Physical properties of solutions can be summarized in 3 sentences:
A solution is a homogeneous mixture of two or more substances where the solute is present in smaller amounts and the solvent in larger amounts. Solutions can be characterized by their concentration and properties such as vapor pressure, boiling point, and freezing point are influenced by the number of solute particles based on colligative properties. Electrolyte solutions exhibit these colligative properties based on the van't Hoff factor which accounts for dissociation of solute particles in solution.
* Ethylene glycol (C2H6O2) molar mass = 62.07 g/mol
* Solution contains 478 g ethylene glycol
* Moles of ethylene glycol = 478 g / 62.07 g/mol = 7.69 mol
* Solution contains 3202 g water
* Mass of water = 3202 g
* Molality = moles of solute / kg of solvent
= 7.69 mol / 3.202 kg
= 2.40 m
* Freezing point depression constant (Kf) for water is 1.86 °C/m
* Freezing point depression = ΔTf = Kf × m
= 1.86 °C
1) Aqueous solutions are homogeneous mixtures where a solute is dissolved in a solvent, usually water. Water is a good solvent due to its polar molecular structure.
2) Solutions can be strong or weak electrolytes depending on how completely the solute dissociates into ions when dissolved. Strong electrolytes fully dissociate into many ions, while weak electrolytes only partially dissociate.
3) Precipitation reactions occur when oppositely charged ions in aqueous solutions combine to form an insoluble ionic compound as a solid precipitate. These reactions can be used to separate out desired products through filtration.
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.
This document provides an overview of stoichiometry in solutions. It outlines the key steps to solving stoichiometry problems which include identifying compounds/elements, writing balanced equations, calculating moles of reactants and products, and converting units. It then works through an example problem calculating the grams of aluminum chloride produced from a reaction between aluminum and hydrochloric acid.
This lab experiment investigated how the concentration and conductivity of a sodium chloride solution changed as sodium chloride was added incrementally. The solution's conductivity increased with each addition as the number of ions increased, until the fifth addition when undissolved salt remained, indicating saturation. The goal was to prepare saturated solutions of various ionic compounds and determine their concentrations using Ksp calculations and measurements.
This lab experiment explored how the concentration and conductivity of a sodium chloride solution changed as sodium chloride was added incrementally. The solution's conductivity increased with each addition as the number of ions increased in the fixed volume of water. Eventually, adding more sodium chloride no longer increased the conductivity, indicating the solution had reached saturation. The saturated solution was in dynamic equilibrium, with ions continuously dissolving from and crystallizing onto the solid.
This document summarizes key concepts about aqueous solutions and types of reactions from Chapter 4. It defines terms like solvent, solute, solubility, electrolytes, and molarity. It describes how water is a polar solvent that can dissolve ionic compounds by hydrating ions. It explains types of solutions like strong/weak electrolytes and acids/bases. Precipitation, acid-base, and other reactions in solutions are discussed along with molecular, complete ionic, and net ionic equations. Solubility rules and stoichiometry of precipitation reactions are also covered.
* Ethylene glycol (C2H6O2) molar mass = 62.07 g/mol
* Solution contains 478 g ethylene glycol
* Moles of ethylene glycol = 478 g / 62.07 g/mol = 7.69 mol
* Solution contains 3202 g water
* Mass of water = 3202 g
* Molality = moles of solute / kg of solvent
= 7.69 mol / 3.202 kg
= 2.40 m
* Freezing point depression constant (Kf) for water is 1.86 °C/m
* Freezing point depression = ΔTf = Kf × m
= 1.86 °C
1) Aqueous solutions are homogeneous mixtures where a solute is dissolved in a solvent, usually water. Water is a good solvent due to its polar molecular structure.
2) Solutions can be strong or weak electrolytes depending on how completely the solute dissociates into ions when dissolved. Strong electrolytes fully dissociate into many ions, while weak electrolytes only partially dissociate.
3) Precipitation reactions occur when oppositely charged ions in aqueous solutions combine to form an insoluble ionic compound as a solid precipitate. These reactions can be used to separate out desired products through filtration.
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.
This document provides an overview of stoichiometry in solutions. It outlines the key steps to solving stoichiometry problems which include identifying compounds/elements, writing balanced equations, calculating moles of reactants and products, and converting units. It then works through an example problem calculating the grams of aluminum chloride produced from a reaction between aluminum and hydrochloric acid.
This lab experiment investigated how the concentration and conductivity of a sodium chloride solution changed as sodium chloride was added incrementally. The solution's conductivity increased with each addition as the number of ions increased, until the fifth addition when undissolved salt remained, indicating saturation. The goal was to prepare saturated solutions of various ionic compounds and determine their concentrations using Ksp calculations and measurements.
This lab experiment explored how the concentration and conductivity of a sodium chloride solution changed as sodium chloride was added incrementally. The solution's conductivity increased with each addition as the number of ions increased in the fixed volume of water. Eventually, adding more sodium chloride no longer increased the conductivity, indicating the solution had reached saturation. The saturated solution was in dynamic equilibrium, with ions continuously dissolving from and crystallizing onto the solid.
This document summarizes key concepts about aqueous solutions and types of reactions from Chapter 4. It defines terms like solvent, solute, solubility, electrolytes, and molarity. It describes how water is a polar solvent that can dissolve ionic compounds by hydrating ions. It explains types of solutions like strong/weak electrolytes and acids/bases. Precipitation, acid-base, and other reactions in solutions are discussed along with molecular, complete ionic, and net ionic equations. Solubility rules and stoichiometry of precipitation reactions are also covered.
Many chemical reactions occur in water. Water is a polar solvent that can dissolve ionic compounds via hydration. When an ionic compound dissolves in water, it separates into its constituent ions which are surrounded by water molecules. The concentration of a solution is expressed as molarity, which is the number of moles of solute per liter of solution. Solutions can be prepared by accurately weighing out and dissolving the solute in a volumetric flask and diluting the solution as needed.
Physical Properties of Solutions discusses the key concepts of solutions including:
- A solution is a homogeneous mixture of two or more substances, with the solute present in smaller amounts than the solvent.
- Solubility is affected by temperature, with most solutes becoming more soluble at higher temperatures.
- Colligative properties depend only on the number of solute particles and include vapor pressure lowering, boiling point elevation, freezing point depression, and osmotic pressure.
- For electrolyte solutions, the van't Hoff factor accounts for particle dissociation, affecting colligative properties.
SOLUTION PPT CHAPTER 2(DONE BY AMAN RAJ CLASS XII-'A'.pptxSonam971503
This document provides an overview of solutions, including definitions of key terms like mixtures, heterogeneous mixtures, homogeneous mixtures, solutions, solutes, and solvents. It discusses different types of solutions like gaseous, liquid, and solid solutions. It also covers topics like concentration, solubility, factors that affect solubility, and the relationship between temperature and solubility. The document explains concepts such as molarity, dilutions, mass percent, and solution stoichiometry. Finally, it briefly introduces vapor pressure, Dalton's law of partial pressures, Raoult's law, ideal and non-ideal solutions, and pressure-composition curves.
This document discusses different types of solutions and concepts related to solutions. It defines heterogeneous and homogeneous mixtures, and notes that solutions are homogeneous mixtures composed of solutes and solvents. It describes factors that affect solubility, such as temperature, particle size, and polarity. The document also discusses concentration in terms of molarity, dilutions, mass percent, and solution stoichiometry. Finally, it covers vapor pressure concepts such as Dalton's law, Raoult's law, mole fraction in the vapor phase, ideal and non-ideal solutions, and positive and negative deviations from ideality.
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
Diploma_I_Applied science(chemistry)_U-II(A) Preparation of solution Rai University
This document provides definitions and concepts related to solutions and concentration units. It defines key terms like solute, solvent, saturated and unsaturated solutions. It also explains concepts like mole, molecular weight, equivalent weight and how to calculate them. Finally, it discusses different units of concentration including normality, molarity, molality, percentage, parts per million (ppm) and how to interconvert between them through examples.
This document defines key terms related to solutions and summarizes factors that affect solubility. It defines a solution as a homogeneous mixture where a solute is dissolved in a solvent. Temperature, pressure, and the nature of the solute and solvent affect solubility. There are various units to express concentration, including molarity, molality, and percent composition. Colligative properties like boiling point elevation and freezing point depression depend on the number of solute particles rather than their identity.
This document discusses different types of solutions and how they can be classified. It defines key terms like solute, solvent, saturated, unsaturated and supersaturated solutions. It also explains different ways of expressing the concentration of solutions, including percent by mass, parts per million, mole fraction, molarity and molality. Examples are provided for calculating concentration using each method. Finally, some sample problems are given for students to practice calculating concentrations of various solutions.
Physical properties of solutions - Basic Chemistrynihal233328
This document provides an overview of CHE 106 Chemistry course. The purpose of the course is to build a solid foundation of basic chemical concepts and principles for students and show examples of chemistry's important role in daily life to get students interested in chemistry. The course will use the textbook Chemistry by Chang R. and recommended supporting textbooks. It aims to develop students' understanding of fundamental chemical concepts and principles and inspire interest in chemistry through examples of its relevance to everyday life.
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.
The document provides information on different ways of expressing the concentration of solutions, including percent by mass, mole fraction, molarity, molality, percent by volume, and parts per million (ppm). It discusses an activity where students are asked to mix a substance with water and observe whether the mixture is uniform or non-uniform. Finally, it defines key terms related to solution concentration such as solution, solute, solvent, concentration, solubility, miscible, and immiscible.
A document discusses various types of mixtures and solutions. It defines heterogeneous and homogeneous mixtures, and describes solutions as homogeneous mixtures composed of solutes and solvents. The document discusses different types of solutions including gaseous, liquid, and solid solutions. It also covers topics like concentration, molarity, molality, mole fraction, saturation, solubility, and colligative properties. Colligative properties discussed include vapor pressure reduction, boiling point elevation, freezing point depression, and osmotic pressure. Factors affecting solubility and the rate of dissolution are also summarized.
1. The document discusses various concepts in chemistry including equivalent mass, normality, molarity, molality, strength of solutions, and percentage concentration.
2. It provides examples of calculating the equivalent mass of acids, bases, and salts. Normality is defined as the number of equivalents of solute per liter of solution.
3. Molarity is the number of moles of solute per liter of solution. Molality is the number of moles of solute per kilogram of solvent. Strength is the mass of solute per liter of solution.
The document discusses molarity, which is a measurement of concentration that expresses the number of moles of solute per liter of solution. It provides examples of calculating molarity when given the mass of a solute and volume of solution. It also covers diluting solutions, where the moles of solute stay the same but the concentration decreases as volume increases. Molarity can be used to determine the moles, mass, or volume of a solution component when any two pieces of information are known.
A 0.12 M solution of CuCl can be prepared by diluting a 0.29 M CuCl solution. The key steps are:
1) The original solution is 10 mL of 0.29 M CuCl. This contains 0.29 moles/L x 0.01 L = 0.0029 moles of CuCl.
2) The final solution volume is not specified, but the moles of CuCl must remain 0.0029 moles.
3) Using the dilution equation, the final volume can be calculated as 0.0029 moles / 0.12 M = 0.024 L or 24 mL.
4) Add water to the original 10 mL solution to
1. The document discusses various terms used to express the concentration of solutions such as percentage, molarity, molality, normality, and mole fraction. It provides examples and formulas to calculate these quantities.
2. Several numerical problems are given related to calculating concentration based on the mass or volume of components in a solution. This includes problems determining the percentage or mole fraction composition of mixed solutions.
3. Additional "HOTS" or higher-order thinking skills problems are presented involving multiple steps to determine volumes, densities, or concentrations required to achieve a desired solution composition.
1. The document discusses various terms used to express the concentration of solutions such as percentage, molarity, molality, normality, and mole fraction. It provides examples and formulas to calculate these quantities.
2. Several numerical problems are given related to calculating concentration based on the mass or volume of components in a solution. This includes problems determining the percentage or mole fraction composition of mixed solutions.
3. Additional "HOTS" or higher-order thinking skills problems are presented involving multiple steps to determine volumes or densities based on given molarities, molalities, or percentages of solutions.
1. The document discusses various terms used to express the concentration of solutions such as percentage, molarity, molality, normality, and mole fraction.
2. It provides examples and formulas to calculate concentration based on these terms, and the relationships between some of the terms like molarity and molality.
3. Several numerical problems are included at the end to practice calculating concentration values using the different terms and their relationships.
This is the power point presentation for the students of class XII. This includes: Types of solutions, concentration of solutions, Solution of solid in liquid, solution of gas in liquid: Henry's law, vapour pressure of solutions, Raoult's law, Ideal & non ideal solutions, azeotropic mixtures, Colligative properties - (1) relative lowering of vapour pressure of solution of volatile solute, (2) elevation in boiling point of solution (3) depression in freezing point of solution (4) osmotic pressure, abnormal molar mass of solute, Van't Hoff's factor, numerical problems.
This document provides information on various chemistry concepts related to solutions including:
1) Definitions of key terms like solvent, solute, concentration, and activity.
2) Explanations of concentration terms like molarity, molality, and normality.
3) Procedures for preparing solutions of specific concentrations.
4) Calculations for determining molecular weights, equivalent weights, and concentrations in parts per million and billion.
5) A description and procedure for standardizing a potassium permanganate solution through titration with oxalic acid.
Many chemical reactions occur in water. Water is a polar solvent that can dissolve ionic compounds via hydration. When an ionic compound dissolves in water, it separates into its constituent ions which are surrounded by water molecules. The concentration of a solution is expressed as molarity, which is the number of moles of solute per liter of solution. Solutions can be prepared by accurately weighing out and dissolving the solute in a volumetric flask and diluting the solution as needed.
Physical Properties of Solutions discusses the key concepts of solutions including:
- A solution is a homogeneous mixture of two or more substances, with the solute present in smaller amounts than the solvent.
- Solubility is affected by temperature, with most solutes becoming more soluble at higher temperatures.
- Colligative properties depend only on the number of solute particles and include vapor pressure lowering, boiling point elevation, freezing point depression, and osmotic pressure.
- For electrolyte solutions, the van't Hoff factor accounts for particle dissociation, affecting colligative properties.
SOLUTION PPT CHAPTER 2(DONE BY AMAN RAJ CLASS XII-'A'.pptxSonam971503
This document provides an overview of solutions, including definitions of key terms like mixtures, heterogeneous mixtures, homogeneous mixtures, solutions, solutes, and solvents. It discusses different types of solutions like gaseous, liquid, and solid solutions. It also covers topics like concentration, solubility, factors that affect solubility, and the relationship between temperature and solubility. The document explains concepts such as molarity, dilutions, mass percent, and solution stoichiometry. Finally, it briefly introduces vapor pressure, Dalton's law of partial pressures, Raoult's law, ideal and non-ideal solutions, and pressure-composition curves.
This document discusses different types of solutions and concepts related to solutions. It defines heterogeneous and homogeneous mixtures, and notes that solutions are homogeneous mixtures composed of solutes and solvents. It describes factors that affect solubility, such as temperature, particle size, and polarity. The document also discusses concentration in terms of molarity, dilutions, mass percent, and solution stoichiometry. Finally, it covers vapor pressure concepts such as Dalton's law, Raoult's law, mole fraction in the vapor phase, ideal and non-ideal solutions, and positive and negative deviations from ideality.
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
Diploma_I_Applied science(chemistry)_U-II(A) Preparation of solution Rai University
This document provides definitions and concepts related to solutions and concentration units. It defines key terms like solute, solvent, saturated and unsaturated solutions. It also explains concepts like mole, molecular weight, equivalent weight and how to calculate them. Finally, it discusses different units of concentration including normality, molarity, molality, percentage, parts per million (ppm) and how to interconvert between them through examples.
This document defines key terms related to solutions and summarizes factors that affect solubility. It defines a solution as a homogeneous mixture where a solute is dissolved in a solvent. Temperature, pressure, and the nature of the solute and solvent affect solubility. There are various units to express concentration, including molarity, molality, and percent composition. Colligative properties like boiling point elevation and freezing point depression depend on the number of solute particles rather than their identity.
This document discusses different types of solutions and how they can be classified. It defines key terms like solute, solvent, saturated, unsaturated and supersaturated solutions. It also explains different ways of expressing the concentration of solutions, including percent by mass, parts per million, mole fraction, molarity and molality. Examples are provided for calculating concentration using each method. Finally, some sample problems are given for students to practice calculating concentrations of various solutions.
Physical properties of solutions - Basic Chemistrynihal233328
This document provides an overview of CHE 106 Chemistry course. The purpose of the course is to build a solid foundation of basic chemical concepts and principles for students and show examples of chemistry's important role in daily life to get students interested in chemistry. The course will use the textbook Chemistry by Chang R. and recommended supporting textbooks. It aims to develop students' understanding of fundamental chemical concepts and principles and inspire interest in chemistry through examples of its relevance to everyday life.
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.
The document provides information on different ways of expressing the concentration of solutions, including percent by mass, mole fraction, molarity, molality, percent by volume, and parts per million (ppm). It discusses an activity where students are asked to mix a substance with water and observe whether the mixture is uniform or non-uniform. Finally, it defines key terms related to solution concentration such as solution, solute, solvent, concentration, solubility, miscible, and immiscible.
A document discusses various types of mixtures and solutions. It defines heterogeneous and homogeneous mixtures, and describes solutions as homogeneous mixtures composed of solutes and solvents. The document discusses different types of solutions including gaseous, liquid, and solid solutions. It also covers topics like concentration, molarity, molality, mole fraction, saturation, solubility, and colligative properties. Colligative properties discussed include vapor pressure reduction, boiling point elevation, freezing point depression, and osmotic pressure. Factors affecting solubility and the rate of dissolution are also summarized.
1. The document discusses various concepts in chemistry including equivalent mass, normality, molarity, molality, strength of solutions, and percentage concentration.
2. It provides examples of calculating the equivalent mass of acids, bases, and salts. Normality is defined as the number of equivalents of solute per liter of solution.
3. Molarity is the number of moles of solute per liter of solution. Molality is the number of moles of solute per kilogram of solvent. Strength is the mass of solute per liter of solution.
The document discusses molarity, which is a measurement of concentration that expresses the number of moles of solute per liter of solution. It provides examples of calculating molarity when given the mass of a solute and volume of solution. It also covers diluting solutions, where the moles of solute stay the same but the concentration decreases as volume increases. Molarity can be used to determine the moles, mass, or volume of a solution component when any two pieces of information are known.
A 0.12 M solution of CuCl can be prepared by diluting a 0.29 M CuCl solution. The key steps are:
1) The original solution is 10 mL of 0.29 M CuCl. This contains 0.29 moles/L x 0.01 L = 0.0029 moles of CuCl.
2) The final solution volume is not specified, but the moles of CuCl must remain 0.0029 moles.
3) Using the dilution equation, the final volume can be calculated as 0.0029 moles / 0.12 M = 0.024 L or 24 mL.
4) Add water to the original 10 mL solution to
1. The document discusses various terms used to express the concentration of solutions such as percentage, molarity, molality, normality, and mole fraction. It provides examples and formulas to calculate these quantities.
2. Several numerical problems are given related to calculating concentration based on the mass or volume of components in a solution. This includes problems determining the percentage or mole fraction composition of mixed solutions.
3. Additional "HOTS" or higher-order thinking skills problems are presented involving multiple steps to determine volumes, densities, or concentrations required to achieve a desired solution composition.
1. The document discusses various terms used to express the concentration of solutions such as percentage, molarity, molality, normality, and mole fraction. It provides examples and formulas to calculate these quantities.
2. Several numerical problems are given related to calculating concentration based on the mass or volume of components in a solution. This includes problems determining the percentage or mole fraction composition of mixed solutions.
3. Additional "HOTS" or higher-order thinking skills problems are presented involving multiple steps to determine volumes or densities based on given molarities, molalities, or percentages of solutions.
1. The document discusses various terms used to express the concentration of solutions such as percentage, molarity, molality, normality, and mole fraction.
2. It provides examples and formulas to calculate concentration based on these terms, and the relationships between some of the terms like molarity and molality.
3. Several numerical problems are included at the end to practice calculating concentration values using the different terms and their relationships.
This is the power point presentation for the students of class XII. This includes: Types of solutions, concentration of solutions, Solution of solid in liquid, solution of gas in liquid: Henry's law, vapour pressure of solutions, Raoult's law, Ideal & non ideal solutions, azeotropic mixtures, Colligative properties - (1) relative lowering of vapour pressure of solution of volatile solute, (2) elevation in boiling point of solution (3) depression in freezing point of solution (4) osmotic pressure, abnormal molar mass of solute, Van't Hoff's factor, numerical problems.
This document provides information on various chemistry concepts related to solutions including:
1) Definitions of key terms like solvent, solute, concentration, and activity.
2) Explanations of concentration terms like molarity, molality, and normality.
3) Procedures for preparing solutions of specific concentrations.
4) Calculations for determining molecular weights, equivalent weights, and concentrations in parts per million and billion.
5) A description and procedure for standardizing a potassium permanganate solution through titration with oxalic acid.
Similar to Ch 12 Physical Properties of Solutions.ppt (20)
This report explores the significance of border towns and spaces for strengthening responses to young people on the move. In particular it explores the linkages of young people to local service centres with the aim of further developing service, protection, and support strategies for migrant children in border areas across the region. The report is based on a small-scale fieldwork study in the border towns of Chipata and Katete in Zambia conducted in July 2023. Border towns and spaces provide a rich source of information about issues related to the informal or irregular movement of young people across borders, including smuggling and trafficking. They can help build a picture of the nature and scope of the type of movement young migrants undertake and also the forms of protection available to them. Border towns and spaces also provide a lens through which we can better understand the vulnerabilities of young people on the move and, critically, the strategies they use to navigate challenges and access support.
The findings in this report highlight some of the key factors shaping the experiences and vulnerabilities of young people on the move – particularly their proximity to border spaces and how this affects the risks that they face. The report describes strategies that young people on the move employ to remain below the radar of visibility to state and non-state actors due to fear of arrest, detention, and deportation while also trying to keep themselves safe and access support in border towns. These strategies of (in)visibility provide a way to protect themselves yet at the same time also heighten some of the risks young people face as their vulnerabilities are not always recognised by those who could offer support.
In this report we show that the realities and challenges of life and migration in this region and in Zambia need to be better understood for support to be strengthened and tuned to meet the specific needs of young people on the move. This includes understanding the role of state and non-state stakeholders, the impact of laws and policies and, critically, the experiences of the young people themselves. We provide recommendations for immediate action, recommendations for programming to support young people on the move in the two towns that would reduce risk for young people in this area, and recommendations for longer term policy advocacy.
United Nations World Oceans Day 2024; June 8th " Awaken new dephts".Christina Parmionova
The program will expand our perspectives and appreciation for our blue planet, build new foundations for our relationship to the ocean, and ignite a wave of action toward necessary change.
Jennifer Schaus and Associates hosts a complimentary webinar series on The FAR in 2024. Join the webinars on Wednesdays and Fridays at noon, eastern.
Recordings are on YouTube and the company website.
https://www.youtube.com/@jenniferschaus/videos
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Jennifer Schaus and Associates hosts a complimentary webinar series on The FAR in 2024. Join the webinars on Wednesdays and Fridays at noon, eastern.
Recordings are on YouTube and the company website.
https://www.youtube.com/@jenniferschaus/videos
2. 12.1
A solution is a homogenous mixture of 2 or
more substances
The solute is(are) the substance(s) present in the
smaller amount(s)
The solvent is the substance present in the larger
amount
3. An electrolyte is a substance that, when dissolved in
water, results in a solution that can conduct electricity.
A nonelectrolyte is a substance that, when dissolved,
results in a solution that does not conduct electricity.
nonelectrolyte weak electrolyte strong electrolyte
4.1
4. A saturated solution contains the maximum amount of a
solute that will dissolve in a given solvent at a specific
temperature.
An unsaturated solution contains less solute than the
solvent has the capacity to dissolve at a specific
temperature.
A supersaturated solution contains more solute than is
present in a saturated solution at a specific temperature.
Sodium acetate crystals rapidly form when a seed crystal is
added to a supersaturated solution of sodium acetate.
12.1
5. 12.2
Three types of interactions in the solution process:
• solvent-solvent interaction
• solute-solute interaction
• solvent-solute interaction
DHsoln = DH1 + DH2 + DH3
6. “like dissolves like”
Two substances with similar intermolecular forces are likely
to be soluble in each other.
• non-polar molecules are soluble in non-polar solvents
CCl4 in C6H6
• polar molecules are soluble in polar solvents
C2H5OH in H2O
• ionic compounds are more soluble in polar solvents
NaCl in H2O or NH3 (l)
12.2
7. Concentration Units
The concentration of a solution is the amount of solute
present in a given quantity of solvent or solution.
Percent by Mass
% by mass = x 100%
mass of solute
mass of solute + mass of solvent
= x 100%
mass of solute
mass of solution
12.3
Mole Fraction (X)
XA =
moles of A
sum of moles of all components
8. Concentration Units Continued
M =
moles of solute
liters of solution
Molarity (M)
Molality (m)
m =
moles of solute
mass of solvent (kg)
12.3
9. What is the molality of a 5.86 M ethanol (C2H5OH)
solution whose density is 0.927 g/mL?
m =
moles of solute
mass of solvent (kg)
M =
moles of solute
liters of solution
Assume 1 L of solution:
5.86 moles ethanol = 270 g ethanol
927 g of solution (1000 mL x 0.927 g/mL)
mass of solvent = mass of solution – mass of solute
= 927 g – 270 g = 657 g = 0.657 kg
m =
moles of solute
mass of solvent (kg)
=
5.86 moles C2H5OH
0.657 kg solvent
= 8.92 m
12.3
10. Temperature and Solubility
Solid solubility and temperature
solubility increases with
increasing temperature
solubility decreases with
increasing temperature
12.4
11. Fractional crystallization is the separation of a mixture of
substances into pure components on the basis of their differing
solubilities.
Suppose you have 90 g KNO3
contaminated with 10 g NaCl.
Fractional crystallization:
1. Dissolve sample in 100 mL of
water at 600C
2. Cool solution to 00C
3. All NaCl will stay in solution
(s = 34.2g/100g)
4. 78 g of PURE KNO3 will
precipitate (s = 12 g/100g).
90 g – 12 g = 78 g
12.4
13. Pressure and Solubility of Gases
The solubility of a gas in a liquid is proportional to the
pressure of the gas over the solution (Henry’s law).
c = kP
c is the concentration (M) of the dissolved gas
P is the pressure of the gas over the solution
k is a constant (mol/L•atm) that depends only
on temperature
low P
low c
high P
high c
14. Chemistry In Action: The Killer Lake
Lake Nyos, West Africa
8/21/86
CO2 Cloud Released
1700 Casualties
Trigger?
• earthquake
• landslide
• strong Winds
15. Solution Stoichiometry (Chapter 4)
The concentration of a solution is the amount of solute
present in a given quantity of solvent or solution.
M = molarity =
moles of solute
liters of solution
What mass of KI is required to make 500. mL of
a 2.80 M KI solution?
volume KI moles KI grams KI
M KI M KI
500. mL = 232 g KI
166 g KI
1 mol KI
x
2.80 mol KI
1 L soln
x
1 L
1000 mL
x
4.5
17. Dilution is the procedure for preparing a less concentrated
solution from a more concentrated solution.
Dilution
Add Solvent
Moles of solute
before dilution (i)
Moles of solute
after dilution (f)
=
MiVi MfVf
=
4.5
18. How would you prepare 60.0 mL of 0.2 M
HNO3 from a stock solution of 4.00 M HNO3?
MiVi = MfVf
Mi = 4.00 Mf = 0.200 Vf = 0.06 L Vi = ? L
4.5
Vi =
MfVf
Mi
=
0.200 x 0.06
4.00
= 0.003 L = 3 mL
3 mL of acid + 57 mL of water = 60 mL of solution
19. Gravimetric Analysis
4.6
1. Dissolve unknown substance in water
2. React unknown with known substance to form a precipitate
3. Filter and dry precipitate
4. Weigh precipitate
5. Use chemical formula and mass of precipitate to determine
amount of unknown ion
20. Titrations
In a titration a solution of accurately known concentration is
added gradually added to another solution of unknown
concentration until the chemical reaction between the two
solutions is complete.
Equivalence point – the point at which the reaction is complete
Indicator – substance that changes color at (or near) the
equivalence point
Slowly add base
to unknown acid
UNTIL
the indicator
changes color
4.7
21. What volume of a 1.420 M NaOH solution is
Required to titrate 25.00 mL of a 4.50 M H2SO4
solution?
4.7
WRITE THE CHEMICAL EQUATION!
volume acid moles acid moles base volume base
H2SO4 + 2NaOH 2H2O + Na2SO4
4.50 mol H2SO4
1000 mL soln
x
2 mol NaOH
1 mol H2SO4
x
1000 ml soln
1.420 mol NaOH
x
25.00 mL = 158 mL
M
acid
rx
coef.
M
base
22. Chemistry in Action: Metals from the Sea
CaCO3 (s) CaO (s) + CO2 (g)
Mg(OH)2 (s) + 2HCl (aq) MgCl2 (aq) + 2H2O (l)
CaO (s) + H2O (l) Ca2+ (aq) + 2OH (aq)
-
Mg2+ (aq) + 2OH (aq) Mg(OH)2 (s)
-
Mg2+ + 2e- Mg
2Cl- Cl2 + 2e-
MgCl2 (l) Mg (l) + Cl2 (g)
Now back to Chapter 12…
23. Colligative Properties of Nonelectrolyte Solutions
Colligative properties are properties that depend only on the
number of solute particles in solution and not on the nature of
the solute particles.
Vapor-Pressure Lowering
Raoult’s law
If the solution contains only one solute:
X1 = 1 – X2
P 1
0
- P1 = DP = X2 P 1
0
P 1
0
= vapor pressure of pure solvent
X1 = mole fraction of the solvent
X2 = mole fraction of the solute
12.6
P1 = X1 P 1
0
24. PA = XA P A
0
PB = XB P B
0
PT = PA + PB
PT = XA P A
0
+ XB P B
0
Ideal Solution
12.6
25. PT is greater than
predicted by Raoults’s law
PT is less than
predicted by Raoults’s law
Force
A-B
Force
A-A
Force
B-B
< &
Force
A-B
Force
A-A
Force
B-B
> &
12.6
27. Boiling-Point Elevation
DTb = Tb – T b
0
Tb > T b
0
DTb > 0
T b is the boiling point of
the pure solvent
0
T b is the boiling point of
the solution
DTb = Kb m
m is the molality of the solution
Kb is the molal boiling-point
elevation constant (0C/m)
12.6
28. Freezing-Point Depression
DTf = T f – Tf
0
T f > Tf
0
DTf > 0
T f is the freezing point of
the pure solvent
0
T f is the freezing point of
the solution
DTf = Kf m
m is the molality of the solution
Kf is the molal freezing-point
depression constant (0C/m)
12.6
30. What is the freezing point of a solution containing 478 g
of ethylene glycol (antifreeze) in 3202 g of water? The
molar mass of ethylene glycol is 62.01 g.
DTf = Kf m
m =
moles of solute
mass of solvent (kg)
= 2.41 m
=
3.202 kg solvent
478 g x
1 mol
62.01 g
Kf water = 1.86 0C/m
DTf = Kf m = 1.86 0C/m x 2.41 m = 4.48 0C
DTf = T f – Tf
0
Tf = T f – DTf
0
= 0.00 0C – 4.48 0C = -4.48 0C
12.6
31. Colligative Properties of Nonelectrolyte Solutions
Colligative properties are properties that depend only on the
number of solute particles in solution and not on the nature of
the solute particles.
12.6
Vapor-Pressure Lowering P1 = X1 P 1
0
Boiling-Point Elevation DTb = Kb m
Freezing-Point Depression DTf = Kf m
Osmotic Pressure (p) p = MRT
32. Colligative Properties of Electrolyte Solutions
12.7
0.1 m NaCl solution 0.1 m Na+ ions & 0.1 m Cl- ions
Colligative properties are properties that depend only on the
number of solute particles in solution and not on the nature of
the solute particles.
0.1 m NaCl solution 0.2 m ions in solution
van’t Hoff factor (i) =
actual number of particles in soln after dissociation
number of formula units initially dissolved in soln
nonelectrolytes
NaCl
CaCl2
i should be
1
2
3
33. Which would you use for the streets of
Bloomington to lower the freezing point
of ice and why? Would the temperature
make any difference in your decision?
a) sand, SiO2
b) Rock salt, NaCl
c) Ice Melt, CaCl2
Change in Freezing Point
34. Boiling-Point Elevation DTb = i Kb m
Freezing-Point Depression DTf = i Kf m
Osmotic Pressure (p) p = iMRT
Colligative Properties of Electrolyte Solutions
12.7
35. Change in Freezing Point
Common Applications
of Freezing Point
Depression
Propylene glycol
Ethylene
glycol –
deadly to
small
animals
36. Change in Boiling Point
Common Applications of
Boiling Point Elevation
37. At what temperature will a 5.4 molal
solution of NaCl freeze?
Solution
∆TFP = Kf • m • i
∆TFP = (1.86 oC/molal) • 5.4 m • 2
∆TFP = 20.1 oC
FP = 0 – 20.1 = -20.1 oC
Freezing Point Depression
39. Osmotic Pressure (p)
12.6
Osmosis is the selective passage of solvent molecules through a porous
membrane from a dilute solution to a more concentrated one.
A semipermeable membrane allows the passage of solvent molecules but
blocks the passage of solute molecules.
Osmotic pressure (p) is the pressure required to stop osmosis.
dilute
more
concentrated
43. A colloid is a dispersion of particles of one substance
throughout a dispersing medium of another substance.
Colloid versus solution
• collodial particles are much larger than solute molecules
• collodial suspension is not as homogeneous as a solution
12.8