANIK
This document discusses colligative properties of dilute solutions. It defines colligative properties as properties that depend on the concentration of a solute but not its identity. The four main colligative properties are lowering of vapor pressure, elevation of boiling point, depression of freezing point, and osmotic pressure. The document provides detailed explanations and derivations of Raoult's law for vapor pressure lowering and boiling point elevation, freezing point depression, and Van't Hoff's law for osmotic pressure. It discusses how these colligative properties can be used to determine the molecular mass of solutes.
Colligative property
This document discusses colligative properties of solutions and ways of expressing concentration. It begins by defining key terms like solute, solvent, concentration, dilute and concentrated solutions. It then describes various ways of expressing concentration including percentage by weight, mole fraction, molarity, molality, normality and parts per million. The document also discusses colligative properties like lowering of vapor pressure, elevation of boiling point, depression of freezing point and osmotic pressure. It provides equations and experimental methods for determining these properties and using them to calculate molecular masses. The concept of abnormal molar masses from association or dissociation in solution is introduced along with the van't Hoff factor.
Colligative properties
colligative properties, solutions, vapor pressure, boiling and freezing point changes, osmotic pressure
Properties of solutions
1) Solutions are homogeneous mixtures of two or more substances, where the solute is dispersed uniformly throughout the solvent.
2) For a solution to form, the intermolecular forces between solute and solvent particles must be strong enough to overcome those within the pure substances.
3) The energetics of dissolving involves breaking interactions within the pure substances and forming new interactions between solute and solvent particles. Even endothermic processes can occur spontaneously if they increase the disorder or entropy of the system.
3- Solutions & It's Colligative Properties(Physical Pharmacy)
This document discusses various topics in physical pharmacy and solutions, including:
- Types of solutes such as electrolytes and non-electrolytes.
- Expressions used to quantify concentration in solutions such as molarity, molality, and mole fraction.
- Factors that influence vapor pressure, boiling point, and freezing point of solutions.
- The concept of ideal and real solutions in relation to Raoult's law and deviations from ideal behavior.
- Colligative properties of solutions that depend only on the number of solute particles, including vapor pressure lowering, boiling point elevation, freezing point depression, and osmotic pressure.
Colligative properties, 13(3)
Vapor pressure (of the solvent)
Freezing point depression
Boiling point elevation
Osmotic pressure
Solution
Solution , Types of Solutions,Raoult’s Law,Ideal and Non-Ideal Solutions,Colligative Properties, Abnormal Molecular Weight and Van't Hoff Factor
New chm 151_unit_14_power_points-su13
The document provides an overview of colligative properties of solutions, which are physical properties that depend on the number of solute particles in solution rather than the chemical identity of the solute. Examples of colligative properties discussed include vapor pressure lowering, boiling point elevation, freezing point depression, and osmotic pressure. Formulas are provided to calculate these colligative properties based on variables like molality, vapor pressure of the pure solvent, and temperature.
Presentation1
This document provides information and examples about various chemistry concepts related to concentration including molarity, molality, normality, milliequivalents, percent solutions, dilution, and serial dilution. It includes example calculations for determining the molarity of a sugar solution, molality of solutions, normality of solutions containing different numbers of equivalents, conversions between milligrams, millimoles and milliequivalents, percent weight by volume and weight by weight solutions, and calculations for single and serial dilutions.
AP Chemistry Chapter 13 Outline
The document discusses key concepts about solutions including:
1) Solutions are homogeneous mixtures of two or more substances where the solute is dispersed uniformly throughout the solvent.
2) For a solution to form, the intermolecular forces between solute and solvent particles must be strong enough to overcome interactions between pure components.
3) The enthalpy change of dissolving depends on the energy changes of separating solute and solvent particles and forming new interactions between them.
Experiment 9: Molecular Weight Determination using Freezing Point Depression
Just retrieved my files way back in my undergraduate days. Might as well share it.the purpose of this experiment is to determine the apparent molecular weight of the solute from the lowering of freezing point and to determine the extent of dimerization and dissociation of acetic acid in benzene
Solutions of nonelectrolytes-Physical Pharmacy
The document discusses various topics related to solutions of nonelectrolytes including:
1. Definitions of key terms like solute, solvent, concentration expressions and equivalent weights.
2. The differences between ideal and real solutions and how Raoult's law applies to ideal solutions. Real solutions can exhibit positive or negative deviations from Raoult's law.
3. Colligative properties which depend on the number of particles in a solution and include vapor pressure lowering, boiling point elevation, freezing point depression, and osmotic pressure.
LESSON-2.-CONCENTRATION-OF-SOLUTIONS.pdf
This document provides an overview of solutions and mixtures. It defines key terms like homogeneous and heterogeneous mixtures, solutes and solvents, concentration, and solubility. It also discusses different units used to measure concentration, including molarity, molality, and percent composition. Methods for separating mixtures like distillation, filtering, and chromatography are also outlined. The document provides examples of calculating concentration using various units and solving stoichiometric problems involving solutions.
New chm-151-unit-14-power-points-su13-140227172226-phpapp02
This document provides an overview of colligative properties and solutions. It begins with definitions of colligative properties, noting that they depend on the number of solute particles rather than their identity. Examples of colligative properties are given as vapor pressure lowering, boiling point elevation, freezing point depression, and osmotic pressure. The document then discusses each of these properties in more detail. Specific topics covered include how colligative properties are calculated using molality or molarity, data like freezing point depression constants for various solvents, and sample problems calculating values like boiling/freezing points of solutions. The last few pages shift to discussing colloids, providing definitions and examples of different types of colloids.
Solution_presentation.ppt
This document provides an overview of key concepts related to solutions and solution chemistry, including:
- Definitions of key terms like solution, solute, and solvent. Common states of solutions are discussed.
- Methods for describing solution concentration and composition, such as molarity, molality, mass percent, and mole fraction. The differences between molarity and molality are explained.
- Other solution concentration units like normality that are important for acids and bases are defined.
- Factors that determine solubility including entropy and the heat of solution are discussed. Entropy explains why NaCl dissolves in water despite the endothermic heat of solution.
- Different saturation states of solutions -
Mecchapter6 120814200155-phpapp01
This document summarizes key concepts about solutions from Chapter 6. It defines terms like solute, solvent, aqueous solutions, and discusses different types of solutions like liquids, solids, and gases. It then covers general properties of solutions like clarity and color. Specific topics discussed include concentration in terms of mass, moles, and equivalents. Colligative properties like vapor pressure, boiling point elevation, freezing point depression, and osmotic pressure are explained. The importance of water as a universal solvent is also highlighted.
More Related Content
What's hot
Solutions
Solutions are homogeneous mixtures formed when a solute dissolves in a solvent. For a solution to form, the solute and solvent molecules must interact favorably through intermolecular forces like ion-dipole interactions, hydrogen bonding, or dispersion forces. The solubility of a substance is affected by temperature, pressure, and how well the solute and solvent "like" each other. Solutions exhibit colligative properties like lowering of vapor pressure, boiling point elevation, and freezing point depression that depend only on the number of solute particles and not their identity. Osmosis occurs when a semipermeable membrane separates solutions of different solute concentrations, causing net water movement from the lower to higher concentration side.
Lecture 16.3- Colligative Properties
The document discusses colligative properties of solutions, including vapor pressure lowering, boiling point elevation, and freezing point depression. It explains that these properties depend on the number of dissolved particles in solution, regardless of particle type. Specifically, it states that the decrease in vapor pressure and increase in boiling point or freezing point depression is proportional to the number of particles formed by the solute in solution.
Chemistry project
This document provides information about solutions and their properties. It discusses several topics:
1. Electrolytes and non-electrolytes - Solutions that conduct electricity, like those containing ions, are electrolytes. Vinegar contains acetic acid which is only partially dissociated.
2. Electrolysis - Passing electricity through a solution can cause a chemical change, in a process called electrolysis. Electrolytic cells use an external energy source to drive nonspontaneous reactions.
3. Colligative properties - Properties like boiling point elevation and freezing point depression depend only on the amount of solute, not its identity. These include vapor pressure lowering, boiling point increase, freezing point depression, and
3 colligative properties
1. A solution is a homogeneous mixture of one or more solutes dissolved in a solvent. Solubility refers to the ability of a solute to dissolve in a solvent.
2. Henry's law states that the amount of gas that dissolves in a liquid is directly proportional to the partial pressure of the gas above the liquid at a constant temperature.
3. Colligative properties depend on the number of solute particles in solution, not their identity, and include vapor pressure lowering, boiling point elevation, freezing point depression, and osmotic pressure.
Raoults law 2nd assignment
Raoult's law states that the vapor pressure of a solution is directly proportional to the mole fraction of the solvent. It applies to ideal solutions and describes how the vapor pressure of a solution changes as the composition of the liquid changes. For ideal solutions, the vapor pressure decreases linearly as the mole fraction of the solvent decreases. However, real solutions often deviate from Raoult's law due to intermolecular forces. Colligative properties, such as lowering of vapor pressure, boiling point elevation, and freezing point depression, depend only on the number of solute particles and not their identity. These properties are used to determine molar masses of unknown solutes.
Solution%20presentation%20(1)[1]
This document discusses properties of solutions including:
- Types of solutions defined by the states of the solute and solvent.
- Terms used to describe solution composition such as dilute, concentrated, molarity, mass percent, mole fraction, and molality.
- Calculations showing how to determine the molarity, mass percent, mole fraction, and molality of a solution.
- The relationship between molarity and normality for acids and bases.
- Factors that influence solubility including entropy and the heat of solution formation.
colligative Properties MANIK
This document discusses colligative properties of dilute solutions. It defines colligative properties as properties that depend on the concentration of a solute but not its identity. The four main colligative properties are lowering of vapor pressure, elevation of boiling point, depression of freezing point, and osmotic pressure. The document provides detailed explanations and derivations of Raoult's law for vapor pressure lowering and boiling point elevation, freezing point depression, and Van't Hoff's law for osmotic pressure. It discusses how these colligative properties can be used to determine the molecular mass of solutes.
Colligative property
This document discusses colligative properties of solutions and ways of expressing concentration. It begins by defining key terms like solute, solvent, concentration, dilute and concentrated solutions. It then describes various ways of expressing concentration including percentage by weight, mole fraction, molarity, molality, normality and parts per million. The document also discusses colligative properties like lowering of vapor pressure, elevation of boiling point, depression of freezing point and osmotic pressure. It provides equations and experimental methods for determining these properties and using them to calculate molecular masses. The concept of abnormal molar masses from association or dissociation in solution is introduced along with the van't Hoff factor.
Colligative properties
colligative properties, solutions, vapor pressure, boiling and freezing point changes, osmotic pressure
Properties of solutions
1) Solutions are homogeneous mixtures of two or more substances, where the solute is dispersed uniformly throughout the solvent.
2) For a solution to form, the intermolecular forces between solute and solvent particles must be strong enough to overcome those within the pure substances.
3) The energetics of dissolving involves breaking interactions within the pure substances and forming new interactions between solute and solvent particles. Even endothermic processes can occur spontaneously if they increase the disorder or entropy of the system.
3- Solutions & It's Colligative Properties(Physical Pharmacy)
This document discusses various topics in physical pharmacy and solutions, including:
- Types of solutes such as electrolytes and non-electrolytes.
- Expressions used to quantify concentration in solutions such as molarity, molality, and mole fraction.
- Factors that influence vapor pressure, boiling point, and freezing point of solutions.
- The concept of ideal and real solutions in relation to Raoult's law and deviations from ideal behavior.
- Colligative properties of solutions that depend only on the number of solute particles, including vapor pressure lowering, boiling point elevation, freezing point depression, and osmotic pressure.
Colligative properties, 13(3)
Vapor pressure (of the solvent)
Freezing point depression
Boiling point elevation
Osmotic pressure
Solution
Solution , Types of Solutions,Raoult’s Law,Ideal and Non-Ideal Solutions,Colligative Properties, Abnormal Molecular Weight and Van't Hoff Factor
New chm 151_unit_14_power_points-su13
The document provides an overview of colligative properties of solutions, which are physical properties that depend on the number of solute particles in solution rather than the chemical identity of the solute. Examples of colligative properties discussed include vapor pressure lowering, boiling point elevation, freezing point depression, and osmotic pressure. Formulas are provided to calculate these colligative properties based on variables like molality, vapor pressure of the pure solvent, and temperature.
Presentation1
This document provides information and examples about various chemistry concepts related to concentration including molarity, molality, normality, milliequivalents, percent solutions, dilution, and serial dilution. It includes example calculations for determining the molarity of a sugar solution, molality of solutions, normality of solutions containing different numbers of equivalents, conversions between milligrams, millimoles and milliequivalents, percent weight by volume and weight by weight solutions, and calculations for single and serial dilutions.
AP Chemistry Chapter 13 Outline
The document discusses key concepts about solutions including:
1) Solutions are homogeneous mixtures of two or more substances where the solute is dispersed uniformly throughout the solvent.
2) For a solution to form, the intermolecular forces between solute and solvent particles must be strong enough to overcome interactions between pure components.
3) The enthalpy change of dissolving depends on the energy changes of separating solute and solvent particles and forming new interactions between them.
Experiment 9: Molecular Weight Determination using Freezing Point Depression
Just retrieved my files way back in my undergraduate days. Might as well share it.the purpose of this experiment is to determine the apparent molecular weight of the solute from the lowering of freezing point and to determine the extent of dimerization and dissociation of acetic acid in benzene
Solutions of nonelectrolytes-Physical Pharmacy
The document discusses various topics related to solutions of nonelectrolytes including:
1. Definitions of key terms like solute, solvent, concentration expressions and equivalent weights.
2. The differences between ideal and real solutions and how Raoult's law applies to ideal solutions. Real solutions can exhibit positive or negative deviations from Raoult's law.
3. Colligative properties which depend on the number of particles in a solution and include vapor pressure lowering, boiling point elevation, freezing point depression, and osmotic pressure.
What's hot (18)
3- Solutions & It's Colligative Properties(Physical Pharmacy)
3- Solutions & It's Colligative Properties(Physical Pharmacy)
Experiment 9: Molecular Weight Determination using Freezing Point Depression
Experiment 9: Molecular Weight Determination using Freezing Point Depression
Similar to Exp 12 FP depression
LESSON-2.-CONCENTRATION-OF-SOLUTIONS.pdf
This document provides an overview of solutions and mixtures. It defines key terms like homogeneous and heterogeneous mixtures, solutes and solvents, concentration, and solubility. It also discusses different units used to measure concentration, including molarity, molality, and percent composition. Methods for separating mixtures like distillation, filtering, and chromatography are also outlined. The document provides examples of calculating concentration using various units and solving stoichiometric problems involving solutions.
New chm-151-unit-14-power-points-su13-140227172226-phpapp02
This document provides an overview of colligative properties and solutions. It begins with definitions of colligative properties, noting that they depend on the number of solute particles rather than their identity. Examples of colligative properties are given as vapor pressure lowering, boiling point elevation, freezing point depression, and osmotic pressure. The document then discusses each of these properties in more detail. Specific topics covered include how colligative properties are calculated using molality or molarity, data like freezing point depression constants for various solvents, and sample problems calculating values like boiling/freezing points of solutions. The last few pages shift to discussing colloids, providing definitions and examples of different types of colloids.
Solution_presentation.ppt
This document provides an overview of key concepts related to solutions and solution chemistry, including:
- Definitions of key terms like solution, solute, and solvent. Common states of solutions are discussed.
- Methods for describing solution concentration and composition, such as molarity, molality, mass percent, and mole fraction. The differences between molarity and molality are explained.
- Other solution concentration units like normality that are important for acids and bases are defined.
- Factors that determine solubility including entropy and the heat of solution are discussed. Entropy explains why NaCl dissolves in water despite the endothermic heat of solution.
- Different saturation states of solutions -
Mecchapter6 120814200155-phpapp01
This document summarizes key concepts about solutions from Chapter 6. It defines terms like solute, solvent, aqueous solutions, and discusses different types of solutions like liquids, solids, and gases. It then covers general properties of solutions like clarity and color. Specific topics discussed include concentration in terms of mass, moles, and equivalents. Colligative properties like vapor pressure, boiling point elevation, freezing point depression, and osmotic pressure are explained. The importance of water as a universal solvent is also highlighted.
Chapter 13
This document discusses various topics relating to solutions, including:
- Solutions are homogeneous mixtures of two or more substances where the solute is uniformly dispersed throughout the solvent.
- For a solution to form, the intermolecular forces between solute and solvent particles must be strong enough to overcome those within the pure substances.
- The energy changes during solution formation depend on the enthalpy of separating solute and solvent particles and the new interactions between them.
- Solubility is affected by the similarity between solute and solvent intermolecular forces, temperature, and pressure.
- Colligative properties like boiling point elevation and freezing point depression depend only on the number of solute particles and can be
Colligative properties
Colligative properties such as boiling point elevation, freezing point depression, and osmotic pressure depend only on the number of solute particles in solution, not their identity. The document discusses these properties and how they are affected when solutes dissolve. It explains that boiling point is elevated and freezing point is depressed because solutes lower vapor pressure, requiring more energy for phase changes. Osmotic pressure arises from differences in solute concentration across a semipermeable membrane. The van't Hoff factor accounts for changes in observed properties when solutes dissociate or associate in solution.
Lab-Solution-Preperation-Guide-1.pdf
The document discusses the concept of molarity, which is defined as the number of moles of solute per liter of solution. It provides examples of how to calculate the mass of solute needed to make a solution of a given molarity and volume. The document also discusses how to dilute a more concentrated solution to a desired molarity and volume. Additional topics covered include percent solutions and how to convert between mass and volume percent. The remainder of the document provides recipes for making common laboratory solutions with given molarities.
CONCENTRATION OF SOLUTIONS
Here are the key steps to solve this problem:
1) Convert grams of NH3 to moles using molar mass (65.3 g / 17 g/mol = 3.83 mol NH3)
2) Use balanced equation to determine moles of other substances (3.83 mol NH3 x 4/1 = 15.32 mol NO)
3) Use heat of reaction and moles of limiting reactant to determine heat (ΔH = -904 kJ/mol NH3 x 3.83 mol NH3 = -3,459 kJ)
chem(xii) solution
This document provides information about solutions and their properties. It defines a solution as a homogeneous mixture of two or more substances and discusses the components of a solution - the solute and solvent. It then describes different types of solutions based on the states of the solute and solvent. The document also explains various methods of expressing the concentration of a solution, such as percentage, molarity, and ppm. It provides examples of calculating concentration. Finally, it discusses properties of solutions like solubility, Henry's law, and colligative properties.
Chemistry of solutions
This document discusses the chemistry of solutions, including:
- Solutions are formed when a solvent dissolves a solute through solvation. The amount of solute dissolved depends on temperature, pressure, and agitation.
- Solubility is the maximum amount of solute that can dissolve in a given solvent under certain conditions. Higher temperatures generally increase solubility for solid-liquid and gas-liquid solutions, while higher pressures increase gas solubility.
- Concentration refers to the proportion of solute in a solution and can be measured by various units including percentage, molarity, molality, and normality. Colligative properties like boiling point and freezing point depend on concentration.
Nyb F09 Unit 2 Slides 1 25
The document discusses colligative properties of solutions, which depend only on the number of solute particles and not their type. It describes how adding solute particles lowers vapor pressure and freezing point and raises boiling point of the solvent. Specifically, it provides equations to calculate boiling point elevation, freezing point depression, and osmotic pressure based on molality and van't Hoff factor of the solution.
Colligative_Properties_Notes.ppt
Colligative properties refer to how dissolving a solute into a solvent affects the solvent's physical properties. Specifically, it lowers the vapor pressure and freezing point and raises the boiling point. These effects are due to interactions between the solute particles and solvent molecules. The greater the number of solute particles, the larger the impact on the solvent's properties. This number depends on whether the solute is an electrolyte or non-electrolyte. Electrolytes dissociate into multiple ions in solution, whereas non-electrolytes remain intact molecules. The document provides examples of calculating the changes in boiling point and freezing point based on molality and other factors.
Roultes law
Raoult's law describes the behavior of ideal solutions. It states that the vapor pressure of a solution is proportional to the mole fraction of the solvent in the solution. The vapor pressure of a solution is lower than that of the pure solvent due to the presence of nonvolatile solute particles. This lowering of vapor pressure leads to boiling point elevation and freezing point depression in solutions, as described by the colligative properties. The quantitative relationships for boiling point elevation and freezing point depression involve the molal concentration of the solute.
Solution (Chemistry) MANIK
Solutions: types and properties of solutions. Units of concentration, ideal and real
solutions. Henry’s law, distribution of solids between two immiscible liquids, distribution
law. Partition coefficient and solvent extraction.
Apchemunit11presentation 120104190723-phpapp01
This solution exhibits nonideal behavior. Acetone and chloroform are both volatile liquids that contribute to the total vapor pressure. To determine if it is ideal or nonideal, we would need the individual vapor pressures of acetone and chloroform at 35°C and their mole fractions in order to use the modified Raoult's law equation and compare the calculated total pressure to the measured 260 torr.
Ap chem unit 11 presentation
This document discusses several topics related to solutions, including:
1. It defines solutions and describes ways to express concentration such as molarity, mass percent, and mole fraction.
2. It explains that the enthalpy of solution depends on the energies required to separate the solute, expand the solvent, and allow interactions between solute and solvent particles. The overall enthalpy can be endothermic or exothermic.
3. Factors that affect solubility include like dissolving like, pressure, temperature, and molecular structure. Henry's law relates the solubility of gases to pressure. Temperature can either increase or decrease solubility depending on the substances involved.
pavan1-180820113614.pptx
Colligative properties depend only on the number of solute particles and not their identity. They include vapor pressure lowering, boiling point elevation, freezing point depression, and osmotic pressure. The boiling point of a solution is higher than the pure solvent due to lowered vapor pressure when solutes are added. Boiling point elevation is directly proportional to the molal concentration of the solute. Freezing point is also depressed when solutes are added, with freezing point depression directly proportional to molality. Osmosis is the movement of the solvent through a semipermeable membrane from a region of lower to higher solute concentration.
Solution chemistry notes
This document provides information on solution chemistry and concepts including:
- Definitions of key terms like solution, solute, and solvent
- The process of dissolution where solvent molecules pull apart solute molecules
- How saturated, supersaturated and concentrated solutions are classified
- Factors that influence solubility like temperature, pressure and nature of solute
- Colligative properties of solutions like vapor pressure lowering, freezing point depression and boiling point elevation that depend on amount of solute.
- Equations to calculate values like molarity, molality and mole fraction in solutions.
Solutions and Colligative properties
The document discusses various topics related to solutions and colligative properties. It defines key terms like solute, solvent, concentration methods. It explains concepts such as Raoult's law, deviations from Raoult's law, ideal and non-ideal solutions. It also covers colligative properties including elevation in boiling point, depression in freezing point, osmotic pressure and lowering of vapour pressure. It discusses abnormal molecular masses that can arise from solute dissociation or association and how the van't Hoff factor can explain this.
molarity lesson quarter 3 science 7 pdf/file
The document discusses concentration of solutions and molarity. It defines molarity as the number of moles of solute dissolved in 1 liter of solution. It provides examples of calculating molarity based on moles of solute and volume of solution. It also discusses making dilute solutions by taking an initial volume of a concentrated stock solution and diluting it with solvent to a final volume. Dilution does not change the total moles of solute.
Similar to Exp 12 FP depression (20)
New chm-151-unit-14-power-points-su13-140227172226-phpapp02
New chm-151-unit-14-power-points-su13-140227172226-phpapp02
More from genchemlab
Academic offenses in Labs
This document outlines academic offenses and plagiarism policies for chemistry labs at the University of Kentucky. It defines plagiarism as using another's words or ideas without proper attribution. Examples of academic offenses include changing lab data, copying from others' work, sharing unauthorized materials during exams, and falsifying absences. Students must write lab reports individually and are prohibited from sharing work. Penalties for offenses include failing grades and academic misconduct records. The department takes all offenses seriously and will penalize any involved students according to university rules.
Exp 11 Enthalpy
Here are the steps to solve this problem using Hess's Law:
1) Write the balanced equation for the reaction of interest:
NO(g) + O(g) → NO2(g)
2) Identify the relevant standard enthalpy change reactions:
2O3(g) → 3O2(g) ΔH° = -427 kJ
O2(g) → 2O(g) ΔH° = +495 kJ
NO(g) + O3(g) → NO2(g) + O2(g) ΔH° = -199 kJ
3) Rearrange the equations to obtain the overall reaction:
2O
Calculations for Chemistry is pHun
This document provides instructions for students to complete pre-lab calculations to design a buffer solution for a chemistry lab experiment. It specifies that students must determine the acid/salt pair to use based on an assigned pH value between 1 and 8. It then outlines the calculations needed to determine the amounts of acid and salt to measure out, including molar concentrations and masses, using the dilution equation and Henderson-Hasselbalch formula. Students are reminded to show their work and have their calculations verified before starting the experiment.
16 buffers sp16
This document provides information about buffers and how to prepare a buffer solution in the laboratory. It defines a buffer as a solution that can maintain a constant pH level when small amounts of acid or base are added. Buffers are composed of an acid and its conjugate base. The key properties that should match the desired pH are the acid's pKa value and that its conjugate base only differs by one hydrogen ion. The document outlines how to calculate the mass of salt needed using the Henderson-Hasselbalch equation and dilute the acid solution, and describes various methods for measuring the pH of buffer solutions. It also defines buffer capacity and how it can be experimentally determined.
Calculationsforchemistryisphun
The document provides instructions for students to complete calculations to design a buffer of their assigned pH for a chemistry lab experiment. Students are told to use provided resources to determine the appropriate acid-salt pair to use based on the acid's pKa value relative to the assigned pH. They are then directed to use dilution equations to calculate amounts of acid and the Henderson-Hasselbalch equation to find the conjugate base concentration needed to achieve the target pH with their buffer.
16 solubility
The document provides instructions for an experiment to determine the solubility of calcium hydroxide. The experiment involves preparing a saturated calcium hydroxide solution, standardizing hydrochloric acid, and then titrating the calcium hydroxide solution with the standardized acid. Students are advised to review solubility and the solubility product constant (Ksp) in their textbook before setting up calculations involving Ksp. The titration will have two equivalence points but sometimes only one will be visible, and students are told to continue titrating until their data plateaus.
7-EnthalpyOfReaction
This document provides instructions on how to determine the enthalpy of a chemical reaction using calorimetry. Key points include:
1) Calorimetry involves measuring the temperature change of a reaction to calculate the heat released or absorbed.
2) Reactions can be exothermic (releasing heat) or endothermic (absorbing heat).
3) The enthalpy change (ΔH) of a reaction is an intensive property representing the heat of the reaction per mole.
4) Hess's law states that the enthalpy change of a reaction is independent of the pathway and can be determined from the sum of multiple steps.
15 buffers
Buffers maintain pH through small additions of acid or base and are composed of an acid and its conjugate base, with the pKa slightly above the desired pH. Dilutions can be calculated using the dilution formula of M1V1 = M2V2. The pH of solutions can be determined through litmus paper, pH paper, indicators, or a pH meter. Calculations must be completed and checked by the TA in advance of the experiment.
Calculations for chemistry_is_p_hun_
The document provides instructions for students to complete calculations to design a buffer of their assigned pH for a chemistry lab experiment. Students are told to use provided resources to determine the appropriate acid-salt pair, calculate concentrations and volumes of solutions needed, and show all work for their teaching assistant to verify before starting the experiment.
14 standardization&titration
Standardization and titration is a quantitative technique that can produce accurate and precise results when done carefully. It involves standardizing a sodium hydroxide (NaOH) solution by performing multiple titrations of a primary standard potassium hydrogen phthalate (KHP) of known molarity. This allows the determination of an unknown concentration of acetic acid by titrating samples with the standardized NaOH solution. Proper experimental procedure and tips are provided to complete the standardization and acetic acid titrations.
06 microscale titration_fa06
The document discusses acid-base titration, including the analyte, standard, neutralization reaction, equivalence point, and procedure. It explains that an acid-base titration involves titrating an acid with a base until the moles of H+ equal the moles of OH-. It also discusses using a pH sensor and indicator to determine the equivalence point, and using stoichiometry to calculate unknown concentrations from experimental data.
5-Ten Test Tube Mystery
This document describes Experiment 5 which tests 10 unknown solutions using precipitation reactions. Students will observe any solids formed and use these results along with solubility rules to identify each of the 10 solutions. The procedure instructs students to test each combination of solutions systematically and keep their lab organized. Tips are provided on washing equipment, handling odors, and making an organized data table and worksheet to document their results and identify each of the solutions based on at least two pieces of evidence from their experiments.
More from genchemlab (12)
Recently uploaded
BÀI TẬP BỔ TRỢ TIẾNG ANH 8 CẢ NĂM - GLOBAL SUCCESS - NĂM HỌC 2023-2024 (CÓ FI...
BÀI TẬP BỔ TRỢ TIẾNG ANH 8 CẢ NĂM - GLOBAL SUCCESS - NĂM HỌC 2023-2024 (CÓ FI...Nguyen Thanh Tu Collection
https://app.box.com/s/y977uz6bpd3af4qsebv7r9b7s21935vdHow to Setup Warehouse & Location in Odoo 17 Inventory
In this slide, we'll explore how to set up warehouses and locations in Odoo 17 Inventory. This will help us manage our stock effectively, track inventory levels, and streamline warehouse operations.
Walmart Business+ and Spark Good for Nonprofits.pdf
"Learn about all the ways Walmart supports nonprofit organizations.
You will hear from Liz Willett, the Head of Nonprofits, and hear about what Walmart is doing to help nonprofits, including Walmart Business and Spark Good. Walmart Business+ is a new offer for nonprofits that offers discounts and also streamlines nonprofits order and expense tracking, saving time and money.
The webinar may also give some examples on how nonprofits can best leverage Walmart Business+.
The event will cover the following::
Walmart Business + (https://business.walmart.com/plus) is a new shopping experience for nonprofits, schools, and local business customers that connects an exclusive online shopping experience to stores. Benefits include free delivery and shipping, a 'Spend Analytics” feature, special discounts, deals and tax-exempt shopping.
Special TechSoup offer for a free 180 days membership, and up to $150 in discounts on eligible orders.
Spark Good (walmart.com/sparkgood) is a charitable platform that enables nonprofits to receive donations directly from customers and associates.
Answers about how you can do more with Walmart!"
Pengantar Penggunaan Flutter - Dart programming language1.pptx
Pengantar Penggunaan Flutter - Dart programming language1.pptx
How to deliver Powerpoint Presentations.pptx
"How to make and deliver dynamic presentations by making it more interactive to captivate your audience attention"
ISO/IEC 27001, ISO/IEC 42001, and GDPR: Best Practices for Implementation and...
Denis is a dynamic and results-driven Chief Information Officer (CIO) with a distinguished career spanning information systems analysis and technical project management. With a proven track record of spearheading the design and delivery of cutting-edge Information Management solutions, he has consistently elevated business operations, streamlined reporting functions, and maximized process efficiency.
Certified as an ISO/IEC 27001: Information Security Management Systems (ISMS) Lead Implementer, Data Protection Officer, and Cyber Risks Analyst, Denis brings a heightened focus on data security, privacy, and cyber resilience to every endeavor.
His expertise extends across a diverse spectrum of reporting, database, and web development applications, underpinned by an exceptional grasp of data storage and virtualization technologies. His proficiency in application testing, database administration, and data cleansing ensures seamless execution of complex projects.
What sets Denis apart is his comprehensive understanding of Business and Systems Analysis technologies, honed through involvement in all phases of the Software Development Lifecycle (SDLC). From meticulous requirements gathering to precise analysis, innovative design, rigorous development, thorough testing, and successful implementation, he has consistently delivered exceptional results.
Throughout his career, he has taken on multifaceted roles, from leading technical project management teams to owning solutions that drive operational excellence. His conscientious and proactive approach is unwavering, whether he is working independently or collaboratively within a team. His ability to connect with colleagues on a personal level underscores his commitment to fostering a harmonious and productive workplace environment.
Date: May 29, 2024
Tags: Information Security, ISO/IEC 27001, ISO/IEC 42001, Artificial Intelligence, GDPR
-------------------------------------------------------------------------------
Find out more about ISO training and certification services
Training: ISO/IEC 27001 Information Security Management System - EN | PECB
ISO/IEC 42001 Artificial Intelligence Management System - EN | PECB
General Data Protection Regulation (GDPR) - Training Courses - EN | PECB
Webinars: https://pecb.com/webinars
Article: https://pecb.com/article
-------------------------------------------------------------------------------
For more information about PECB:
Website: https://pecb.com/
LinkedIn: https://www.linkedin.com/company/pecb/
Facebook: https://www.facebook.com/PECBInternational/
Slideshare: http://www.slideshare.net/PECBCERTIFICATION
Solutons Maths Escape Room Spatial .pptx
Solutions of Puzzles of Mathematics Escape Room Game in Spatial.io
Mule event processing models | MuleSoft Mysore Meetup #47
Mule event processing models | MuleSoft Mysore Meetup #47
Event Link:- https://meetups.mulesoft.com/events/details/mulesoft-mysore-presents-mule-event-processing-models/
Agenda
● What is event processing in MuleSoft?
● Types of event processing models in Mule 4
● Distinction between the reactive, parallel, blocking & non-blocking processing
For Upcoming Meetups Join Mysore Meetup Group - https://meetups.mulesoft.com/mysore/YouTube:- youtube.com/@mulesoftmysore
Mysore WhatsApp group:- https://chat.whatsapp.com/EhqtHtCC75vCAX7gaO842N
Speaker:-
Shivani Yasaswi - https://www.linkedin.com/in/shivaniyasaswi/
Organizers:-
Shubham Chaurasia - https://www.linkedin.com/in/shubhamchaurasia1/
Giridhar Meka - https://www.linkedin.com/in/giridharmeka
Priya Shaw - https://www.linkedin.com/in/priya-shaw
Main Java[All of the Base Concepts}.docx
This is part 1 of my Java Learning Journey. This Contains Custom methods, classes, constructors, packages, multithreading , try- catch block, finally block and more.
Hindi varnamala | hindi alphabet PPT.pdf
हिंदी वर्णमाला पीपीटी, hindi alphabet PPT presentation, hindi varnamala PPT, Hindi Varnamala pdf, हिंदी स्वर, हिंदी व्यंजन, sikhiye hindi varnmala, dr. mulla adam ali, hindi language and literature, hindi alphabet with drawing, hindi alphabet pdf, hindi varnamala for childrens, hindi language, hindi varnamala practice for kids, https://www.drmullaadamali.com
clinical examination of hip joint (1).pdf
described clinical examination all orthopeadic conditions .
Beyond Degrees - Empowering the Workforce in the Context of Skills-First.pptx
Iván Bornacelly, Policy Analyst at the OECD Centre for Skills, OECD, presents at the webinar 'Tackling job market gaps with a skills-first approach' on 12 June 2024
ANATOMY AND BIOMECHANICS OF HIP JOINT.pdf
it describes the bony anatomy including the femoral head , acetabulum, labrum . also discusses the capsule , ligaments . muscle that act on the hip joint and the range of motion are outlined. factors affecting hip joint stability and weight transmission through the joint are summarized.
Chapter wise All Notes of First year Basic Civil Engineering.pptx
Chapter wise All Notes of First year Basic Civil Engineering
Syllabus
Chapter-1
Introduction to objective, scope and outcome the subject
Chapter 2
Introduction: Scope and Specialization of Civil Engineering, Role of civil Engineer in Society, Impact of infrastructural development on economy of country.
Chapter 3
Surveying: Object Principles & Types of Surveying; Site Plans, Plans & Maps; Scales & Unit of different Measurements.
Linear Measurements: Instruments used. Linear Measurement by Tape, Ranging out Survey Lines and overcoming Obstructions; Measurements on sloping ground; Tape corrections, conventional symbols. Angular Measurements: Instruments used; Introduction to Compass Surveying, Bearings and Longitude & Latitude of a Line, Introduction to total station.
Levelling: Instrument used Object of levelling, Methods of levelling in brief, and Contour maps.
Chapter 4
Buildings: Selection of site for Buildings, Layout of Building Plan, Types of buildings, Plinth area, carpet area, floor space index, Introduction to building byelaws, concept of sun light & ventilation. Components of Buildings & their functions, Basic concept of R.C.C., Introduction to types of foundation
Chapter 5
Transportation: Introduction to Transportation Engineering; Traffic and Road Safety: Types and Characteristics of Various Modes of Transportation; Various Road Traffic Signs, Causes of Accidents and Road Safety Measures.
Chapter 6
Environmental Engineering: Environmental Pollution, Environmental Acts and Regulations, Functional Concepts of Ecology, Basics of Species, Biodiversity, Ecosystem, Hydrological Cycle; Chemical Cycles: Carbon, Nitrogen & Phosphorus; Energy Flow in Ecosystems.
Water Pollution: Water Quality standards, Introduction to Treatment & Disposal of Waste Water. Reuse and Saving of Water, Rain Water Harvesting. Solid Waste Management: Classification of Solid Waste, Collection, Transportation and Disposal of Solid. Recycling of Solid Waste: Energy Recovery, Sanitary Landfill, On-Site Sanitation. Air & Noise Pollution: Primary and Secondary air pollutants, Harmful effects of Air Pollution, Control of Air Pollution. . Noise Pollution Harmful Effects of noise pollution, control of noise pollution, Global warming & Climate Change, Ozone depletion, Greenhouse effect
Text Books:
1. Palancharmy, Basic Civil Engineering, McGraw Hill publishers.
2. Satheesh Gopi, Basic Civil Engineering, Pearson Publishers.
3. Ketki Rangwala Dalal, Essentials of Civil Engineering, Charotar Publishing House.
4. BCP, Surveying volume 1
Recently uploaded (20)
BÀI TẬP BỔ TRỢ TIẾNG ANH 8 CẢ NĂM - GLOBAL SUCCESS - NĂM HỌC 2023-2024 (CÓ FI...
BÀI TẬP BỔ TRỢ TIẾNG ANH 8 CẢ NĂM - GLOBAL SUCCESS - NĂM HỌC 2023-2024 (CÓ FI...
IGCSE Biology Chapter 14- Reproduction in Plants.pdf
IGCSE Biology Chapter 14- Reproduction in Plants.pdf
How to Setup Warehouse & Location in Odoo 17 Inventory
How to Setup Warehouse & Location in Odoo 17 Inventory
Walmart Business+ and Spark Good for Nonprofits.pdf
Walmart Business+ and Spark Good for Nonprofits.pdf
Pengantar Penggunaan Flutter - Dart programming language1.pptx
Pengantar Penggunaan Flutter - Dart programming language1.pptx
ISO/IEC 27001, ISO/IEC 42001, and GDPR: Best Practices for Implementation and...
ISO/IEC 27001, ISO/IEC 42001, and GDPR: Best Practices for Implementation and...
Mule event processing models | MuleSoft Mysore Meetup #47
Mule event processing models | MuleSoft Mysore Meetup #47
B. Ed Syllabus for babasaheb ambedkar education university.pdf
B. Ed Syllabus for babasaheb ambedkar education university.pdf
Liberal Approach to the Study of Indian Politics.pdf
Liberal Approach to the Study of Indian Politics.pdf
Beyond Degrees - Empowering the Workforce in the Context of Skills-First.pptx
Beyond Degrees - Empowering the Workforce in the Context of Skills-First.pptx
Chapter wise All Notes of First year Basic Civil Engineering.pptx
Chapter wise All Notes of First year Basic Civil Engineering.pptx
Exp 12 FP depression
- 1. Freezing Point Depression General Chemistry Laboratory
- 2. Goals • To determine the freezing point depression constant of water • To determine the relationship between concentration and freezing point • To explore the effect of electrolytes on the freezing point of a solution
- 3. Colligative Properties • Properties that depend on the number of dissolved particles (aka concentration) present in the solution • What is the effect of increased concentration on BP and FP?
- 4. Molality (m) 𝑚 = moles of solute kg of solvent Example: What is the molality (MW = 180.16 g/mol) of a glucose solution containing 50 g glucose in 100 mL of water?
- 5. Freezing Point Depression Relationship between freezing point and molality: ΔT = iKfm ΔT: Change in temperature from the pure solvent’s original freezing point i: Van’t Hoff Factor Kf: Freezing Point Depression Constant
- 6. Van’t Hoff Factor (i) • The ratio of solute particles to the number of the formula units dissolved 𝑖 = 𝑚𝑜𝑙𝑒𝑠 𝑜𝑓 𝑝𝑎𝑟𝑡𝑖𝑐𝑙𝑒𝑠 𝑖𝑛 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛 𝑚𝑜𝑙𝑒𝑠 𝑜𝑓 𝑓𝑜𝑟𝑚𝑢𝑙𝑎 𝑢𝑛𝑖𝑡𝑠 𝑑𝑖𝑠𝑠𝑜𝑙𝑣𝑒𝑑 • Electrolyes break up into ions in solution • Nonelectrolytes do not yield ions when dissolved
- 7. Example – Glucose, C6H12O6 – Magnesium chloride, MgCl2
- 8. Procedural Hints • Sucrose is very soluble in water, approx. 2 g/mL • Prepare at least 4 sugar solutions of varying concentration (max conc. <0.5 g/mL) • Solutions should be between 100 and 200 mL • One salt solution should be prepared with equal molality to one of the sugar solutions
- 9. Interpreting Your Data • Interpreting these graphs will be on your exams.
- 10. Waste Disposal • Solids trash can • Liquids sink • Dry ice sink • Brush off the balances when you are done weighing your sample. • Weigh boats should be put in the trash after use.
Editor's Notes
- Glucose is a nonelectrolyte, so does not form ions in solution. Magnesium chloride is an electrolyte. It breaks apart into Mg2+ and Cl- ions, thus its van’t Hoff factor is 3.