2nd Lecture on Solutions | Chemistry Part I | 12th Science
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This document summarizes key concepts about colligative properties of nonelectrolyte solutions. It discusses four colligative properties - vapor pressure lowering, boiling point elevation, freezing point depression, and osmotic pressure. Specifically, it explains how vapor pressure lowering depends on the number of solute particles in solution according to Raoult's law. It also describes how the boiling point of a solution is higher than that of the pure solvent due to vapor pressure lowering. Furthermore, it provides equations to calculate the molar mass of a solute using vapor pressure lowering or boiling point elevation measurements.
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RAOULT'S LAW ( Physical & Analytical Chemistry)
Name; Hasnain Nawaz
Surname : Shaikh
ROLL NO: 16 CH 42
B.E: Chemical Engineering (In Progress).
Mehran University of Engineering and Technology
Jamshore, ISO 9001 Certified.
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
Solution , Types of Solutions,Raoult’s Law,Ideal and Non-Ideal Solutions,Colligative Properties, Abnormal Molecular Weight and Van't Hoff Factor
Solutions CH02 12th NCERT chemistry notes
Solutions are homogeneous mixtures of two or more components. Key characteristics of solutions include concentration, vapor pressure, boiling point, freezing point, and osmotic pressure. Concentration, vapor pressure, boiling point elevation, freezing point depression, and osmotic pressure are colligative properties that depend only on the number of solute particles and not their identity. Deviations from ideal behavior are classified as positive or negative. Solutions can form azeotropes with unique boiling points.
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.
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.
CBSE Class 12 Chemistry Chapter 2 (Solutions) | Homi Institute
1) The solubility of solids in liquids is significantly affected by temperature changes, with solubility generally increasing as temperature decreases. Pressure does not significantly impact solubility.
2) According to Dalton's law of partial pressures, the total vapor pressure over a solution is equal to the sum of the partial pressures of the individual components in the solution.
3) Solutions can be classified as ideal or non-ideal based on whether they obey Raoult's law. Ideal solutions have zero enthalpy and volume changes upon mixing and the vapor pressure decreases linearly with changes in mole fractions.
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.
Recommended
RAOULT'S LAW ( Physical & Analytical Chemistry)
Name; Hasnain Nawaz
Surname : Shaikh
ROLL NO: 16 CH 42
B.E: Chemical Engineering (In Progress).
Mehran University of Engineering and Technology
Jamshore, ISO 9001 Certified.
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
Solution , Types of Solutions,Raoult’s Law,Ideal and Non-Ideal Solutions,Colligative Properties, Abnormal Molecular Weight and Van't Hoff Factor
Solutions CH02 12th NCERT chemistry notes
Solutions are homogeneous mixtures of two or more components. Key characteristics of solutions include concentration, vapor pressure, boiling point, freezing point, and osmotic pressure. Concentration, vapor pressure, boiling point elevation, freezing point depression, and osmotic pressure are colligative properties that depend only on the number of solute particles and not their identity. Deviations from ideal behavior are classified as positive or negative. Solutions can form azeotropes with unique boiling points.
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.
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.
CBSE Class 12 Chemistry Chapter 2 (Solutions) | Homi Institute
1) The solubility of solids in liquids is significantly affected by temperature changes, with solubility generally increasing as temperature decreases. Pressure does not significantly impact solubility.
2) According to Dalton's law of partial pressures, the total vapor pressure over a solution is equal to the sum of the partial pressures of the individual components in the solution.
3) Solutions can be classified as ideal or non-ideal based on whether they obey Raoult's law. Ideal solutions have zero enthalpy and volume changes upon mixing and the vapor pressure decreases linearly with changes in mole fractions.
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.
solutions state chemistry for class xii-
1. Solutions are homogeneous mixtures of two or more components, where the component present in smaller amounts is called the solute and the primary liquid component is the solvent.
2. Solutes can be electrolytes, which dissociate into ions, or nonelectrolytes, which do not dissociate. Common methods to express the concentration of solutions include molarity, molality, mole fraction, and percent composition.
3. The solubility of solids in liquids and gases in liquids depends on factors like temperature, pressure, and the nature of the solute and solvent. Henry's law and Raoult's law describe gas solubility and vapor pressure lowering in solutions. Ideal solutions follow
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
Ideal solution and non ideal solution
This document discusses ideal gases, Raoult's law, ideal solutions, and deviations from Raoult's law. It explains that an ideal gas is composed of randomly moving particles that only interact during elastic collisions. Raoult's law describes ideal solutions. Non-ideal solutions show either positive or negative deviations from Raoult's law due to differences in intermolecular forces between solvent-solute and pure components. Positive deviations occur when these interactions are weaker, while negative deviations occur when they are stronger.
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.
Colligative properties of dilute solutions Manik
lowering of vapour pressure, elevation of boiling point, depression of freezing point and osmotic pressure including necessary thermodynamic derivations.
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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.
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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.
Binary liquids
This document provides an overview of binary liquid systems, including vapor pressure, Raoult's law, ideal and non-ideal solutions, solubility of liquids in liquids, and the lever rule. It discusses how vapor pressure works for solids and liquids and introduces Raoult's law, which states that the vapor pressure of a solution decreases based on the mole fraction of the solute. Ideal solutions obey Raoult's law while real solutions can show positive or negative deviations. Positive deviations occur when interactions between like molecules are stronger, while negative deviations occur when interactions between unlike molecules are stronger. The document also covers the different types of solubility between liquids and uses the lever rule to determine the composition and amount of each phase
Colligative Properties III
This document discusses colligative properties, which are physical properties of solutions that depend only on the ratio of solute to solvent particles and not the identity of the solute. It describes four colligative properties: boiling point elevation, freezing point depression, vapor pressure lowering, and osmotic pressure. It explains how adding a nonvolatile solute affects the phase diagram by shifting the freezing point downward and boiling point upward. Formulas are provided to calculate changes in boiling point and freezing point based on molality. Raoult's Law is introduced to explain how vapor pressure of a solution depends on the mole fraction of the solvent. Osmotic pressure is defined as the pressure required to prevent solvent flow across a semiperme
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.
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.
Soluion and colligative propertries 2017
it is based on CBSE, ICSE, HSC ,JEE, NEET, AIPMT, MTCET.
class 12 chemistry.
for buy ppt pay by paytm acount- 8879919898. price-Rs99 only/-
for more detail go my site
www.akchem.blogspot.com
Solution chemistry
The document discusses solutions and solution chemistry. It begins by defining solutions as homogeneous mixtures of two or more pure substances, with the solute dispersed uniformly throughout the solvent. It then discusses how solutions form and the energy changes that occur, including the enthalpy changes of separating solute and solvent particles and forming new interactions between them. The rest of the document discusses various factors that affect solubility, such as the nature of the solute and solvent, intermolecular forces, temperature, and pressure. It also covers colligative properties of solutions like vapor pressure lowering, boiling point elevation, freezing point depression, and osmotic pressure.
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.
Colligative Properties Of Solutions
A presentation discussing the main colligative properties of solutions, applicable for high school chemistry or AP Chemistry
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.
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.
Solution and colligative properties
I hope You all like it. I hope It is very beneficial for you all. I really thought that you all get enough knowledge from this presentation. This presentation is about materials and their classifications. After you read this presentation you knowledge is not as before.
3rd Lecture on Solutions | Chemistry Part I | 12th Science
This document discusses colligative properties of solutions such as freezing point depression, boiling point elevation, and osmotic pressure. It explains that these properties are affected by the number of particles in solution. For electrolyte solutions, the properties are greater than nonelectrolyte solutions of the same concentration due to dissociation of ions. The document also defines terms like isotonic, hypertonic, and hypotonic solutions and introduces the Van't Hoff factor to relate colligative properties of electrolytes to their degree of dissociation.
chem2.pptx
Anshuman Singh, a class 12 student, has completed a school project on the topic of "colligative properties" under the guidance of his chemistry teacher, Mr. Sandeep Sharma. The project analyzes colligative properties such as lowering of vapor pressure, boiling point elevation, freezing point depression, and osmotic pressure. It discusses how these properties depend on the concentration of solute particles rather than their identity and defines the mathematical relationships between concentration and each property. Anshuman thanks his principal and teacher for their support and guidance in successfully completing the project.
Solution colligative properties 12th HSC Maharashtra state board
The document discusses solution colligative properties. It defines a solution as a homogeneous mixture of two or more pure substances, with the solvent present in larger quantity than the solute. Solution properties like vapor pressure, boiling point, and freezing point depend on the number of solute particles rather than their identity, and are known as colligative properties. Vapor pressure of a solution is lower than the pure solvent due to the solute particles replacing solvent molecules at the surface and preventing their vaporization. The degree of vapor pressure lowering depends on the mole fraction of solute particles.
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solutions state chemistry for class xii-
1. Solutions are homogeneous mixtures of two or more components, where the component present in smaller amounts is called the solute and the primary liquid component is the solvent.
2. Solutes can be electrolytes, which dissociate into ions, or nonelectrolytes, which do not dissociate. Common methods to express the concentration of solutions include molarity, molality, mole fraction, and percent composition.
3. The solubility of solids in liquids and gases in liquids depends on factors like temperature, pressure, and the nature of the solute and solvent. Henry's law and Raoult's law describe gas solubility and vapor pressure lowering in solutions. Ideal solutions follow
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
Ideal solution and non ideal solution
This document discusses ideal gases, Raoult's law, ideal solutions, and deviations from Raoult's law. It explains that an ideal gas is composed of randomly moving particles that only interact during elastic collisions. Raoult's law describes ideal solutions. Non-ideal solutions show either positive or negative deviations from Raoult's law due to differences in intermolecular forces between solvent-solute and pure components. Positive deviations occur when these interactions are weaker, while negative deviations occur when they are stronger.
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.
Colligative properties of dilute solutions Manik
lowering of vapour pressure, elevation of boiling point, depression of freezing point and osmotic pressure including necessary thermodynamic derivations.
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.
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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.
Binary liquids
This document provides an overview of binary liquid systems, including vapor pressure, Raoult's law, ideal and non-ideal solutions, solubility of liquids in liquids, and the lever rule. It discusses how vapor pressure works for solids and liquids and introduces Raoult's law, which states that the vapor pressure of a solution decreases based on the mole fraction of the solute. Ideal solutions obey Raoult's law while real solutions can show positive or negative deviations. Positive deviations occur when interactions between like molecules are stronger, while negative deviations occur when interactions between unlike molecules are stronger. The document also covers the different types of solubility between liquids and uses the lever rule to determine the composition and amount of each phase
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This document discusses colligative properties, which are physical properties of solutions that depend only on the ratio of solute to solvent particles and not the identity of the solute. It describes four colligative properties: boiling point elevation, freezing point depression, vapor pressure lowering, and osmotic pressure. It explains how adding a nonvolatile solute affects the phase diagram by shifting the freezing point downward and boiling point upward. Formulas are provided to calculate changes in boiling point and freezing point based on molality. Raoult's Law is introduced to explain how vapor pressure of a solution depends on the mole fraction of the solvent. Osmotic pressure is defined as the pressure required to prevent solvent flow across a semiperme
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.
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.
Soluion and colligative propertries 2017
it is based on CBSE, ICSE, HSC ,JEE, NEET, AIPMT, MTCET.
class 12 chemistry.
for buy ppt pay by paytm acount- 8879919898. price-Rs99 only/-
for more detail go my site
www.akchem.blogspot.com
Solution chemistry
The document discusses solutions and solution chemistry. It begins by defining solutions as homogeneous mixtures of two or more pure substances, with the solute dispersed uniformly throughout the solvent. It then discusses how solutions form and the energy changes that occur, including the enthalpy changes of separating solute and solvent particles and forming new interactions between them. The rest of the document discusses various factors that affect solubility, such as the nature of the solute and solvent, intermolecular forces, temperature, and pressure. It also covers colligative properties of solutions like vapor pressure lowering, boiling point elevation, freezing point depression, and osmotic pressure.
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.
Colligative Properties Of Solutions
A presentation discussing the main colligative properties of solutions, applicable for high school chemistry or AP Chemistry
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.
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.
Solution and colligative properties
I hope You all like it. I hope It is very beneficial for you all. I really thought that you all get enough knowledge from this presentation. This presentation is about materials and their classifications. After you read this presentation you knowledge is not as before.
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colligative property ,made by-chinmay jagadev pattanayak
colligative property ,made by-chinmay jagadev pattanayak
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This document discusses colligative properties of solutions such as freezing point depression, boiling point elevation, and osmotic pressure. It explains that these properties are affected by the number of particles in solution. For electrolyte solutions, the properties are greater than nonelectrolyte solutions of the same concentration due to dissociation of ions. The document also defines terms like isotonic, hypertonic, and hypotonic solutions and introduces the Van't Hoff factor to relate colligative properties of electrolytes to their degree of dissociation.
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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.
solution-ch2-ppt.pptx
This document discusses solutions and colligative properties. It defines key terms like solute, solvent, electrolyte and nonelectrolyte. It explains that a solution is a homogeneous mixture and describes different types of solutions like saturated, unsaturated and supersaturated. It also discusses how temperature, pressure and gas solubility relate. The document then covers colligative properties of solutions like vapor pressure lowering, boiling point elevation, freezing point depression and osmotic pressure. It indicates that for electrolytes, these properties depend on the van't Hoff factor which accounts for dissociation of ions in solution. Examples of applications of freezing point and boiling point changes are also provided.
DOC-20230413-WA0000.pptx
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Chapter 12 6-8 Colligative Properties presntation.pptx
This document discusses colligative properties of solutions, which are properties that depend only on the number of solute particles in solution. It defines four main colligative properties - vapor pressure lowering, boiling point elevation, freezing point depression, and osmotic pressure. The document provides formulas for calculating these properties and includes examples of their application. It also discusses how colligative properties are affected in electrolyte vs. nonelectrolyte solutions and introduces the concept of van't Hoff factor. Finally, it briefly touches on colloids and their differences from true solutions.
Soluton and colligative properties
The document discusses various concepts related to solutions including:
- Components of a solution including solvent, solute, and binary solutions.
- Different units used to express concentration such as mass percentage, volume percentage, parts per million, and mole fraction.
- Factors that affect solubility such as nature of solute and solvent, temperature, and pressure.
- Raoult's law and how it relates to ideal and non-ideal solutions.
- Colligative properties that depend only on the number of solute particles such as vapor pressure lowering, boiling point elevation, freezing point depression, and osmotic pressure.
Solution.pdf
The document discusses key concepts regarding solutions including how solutions form, factors that affect solubility, and colligative properties. It provides examples of how increasing pressure increases gas solubility according to Henry's Law and how adding solutes lowers vapor pressure and boiling point or freezing point depression based on colligative properties. The document is intended to teach students about solution chemistry.
solutionchemistry-.pdf
The document discusses key concepts regarding solutions including how solutions form, factors that affect solubility, and colligative properties. It provides examples of how increasing pressure increases gas solubility according to Henry's Law and how adding solutes lowers vapor pressure and boiling point or freezing point depression based on colligative properties. The document is intended to teach students about solution chemistry.
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https://www.etran.rs/2024/en/home-english/在线办理(salfor毕业证书)索尔福德大学毕业证毕业完成信一模一样
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3:国家专业人才认证中心颁发入库证书
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原版制作(carleton毕业证书)卡尔顿大学毕业证硕士文凭原版一模一样
原版纸张【微信：741003700 】【(carleton毕业证书)卡尔顿大学毕业证】【微信：741003700 】学位证，留信认证（真实可查，永久存档）offer、雅思、外壳等材料/诚信可靠,可直接看成品样本，帮您解决无法毕业带来的各种难题！外壳，原版制作，诚信可靠，可直接看成品样本。行业标杆！精益求精，诚心合作，真诚制作！多年品质 ,按需精细制作，24小时接单,全套进口原装设备。十五年致力于帮助留学生解决难题，包您满意。
本公司拥有海外各大学样板无数，能完美还原海外各大学 Bachelor Diploma degree, Master Degree Diploma
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1:该专业认证可证明留学生真实身份
2:同时对留学生所学专业登记给予评定
3:国家专业人才认证中心颁发入库证书
4:这个认证书并且可以归档倒地方
5:凡事获得留信网入网的信息将会逐步更新到个人身份内，将在公安局网内查询个人身份证信息后，同步读取人才网入库信息
6:个人职称评审加20分
7:个人信誉贷款加10分
8:在国家人才网主办的国家网络招聘大会中纳入资料，供国家高端企业选择人才
Phenomics assisted breeding in crop improvement
As the population is increasing and will reach about 9 billion upto 2050. Also due to climate change, it is difficult to meet the food requirement of such a large population. Facing the challenges presented by resource shortages, climate
change, and increasing global population, crop yield and quality need to be improved in a sustainable way over the coming decades. Genetic improvement by breeding is the best way to increase crop productivity. With the rapid progression of functional
genomics, an increasing number of crop genomes have been sequenced and dozens of genes influencing key agronomic traits have been identified. However, current genome sequence information has not been adequately exploited for understanding
the complex characteristics of multiple gene, owing to a lack of crop phenotypic data. Efficient, automatic, and accurate technologies and platforms that can capture phenotypic data that can
be linked to genomics information for crop improvement at all growth stages have become as important as genotyping. Thus,
high-throughput phenotyping has become the major bottleneck restricting crop breeding. Plant phenomics has been defined as the high-throughput, accurate acquisition and analysis of multi-dimensional phenotypes
during crop growing stages at the organism level, including the cell, tissue, organ, individual plant, plot, and field levels. With the rapid development of novel sensors, imaging technology,
and analysis methods, numerous infrastructure platforms have been developed for phenotyping.
Deep Software Variability and Frictionless Reproducibility
Deep Software Variability and Frictionless ReproducibilityUniversity of Rennes, INSA Rennes, Inria/IRISA, CNRS
The ability to recreate computational results with minimal effort and actionable metrics provides a solid foundation for scientific research and software development. When people can replicate an analysis at the touch of a button using open-source software, open data, and methods to assess and compare proposals, it significantly eases verification of results, engagement with a diverse range of contributors, and progress. However, we have yet to fully achieve this; there are still many sociotechnical frictions.
Inspired by David Donoho's vision, this talk aims to revisit the three crucial pillars of frictionless reproducibility (data sharing, code sharing, and competitive challenges) with the perspective of deep software variability.
Our observation is that multiple layers — hardware, operating systems, third-party libraries, software versions, input data, compile-time options, and parameters — are subject to variability that exacerbates frictions but is also essential for achieving robust, generalizable results and fostering innovation. I will first review the literature, providing evidence of how the complex variability interactions across these layers affect qualitative and quantitative software properties, thereby complicating the reproduction and replication of scientific studies in various fields.
I will then present some software engineering and AI techniques that can support the strategic exploration of variability spaces. These include the use of abstractions and models (e.g., feature models), sampling strategies (e.g., uniform, random), cost-effective measurements (e.g., incremental build of software configurations), and dimensionality reduction methods (e.g., transfer learning, feature selection, software debloating).
I will finally argue that deep variability is both the problem and solution of frictionless reproducibility, calling the software science community to develop new methods and tools to manage variability and foster reproducibility in software systems.
Exposé invité Journées Nationales du GDR GPL 2024
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2nd Lecture on Solutions | Chemistry Part I | 12th Science
- 1. The Malegaon High School & Jr. College Malegaon, (Nashik), 423203 2nd Lecture on Solutions Chemistry Part I, 12th Science By Rizwana Mohammad
- 2. Colligative properties of nonelectrolyte solutions: The physical properties of solutions that depend on the number of solute particles in solutions and not on their nature are called Colligative properties. These are 1. Vapour pressure lowering 2. Boiling point elevation 3. Freezing point depression 4. Osmotic pressure
- 3. 1. Vapour pressure lowering: When a liquid in a closed container is in equilibrium with its vapour, the pressure exerted by the vapour on the liquid is its vapour pressure. When a non-volatile, non-ionizable solid is dissolved in a liquid solvent, the vapour pressure of the solution is lower than that of pure solvent. if P1 0 = Vapour pressure of pure solvent P1 = Vapour pressure of solvent above the solution, therefore P1 < P1 0 ΔP = P1 0 - P1
- 4. Raoult’s law for solutions of non-volatile solutes: A plot of P1 Vs x1 is a straight line. Fig 1 : Variation of vapour pressure of solution with mole fraction solvent For binary solution x1 + x2 = 1 x1 = 1 – x2 P1 = P1 0 x1 = P1 0 (1 - x2) = P1 0 – P1 0 x2 P1 0 – P1 = P1 0 x2 ΔP = P1 0 x2 The above equation shows ΔP depends on x2 i.e. on number of solute particles. Thus, ΔP is a colligative property.
- 5. Relative lowering of vapour pressure: The ratio of vapour pressure lowering of solvent divided by the vapour pressure of pure solvent is called relative lowering of vapour pressure. Thus, Relative vapour pressure lowering = Δ𝑃 𝑃1 0 = 𝑃1 0 −𝑃1 𝑃1 0 Δ𝑃 𝑃1 0 = x2 𝑃1 0 −𝑃1 𝑃1 0 = x2
- 6. Molar mass of solute from vapour pressure lowering: Δ𝑃 𝑃1 0 = 𝑥2 We know that 𝑥2 = 𝑛2 𝑛1 +𝑛2 n1 and n2 are the moles of solvent and solute respectively. n1 >> n2 n1 + n2 ≈ n1 Therefore 𝑥2 = 𝑛2 𝑛1 Δ𝑃 𝑃1 0 = 𝑛2 𝑛1 …..1 n1 = 𝑤1 𝑀1 , n2 = 𝑤2 𝑀2 From eq. 1 Δ𝑃 𝑃1 0 = 𝑤2 𝑀2 𝑤1 𝑀1 𝑃1 0 −𝑃1 𝑃1 0 = Δ𝑃 𝑃1 0 = 𝑊2 𝑀1 𝑀2 𝑊1
- 7. Boiling point elevation: The boiling point of liquid is the temperature at which its vapour pressure equals the applied pressure. The boiling point of solution of non-volatile solute is higher than that of pure solvent. if Tb 0 = B.P. of pure solvent Tb = B.P. of solution Therefore, Tb > Tb 0 ΔTb = Tb - Tb 0 Boiling point elevation as a consequence of vapour pressure lowering: Fig 2 : Vapour pressure- temperature of pure solvent and solution.
- 8. Boiling point elevation and concentration of solute: The boiling point elevation is directly proportional to the molality of the solution. Thus, ΔTb ∝ m ΔTb = Kbm m = molality of solution Kb = boiling point elevation constant or molal elevation constant or ebullioscopic constant. If m = 1 , ΔTb = Kb Kb is the boiling point elevation produced by 1 molal solution. Unit of Kb = K kg mol-1
- 9. Molar mass of solute from boiling point elevation: ΔTb = Kbm …1 m = 𝑚𝑜𝑙𝑒𝑠 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑒 𝑚𝑎𝑠𝑠 𝑜𝑓 𝑠𝑜𝑙𝑣𝑒𝑛𝑡 𝑖𝑛 𝑘𝑔 = 𝑊2 𝑀2 𝑚𝑜𝑙 𝑊1 1000 𝑘𝑔 = 1000 𝑊2 𝑀2 𝑊1 𝑚𝑜𝑙 𝑘𝑔 − 1 …2 from eq. 1 & 2 ΔTb = Kb 1000 𝑊2 𝑀2 𝑊1 Hence M2 = 1000Kb 𝑊2 ΔTb 𝑊1