This document contains chemistry questions related to solutions. It includes questions about types of solutions, properties of solutions like boiling point elevation and freezing point depression, and calculations involving molarity, molality, and vapor pressure. The questions cover topics like ideal and non-ideal solutions, Raoult's law, colligative properties, and van't Hoff factor.
This document summarizes key concepts about types of chemical reactions and solution stoichiometry. It discusses water as a solvent, solubility, strong and weak electrolytes, and precipitation, acid-base, and oxidation-reduction reactions in solution. Calculations involve determining moles and masses of reactants and products using molarity, volumes, and balanced equations. Common indicators like phenolphthalein are used in acid-base titrations.
This document discusses the distribution law, also known as the partition coefficient, which describes how a solute will distribute between two immiscible solvents at equilibrium. It provides the equation that the concentration of the solute in the first solvent (C1) divided by the concentration in the second solvent (C2) equals the distribution coefficient (KD). Several applications of the distribution law are described, including solvent extraction, partition chromatography, and determining solubility, dissociation, and association.
F.Sc. Part 1 Chemistry.Ch.09.Test (Malik Xufyan)Malik Xufyan
- The document discusses chemistry test papers and series from Maliks Chemistry for classes 9th, 10th, F.Sc part 1 and part 2.
- It provides chapter-wise and board paper-wise test series to help students prepare for their chemistry exams.
- Contact information is given for JIAS Academy, the publisher of the test series, along with details of other publications available.
AP Chemistry Chapter 13 Sample ExercisesJane Hamze
The document describes calculating the entropy change and disorder/order of a system when water vapor reacts with solid sodium sulfate to form a hydrated salt. It first examines the initial and final states to determine if the system becomes more or less dispersed. Since the water vapor becomes confined in the solid hydrate lattice, the system becomes more ordered and the entropy decreases.
3166995- Solutions, Electrolytes, and Concentrations..docxDavidWestern8
This document summarizes an experiment on solutions, electrolytes, and concentrations. It describes how polar and nonpolar solutes dissolve in polar and nonpolar solvents respectively. Strong electrolytes fully dissociate into ions and have high conductivity, while weak electrolytes partially dissociate and have lower conductivity. Non-electrolytes do not form ions. The document calculates the concentration of NaCl using the mass of solute and volume of solution. The concentration is reported as 5.35M NaCl. It concludes that different compounds have varying behaviors in solutions depending on their polarity and ability to dissociate into ions.
This document appears to be an exam for a chemistry course. It contains 27 multiple choice questions testing concepts related to intermolecular forces, phase diagrams, solutions, and chemical kinetics. The key at the bottom provides the correct answer for each question.
This document outlines an experiment to determine the critical solution temperature of the phenol-water system. It describes the objective, requirements, theory, procedure, observations, calculations, results and precautions. The key steps are: mixing phenol and water in varying proportions, heating with stirring and noting the temperature at which the mixture becomes clear, then cooling and noting when turbidity reappears. By plotting the miscibility temperatures against phenol concentration, the maximum value on the curve gives the critical solution temperature, which is the temperature above which phenol and water are completely miscible in all proportions.
F.Sc. Part 1 Paper Faisalabad Board 2008 (Malik Xufyan)Malik Xufyan
This document contains a chemistry exam for the Faisalabad Board in 2008. It includes a 20 minute, 17 question multiple choice section on topics like combustion analysis, chromatography, sublimation, gas properties, London dispersion forces, and orbital configurations. It also includes a 2 hour and 40 minute subjective/essay section asking students to define terms like isotopes, vapor pressure, state functions, and more. Students are asked to calculate molar masses, percentage ionizations, and determine molecular weights from temperature changes. Questions also address electrode potentials, reaction rates and temperature, and how catalysts affect reversible reactions.
This document summarizes key concepts about types of chemical reactions and solution stoichiometry. It discusses water as a solvent, solubility, strong and weak electrolytes, and precipitation, acid-base, and oxidation-reduction reactions in solution. Calculations involve determining moles and masses of reactants and products using molarity, volumes, and balanced equations. Common indicators like phenolphthalein are used in acid-base titrations.
This document discusses the distribution law, also known as the partition coefficient, which describes how a solute will distribute between two immiscible solvents at equilibrium. It provides the equation that the concentration of the solute in the first solvent (C1) divided by the concentration in the second solvent (C2) equals the distribution coefficient (KD). Several applications of the distribution law are described, including solvent extraction, partition chromatography, and determining solubility, dissociation, and association.
F.Sc. Part 1 Chemistry.Ch.09.Test (Malik Xufyan)Malik Xufyan
- The document discusses chemistry test papers and series from Maliks Chemistry for classes 9th, 10th, F.Sc part 1 and part 2.
- It provides chapter-wise and board paper-wise test series to help students prepare for their chemistry exams.
- Contact information is given for JIAS Academy, the publisher of the test series, along with details of other publications available.
AP Chemistry Chapter 13 Sample ExercisesJane Hamze
The document describes calculating the entropy change and disorder/order of a system when water vapor reacts with solid sodium sulfate to form a hydrated salt. It first examines the initial and final states to determine if the system becomes more or less dispersed. Since the water vapor becomes confined in the solid hydrate lattice, the system becomes more ordered and the entropy decreases.
3166995- Solutions, Electrolytes, and Concentrations..docxDavidWestern8
This document summarizes an experiment on solutions, electrolytes, and concentrations. It describes how polar and nonpolar solutes dissolve in polar and nonpolar solvents respectively. Strong electrolytes fully dissociate into ions and have high conductivity, while weak electrolytes partially dissociate and have lower conductivity. Non-electrolytes do not form ions. The document calculates the concentration of NaCl using the mass of solute and volume of solution. The concentration is reported as 5.35M NaCl. It concludes that different compounds have varying behaviors in solutions depending on their polarity and ability to dissociate into ions.
This document appears to be an exam for a chemistry course. It contains 27 multiple choice questions testing concepts related to intermolecular forces, phase diagrams, solutions, and chemical kinetics. The key at the bottom provides the correct answer for each question.
This document outlines an experiment to determine the critical solution temperature of the phenol-water system. It describes the objective, requirements, theory, procedure, observations, calculations, results and precautions. The key steps are: mixing phenol and water in varying proportions, heating with stirring and noting the temperature at which the mixture becomes clear, then cooling and noting when turbidity reappears. By plotting the miscibility temperatures against phenol concentration, the maximum value on the curve gives the critical solution temperature, which is the temperature above which phenol and water are completely miscible in all proportions.
F.Sc. Part 1 Paper Faisalabad Board 2008 (Malik Xufyan)Malik Xufyan
This document contains a chemistry exam for the Faisalabad Board in 2008. It includes a 20 minute, 17 question multiple choice section on topics like combustion analysis, chromatography, sublimation, gas properties, London dispersion forces, and orbital configurations. It also includes a 2 hour and 40 minute subjective/essay section asking students to define terms like isotopes, vapor pressure, state functions, and more. Students are asked to calculate molar masses, percentage ionizations, and determine molecular weights from temperature changes. Questions also address electrode potentials, reaction rates and temperature, and how catalysts affect reversible reactions.
This document provides definitions and examples of key concepts in general chemistry including:
1. Solvation refers to the attractive interaction between solvent molecules and a solute. Hydration describes the interaction when water is the solvent.
2. The overall enthalpy change of a solution can be either positive (endothermic) or negative (exothermic).
3. A saturated solution is one in equilibrium with undissolved solute where dissolution and crystallization occur at equal rates. Unsaturated and supersaturated solutions contain less or more solute respectively.
4. Colligative properties include vapor pressure depression, freezing point depression, boiling point elevation, and osmotic pressure.
PHYSICAL CHEMISTRY - Two Components Liquid Systemshahzadebaujiti
PHYSICAL CHEMISTRY - Two Components Liquid System
IMMISCIBLE LIQUIDS
Immiscible liquids are liquids which do not mix up to form homogeneous mixture.
When there are two immiscible liquids they form a so called immiscible pair.
Immiscible liquids form heterogeneous mixture.
Environmentatl chemistry water (questions and answers)Martin Brown
This document contains exam questions from 2009-2002 on the topics of water treatment, water quality testing, acid-base chemistry, and sewage treatment. It asks students to define concepts like conjugate acid-base pairs, calculate pH values, identify chemicals used in water treatment and their purposes, and describe the multi-stage processes involved in treating water and sewage.
The poem discusses pollution in American cities. It warns that visitors should not drink the water or breathe the air due to the high levels of pollution, which include smog, sewage, and industrial waste. The pollution has wiped out fish and bird populations. While people try to take precautions like using toothpaste, the pollution is still present in the city streets and waterways.
Colligative properties of dilute solutions Manik Imran Nur Manik
lowering of vapour pressure, elevation of boiling point, depression of freezing point and osmotic pressure including necessary thermodynamic derivations.
Distribution Law
What is Distribution law?
Immiscible liquids
Explanation
APPLICATION OF DISTRIBUTION LAW
Limitations of Distribution Law
Contrast and Comparison between separation through Separating funnel and Fractional Distillation
This document discusses various properties of mixtures, including solutions and colloids. It defines key terms like solvent, solute, and aqueous solutions. It describes factors that affect solubility such as temperature, nature of solute and solvent, and pressure. It also covers gas solubility based on Henry's Law. Finally, it discusses quantitative expressions of concentration including molarity and molality, as well as colligative properties of solutions like boiling point elevation.
1. The document discusses vapor pressure concepts including Raoult's law and ideal solutions. It provides questions related to how vapor pressure is affected by factors like temperature, moles of vapor/liquid, and addition of a non-volatile solute.
2. Key concepts covered include how vapor pressure of a solution is lower than the pure solvent due to the non-volatile solute occupying space in the liquid phase. An ideal solution follows Raoult's law where vapor pressure is directly proportional to mole fraction of solvent.
3. Questions assess understanding of these concepts through calculations and identifying properties of ideal/non-ideal solutions and relationships between liquid/vapor phase compositions according to vapor pressure diagrams.
This document provides information and examples on solutions and titrations in chemistry:
- It defines key terms like solute, solvent, concentration, molarity and explains how to calculate concentrations in g/dm3 and moldm-3.
- Examples are given for calculating the mass of a solute needed to make a solution of a given volume and molarity, and for calculating concentrations when solutions are diluted.
- A titration is described as a procedure using a burette to add one solution of known concentration to a flask of another until reaction is complete.
- Standard solutions that are suitable for titrations are outlined.
- Worked examples of titration calculations include determining
This document discusses electrolyte solutions, milliequivalents, millimoles, micromoles, and osmolarity as they relate to water and electrolyte balance in the body. It provides definitions and examples of calculating concentrations of electrolytes using various units. Electrolytes play an important role in acid-base balance, water volume control, and metabolism. Disturbances in electrolyte and fluid balance can be treated with oral and intravenous electrolyte preparations. Maintaining proper water and electrolyte balance is essential for health.
The document analyzes the water quality of Mankato State University's tap water by measuring alkalinity, acidity, and hardness. Experiments found the water had high alkalinity (29.33 ppm of CaCO3), lower acidity (8 ppm of CaCO3), and was classified as hard (210 ppm of CaCO3). This indicates the water is well-buffered against acidification and has higher dissolved metal content. In conclusion, measuring these factors provides insight into the water's chemical properties and quality.
1) The document discusses Le Châtelier's principle and how chemical equilibriums respond to changes in concentration, temperature, volume or pressure by shifting to counteract the imposed change.
2) It then describes several experiments involving acid-base indicators, the solubility product constant (Ksp) for lead chloride, complex ion equilibriums involving cobalt chloride, and dissolving insoluble salts like zinc hydroxide through the addition of reagents.
3) The experiments are meant to demonstrate Le Châtelier's principle in chemical systems at equilibrium and how the addition of various reagents can shift the equilibrium by changing concentrations or forming new complexes.
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.
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.
Lab 4 alkalinity –acidity and determination of alkalinity in waterAnas Maghayreh
Environmental lab
Lab 4 alkalinity –acidity and determination of alkalinity in water
experiment at JORDAN UNIVERSITY OF SCIENCE AND TECHNOLOGY
by: ANAS MAGHAYREH
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.
1. The document contains a practice test with multiple choice questions about chemical kinetics and equilibrium.
2. Questions cover topics like reaction rates, rate laws, reaction orders, equilibrium constants, Le Chatelier's principle, and the Haber process.
3. There is also a bonus section with chemical nomenclature questions matching names to formulas.
This document provides information about solutions and colloids. It begins with an overview of solutions as homogeneous mixtures that exist as a single phase, while colloids are heterogeneous mixtures that exist in two or more phases. Subsequent sections discuss solubility and how intermolecular forces affect it, concentration terms including molarity, molality and mole fraction, and factors that influence solubility such as temperature and pressure. Examples are provided for calculating concentration in various units and converting between concentration terms. The document concludes with a discussion of using solutions in chemical reactions including titration and diluting solutions.
This document provides a review of key concepts from Chapter 16, including solubility, supersaturated solutions, colligative properties, factors that affect solubility, and calculations involving molarity, molality, mass percent, and volume percent in solution concentration problems. It contains multiple choice and open response questions about these topics.
This document contains 24 chemistry assignment questions about solutions. Some key topics covered include:
1. Determining which liquid has a higher vapor pressure at a given temperature based on their boiling points.
2. Examples of solid solute in a solid solvent and why oil and water do not mix.
3. When molality is preferred over molarity and examples of isotonic solutions.
4. Calculating Vant Hoff factor for a dilute K2SO4 solution and stating Henry's law.
5. Identifying type of deviation from ideal behavior when two liquids produce a warm solution upon mixing.
6. Defining osmotic pressure and explaining why 1 M KCl has a higher osmotic
1. Henry's law relates the pressure of a gas in a solution to its solubility. It has applications.
2. Glucose solution will freeze at a specific temperature, calculated using information provided.
3. Raoult's law describes how volatile liquid solutions deviate from ideal behavior. Positive and negative deviations are explained with examples.
This document provides definitions and examples of key concepts in general chemistry including:
1. Solvation refers to the attractive interaction between solvent molecules and a solute. Hydration describes the interaction when water is the solvent.
2. The overall enthalpy change of a solution can be either positive (endothermic) or negative (exothermic).
3. A saturated solution is one in equilibrium with undissolved solute where dissolution and crystallization occur at equal rates. Unsaturated and supersaturated solutions contain less or more solute respectively.
4. Colligative properties include vapor pressure depression, freezing point depression, boiling point elevation, and osmotic pressure.
PHYSICAL CHEMISTRY - Two Components Liquid Systemshahzadebaujiti
PHYSICAL CHEMISTRY - Two Components Liquid System
IMMISCIBLE LIQUIDS
Immiscible liquids are liquids which do not mix up to form homogeneous mixture.
When there are two immiscible liquids they form a so called immiscible pair.
Immiscible liquids form heterogeneous mixture.
Environmentatl chemistry water (questions and answers)Martin Brown
This document contains exam questions from 2009-2002 on the topics of water treatment, water quality testing, acid-base chemistry, and sewage treatment. It asks students to define concepts like conjugate acid-base pairs, calculate pH values, identify chemicals used in water treatment and their purposes, and describe the multi-stage processes involved in treating water and sewage.
The poem discusses pollution in American cities. It warns that visitors should not drink the water or breathe the air due to the high levels of pollution, which include smog, sewage, and industrial waste. The pollution has wiped out fish and bird populations. While people try to take precautions like using toothpaste, the pollution is still present in the city streets and waterways.
Colligative properties of dilute solutions Manik Imran Nur Manik
lowering of vapour pressure, elevation of boiling point, depression of freezing point and osmotic pressure including necessary thermodynamic derivations.
Distribution Law
What is Distribution law?
Immiscible liquids
Explanation
APPLICATION OF DISTRIBUTION LAW
Limitations of Distribution Law
Contrast and Comparison between separation through Separating funnel and Fractional Distillation
This document discusses various properties of mixtures, including solutions and colloids. It defines key terms like solvent, solute, and aqueous solutions. It describes factors that affect solubility such as temperature, nature of solute and solvent, and pressure. It also covers gas solubility based on Henry's Law. Finally, it discusses quantitative expressions of concentration including molarity and molality, as well as colligative properties of solutions like boiling point elevation.
1. The document discusses vapor pressure concepts including Raoult's law and ideal solutions. It provides questions related to how vapor pressure is affected by factors like temperature, moles of vapor/liquid, and addition of a non-volatile solute.
2. Key concepts covered include how vapor pressure of a solution is lower than the pure solvent due to the non-volatile solute occupying space in the liquid phase. An ideal solution follows Raoult's law where vapor pressure is directly proportional to mole fraction of solvent.
3. Questions assess understanding of these concepts through calculations and identifying properties of ideal/non-ideal solutions and relationships between liquid/vapor phase compositions according to vapor pressure diagrams.
This document provides information and examples on solutions and titrations in chemistry:
- It defines key terms like solute, solvent, concentration, molarity and explains how to calculate concentrations in g/dm3 and moldm-3.
- Examples are given for calculating the mass of a solute needed to make a solution of a given volume and molarity, and for calculating concentrations when solutions are diluted.
- A titration is described as a procedure using a burette to add one solution of known concentration to a flask of another until reaction is complete.
- Standard solutions that are suitable for titrations are outlined.
- Worked examples of titration calculations include determining
This document discusses electrolyte solutions, milliequivalents, millimoles, micromoles, and osmolarity as they relate to water and electrolyte balance in the body. It provides definitions and examples of calculating concentrations of electrolytes using various units. Electrolytes play an important role in acid-base balance, water volume control, and metabolism. Disturbances in electrolyte and fluid balance can be treated with oral and intravenous electrolyte preparations. Maintaining proper water and electrolyte balance is essential for health.
The document analyzes the water quality of Mankato State University's tap water by measuring alkalinity, acidity, and hardness. Experiments found the water had high alkalinity (29.33 ppm of CaCO3), lower acidity (8 ppm of CaCO3), and was classified as hard (210 ppm of CaCO3). This indicates the water is well-buffered against acidification and has higher dissolved metal content. In conclusion, measuring these factors provides insight into the water's chemical properties and quality.
1) The document discusses Le Châtelier's principle and how chemical equilibriums respond to changes in concentration, temperature, volume or pressure by shifting to counteract the imposed change.
2) It then describes several experiments involving acid-base indicators, the solubility product constant (Ksp) for lead chloride, complex ion equilibriums involving cobalt chloride, and dissolving insoluble salts like zinc hydroxide through the addition of reagents.
3) The experiments are meant to demonstrate Le Châtelier's principle in chemical systems at equilibrium and how the addition of various reagents can shift the equilibrium by changing concentrations or forming new complexes.
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.
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.
Lab 4 alkalinity –acidity and determination of alkalinity in waterAnas Maghayreh
Environmental lab
Lab 4 alkalinity –acidity and determination of alkalinity in water
experiment at JORDAN UNIVERSITY OF SCIENCE AND TECHNOLOGY
by: ANAS MAGHAYREH
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.
1. The document contains a practice test with multiple choice questions about chemical kinetics and equilibrium.
2. Questions cover topics like reaction rates, rate laws, reaction orders, equilibrium constants, Le Chatelier's principle, and the Haber process.
3. There is also a bonus section with chemical nomenclature questions matching names to formulas.
This document provides information about solutions and colloids. It begins with an overview of solutions as homogeneous mixtures that exist as a single phase, while colloids are heterogeneous mixtures that exist in two or more phases. Subsequent sections discuss solubility and how intermolecular forces affect it, concentration terms including molarity, molality and mole fraction, and factors that influence solubility such as temperature and pressure. Examples are provided for calculating concentration in various units and converting between concentration terms. The document concludes with a discussion of using solutions in chemical reactions including titration and diluting solutions.
This document provides a review of key concepts from Chapter 16, including solubility, supersaturated solutions, colligative properties, factors that affect solubility, and calculations involving molarity, molality, mass percent, and volume percent in solution concentration problems. It contains multiple choice and open response questions about these topics.
This document contains 24 chemistry assignment questions about solutions. Some key topics covered include:
1. Determining which liquid has a higher vapor pressure at a given temperature based on their boiling points.
2. Examples of solid solute in a solid solvent and why oil and water do not mix.
3. When molality is preferred over molarity and examples of isotonic solutions.
4. Calculating Vant Hoff factor for a dilute K2SO4 solution and stating Henry's law.
5. Identifying type of deviation from ideal behavior when two liquids produce a warm solution upon mixing.
6. Defining osmotic pressure and explaining why 1 M KCl has a higher osmotic
1. Henry's law relates the pressure of a gas in a solution to its solubility. It has applications.
2. Glucose solution will freeze at a specific temperature, calculated using information provided.
3. Raoult's law describes how volatile liquid solutions deviate from ideal behavior. Positive and negative deviations are explained with examples.
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 document provides information about a General Chemistry 2 summer course including the instructor's contact information, teaching assistants, textbook, course schedule, exam details, and chapter outlines. Specifically, it outlines Chapter 11 which discusses the structure of water, intermolecular forces, physical properties of water and liquids, phase diagrams, solutions, and colligative properties.
This document provides instructions and questions for a chemistry revision exam on solutions and electrochemistry for class 12. It includes 30 multiple choice and written response questions across a range of topics. Questions will be worth between 1 to 5 marks each and test concepts such as electrolyte conductivity, standard reduction potentials, molality, deviations from Raoult's law, Kohlrausch's law, electrolysis products, intermolecular forces, Henry's law, cell potentials, freezing point depression, osmotic pressure, and conductivity-concentration relationships for strong and weak electrolytes. Calculations involving moles, mass, equilibrium constants, and dissociation constants are also assessed.
New chm-151-unit-13-power-points-su13s-140227172226-phpapp02Cleophas Rwemera
This document provides an overview of solutions and colloids. It begins by defining solutions and colloids, noting that solutions are homogeneous mixtures that exist in a single phase, while colloids are heterogeneous mixtures that exist in two or more phases. The document then discusses concentration terms such as molarity, molality, and mole fraction. It provides examples of calculating concentrations using these different terms. Finally, the document covers additional topics related to solutions, including factors that affect solubility, dilutions, and interconverting between concentration terms.
This document contains 20 multiple choice questions about colligative properties and solutions. It provides data about the freezing point depression and boiling point elevation of solutions prepared using various solutes like ammonia, sodium carbonate, and an unknown compound dissolved in water or cyclohexane. The questions test understanding of concepts like percent composition, mole fraction, molality, molarity, and van't Hoff factor.
This document describes a procedure for determining water hardness through titration with EDTA. Water hardness is defined as the calcium and magnesium ion content and is reported in parts per million (ppm) of calcium carbonate. The titration uses EDTA to chelate calcium and magnesium ions until the indicator Eriochrome Black T changes color, signaling the endpoint. Standard solutions of calcium carbonate and EDTA are prepared and used to determine the concentration of EDTA and calculate water hardness based on the volume of EDTA needed to reach the endpoint in a sample.
- The original solution contained 30 g of a non-volatile solute dissolved in 90 g of water and had a vapor pressure of 2.8 kPa at 298 K.
- Then, 18 g of additional water was added to the solution.
- The new vapor pressure of the solution after adding water was measured to be 2.9 kPa at 298 K.
- The question asks to calculate the molar mass of the non-volatile solute based on this information.
This document discusses colligative properties, which are physical properties of solutions that depend on the concentration of solute particles rather than the identity of the solute. It defines key colligative properties like boiling point elevation, freezing point depression, and osmotic pressure. The document also explains how these properties obey mathematical relationships like Raoult's law. Several examples are provided to demonstrate how to use these relationships and colligative property equations to calculate values like vapor pressure, boiling point, freezing point, osmotic pressure, and molar mass of a solute.
The document is a past paper for the AIEEE chemistry exam from 2007 containing 40 multiple choice questions related to chemistry concepts and calculations. The questions cover topics like thermodynamics, electrochemistry, acid-base chemistry, organic chemistry reactions, and properties of elements.
The document is a past paper for the AIEEE chemistry exam from 2007 containing 40 multiple choice questions related to chemistry concepts and calculations. The questions cover topics like thermodynamics, electrochemistry, acid-base chemistry, organic chemistry reactions, and properties of elements.
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12 chemistry impq_ch02_solutions_01
1. 18 XII – Chemistry
AK
Unit - 2
SOLUTIONS
VSA QUESTIONS (1 - MARK QUESTIONS)
1. Give an example of ‘liquid in solid’ type solution.
2. Which type of solid solution will result by mixing two solid components with
large difference in the sizes of their molecules?
3. What is meant by semimolar and decimolar solutions?
M M
,
2 10
Ans.:
4. What will be the mole fraction of water in C2H5OH solution containing
equal number of moles of water and C2H5OH? [Ans. : 0.5]
5. Which of the following is a dimensionless quantity : molarity, molality or
mole fraction? [Ans. : mole fraction]
6. 10 g glucose is dissolved in 400 g. of solution. Calculate percentage
concentration of the solution. [Ans. : 2.5% w/w]
7. Gases tend to be less soluble in liquids as the temperature is raised.
Why?
8. State the conditions which must be satisfied if an ideal solution is to be
formed.
9. A mixture of chlorobenzene and bromobenzene forms nearly ideal solution
but a mixture of chloroform and acetone does not. Why?
10. How is the concentration of a solute present in trace amount in a solution
expressed?
*12. N2 and O2 gases have KH values 76.48 kbar and 34.86 kbar respectively
at 293 K temperature. Which one of these will have more solubility in
water?
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2. 19 XII – Chemistry
AK
*13. Under what condition molality and molarity of a solution are identical.
Explain with suitable reason.
*14. Addition of HgI2 to KI (aq.) shows decrease in vapour pressure. Why?
15. What will happen to the boiling point of the solution formed on mixing two
miscible liquids showing negative deviation from Raoult’s law?
16. Liquid ‘Y’ has higher vapour pressure than liquid ‘X’, which of them will
have higher boiling point?
17. When 50 mL of ethanol and 50 mL of water are mixed, predict whether the
volume of the solution is equal to, greater than or less than 100 mL.
Justify.
18. Which type of deviation is shown by the solution formed by mixing
cyclohexane and ethanol?
19. A and B liquids on mixing produce a warm solution. Which type of deviation
from Raoult’s law is there?
20. Define cryoscopic constant (molal freezing point depression constant.)
21. Mention the unit of ebulioscopic constant (molal boiling point elevation
constant.)
22. If kf for water is 1.86 K kg mol–1, what is the freezing point of 0.1 molal
solution of a substance which undergoes no dissociation or association of
solute?
[Hint : Tf = iKf . m]
24. What is reverse osmosis? Give one large scale use of it.
*25. What is the maximum value of van’t Hoff factor (i) for Na2SO4 . 10H2O?
[Ans. : i = 3]
26. What is the value of van’t Hoff factor (i) if solute molecules undergo
dimerisation. [Ans. : i = 0.5]
27. Under what condition is van’t Hoff factor less than one?
[Ans. : Association]
*28. The Phase Diagram for pure solvent and the solution containing nonvolatile
solute are recorded below. The quantity indicated by ‘X’ in the figure is
known as : [Ans. : Tb]
3. 20 XII – Chemistry
AK
*29. AgNO3 on reaction with NaCl in aqueous solution gives white precipitate.
If the two solutions are separated by a semi-permeable membrane, will
there be appearance of a white ppt. in the side ‘X’ due to osmosis?
[Ans. : No ppt, because only solvent particles moves through SPM]
SA (I) - TYPE QUESTIONS (2 - MARK QUESTIONS)
1. Explain the following :
(a) Solubility of a solid in a liquid involves dynamic equilibrium.
(b) Ionic compounds are soluble in water but are insoluble in nonpolar
solvents.
2. Give two examples each of a solution :
(a) showing positive deviation from Raoult’s Law.
(b) showing negative deviation from Raoult’s Law.
3. Draw vapour pressure vs composition (in terms of mole fraction) diagram
for an ideal solution.
4. Define azeotropes with one example of each type.
5. Draw the total vapour pressure vs. mol fraction diagram for a binary
solution exhibiting non-ideal behaviour with negative deviation.
6. The vapour pressure curve for three solutions having the same non-
volatile solute in the same solvent are shown. The curves are parallel to
each other and do not intersect. What is the correct order of the
concentrations of the solutions. [Hint. : A < B < C]
4. 21 XII – Chemistry
AK
7. Show that the relative lowering of vapour pressure of a solvent is a colligative
property.
8. Benzene and toluene form a nearly ideal solution. At a certain temperature,
calculate the vapour pressure of solution containing equal moles of the
two substances.
[Given : P°Benzene = 150 mm of Hg, P°Toluene = 55 mm of Hg]
9. What is meant by abnormal molecular mass? Illustrate it with suitable
examples.
*10. When 1 mole of NaCl is added to 1 litre water, the boiling point increases?
When 1 mole of CH3OH is added to 1 litre water, the boiling point
decreases? Suggest reasons.
11. Can we separate water completely from HNO3 solution by vapourisation?
Justify your answer.
*12. 1 gram each of two solutes ‘A’ and ‘B’ (molar mass of A > molar mass of
B) are dissolved separately in 100 g each of the same solvent. Which
solute will show greater elevation in boiling point and Why?
Solution
2 - MARK QUESTIONS
13. Examine the following illustrations and answer the following questions
1 bar
5. 22 XII – Chemistry
AK
(a) Identify the liquid A and liquid B (pure water or sugar solution)
(b) Name the phenomenon involved in this experiment so that the level
of liquid in this the funnel has risen after some time.
14. How relative lowering in vapour pressure is related with depression in
freezing point and elevation in boiling point?
SA (II) TYPE QUESTIONS (3 - MARK QUESTIONS)
1. (a) State Henry’s Law.
(b) If O2 is bubbled through water at 393 K, how many millimoles of O2
gas would be dissolved in 1L of water? Assume that O2 exerts a
pressure of 0.95 bar.
(Given KH for O2 = 46.82 bar at 393K).
2. Given reason for the following :–
(a) Aquatic species are more comfortable in cold waters than in warm
waters.
(b) To avoid bends scuba divers use air diluted with helium.
(c) Cold drinks bottles are sealed under high pressure of CO2.
3. Why should a solution of a non-volatile and non-eletrolyte solute boil at
a higher temperature? Explain with the help of a diagram. Derive the
relationship between molar mass and elevation in boiling point.
4. Account for the following :–
(a) CaCl2 is used to clear snow from roads in hill stations.
(b) Ethylene glycol is used as antifreeze solution in radiators of vehicles
in cold countries.
(c) The freezing point depression of 0.01 m NaCl is nearly twice that of
0.01 m glucose solution.
5. Why do colligative properties of solution of a given concentration are
found to give abnormal molecular weight of solute. Explain with the help
of suitable examples.
6. Give reasons for the following :–
(a) RBC swell up and finally burst when placed in 0.1% NaCl solution.
(b) When fruits and vegetables that have been dried are placed in
water, they slowly swell and return to original form.
6. 23 XII – Chemistry
AK
(c) A person suffering from high blood pressure is advised to take less
amount of table salt.
*7. Glycerine, ethylene glycol and methanol are sold at the same price per
kg. Which would be cheaper for preparing an antifreeze solution for the
radiator of an automobile? [Ans. : Methanol]
*8. Determine the correct order of the property mentioned against them :
(a) 10% glucose (p1), 10% urea (p2), 10% sucrose (p3) [Osmotic
pressure]
(b) 0.1 m NaCl, 0.1 m urea, 0.1 m MgCl2 [Elevation in b.pt.]
(c) 0.1 m CaCl2, 0.1 m sucrose, 0.1 m NaCl [Depression in f.pt.]
9. For a dilute solution containing 2.5 g of a non-volatile non-electrolyte
solute in 100 g of water, the elevation in boiling point at 1 atm pressure
is 2°C. Assuming concentration of solute is much lower than the
concentration of solvent, determine the vapour pressure (mm of Hg) of the
solution.
[Given : Kb for water = 0.76 kg mol–1] [Ans.: 724 mm of Hg]
[Hind : Tb = Kb.
B
2.5 1000
m 0.76 = 2k
M 100
⇒ × ×
Mb = 9.5 g mol–1
A A
A
p – p 25 18
p 95 100
°
= ×
°
A
A
760 – p 25 18
p = 724 mm of Hg]
760 95 100
= × ⇒
10. 15.0 g of an unknown molecular substance was dissolved in 450 g of
water. The resulting solution was fund to freeze at –0.34°C. What is the
molar mass of this substance. (Kf for water = 1.86 K kg mol–1).
LONG ANSWER TYPE QUESTIONS (5 MARKS)
1. (a) What are ideal solutions? Write two examples.
(b) Calculate the osmoic pressure in pascals exerted by a solution
prepared by dissolving 1.0g of polymer of molar mass 185000 in
450 mL of water at 37°C.
7. 24 XII – Chemistry
AK
2. (a) Describe a method of determining molar mass of a non-volatile solute
from vapour pressure lowering.
(b) How much urea (mol. mass 60 g mol–1) must be dissolved in 50g of
water so that the vapour pressure at the room temperature is reduced
by 25%? Also calculate the molality of the solution obtained.
[Ans. : 55.55 g and 18.5 m]
3. (a) Why is the freezing point depression considered as a colligative
property?
(b) The cryoscopic constant of water is 1.86 km–1. Comment on this
statement.
(c) Calculate the amount of ice that will separate out on cooling solution
containing 50 g of ethylene glycol in 200 g H2O to –9.3°C. (Kf for
water = 1.86 K kg mol–1) [Ans. : 38.71g]
4. (a) Define osmotic pressure.
(b) Why osmotic pressure is preferred over other colligative properties
for the determination of molecular masses of macromolecules?
(c) What is the molar concentration of particles in human blood if the
osmotic pressure is 7.2 atm at normal body temperature of 37°C?
[Ans. : 0.283 M]
NUMERICAL PROBLEMS
1. Calculate the mass percentage of benzene (C6H6) and carbon tetrachloride
(CCl4), If 22g of benzene is dissolved in 122g of carbon tetrachloride.
[Ans. : C6H6 = 15.3%, CCl4 = 84.7%]
2. Calculate the molarity of a solution prepared by mixing 500 mL of 2.5 M
urea solution and 500 mL of 2M urea solution. [Ans. : 2.25 m]
[Hint : 1 1 2 2
1 2
M V + M V
M =
V + V
3. The mole fraction of CH3OH in an aqueous solution is 0.02 and density
of solution 0.994 g cm–3. Determine the molality and molarity.
[Ans. : 1.13m, 1.08m]
4. 200 mL of calcium chloride solution contains 3.011 × 1022 Cl– ions. Calculate
the molarity of the solution. Assume that calcium chloride is completely
ionized. [Ans. : 0.125 M]
8. 25 XII – Chemistry
AK
5. 6 × 10–3 g oxygen is dissolved per kg of sea water. Calculate the ppm of
oxygen in sea water. [Ans. : 6 ppm]
6. The solubility of oxygen in water is 1.35 × 10–3 mol L–1 at 20°C and 1 atm
pressure. Calculate the concentration of oxygen at 20°C and 0.2 atm
pressure. [Ans. : 2.7 × 10–4 mol L–1]
7. Two liquids X and Y on mixing form an ideal solution. The vapour pressure
of the solution containing 2 mol of X and 1 mol of Y is 550 mm Hg. But
when 4 mol of X and 1 mole of Y are mixed, the vapour pressure of
solution thus formed is 560 mm Hg. What will be the vapour pressure of
pure X and pure Y at this temperature?
[Ans. : X = 600 mm Hg; Y = 400 mm Hg]
8. An aqueous solution containing 3.12 g of barium chloride in 250 g of
water is found to be boil at 100.0832°C. Calculate the degree of dissociation
of barium chloride.
[Given molar mass BaCl2 = 208 g mol–1, Kb for water = 0.52 K/m]
[Ans. : 83.3%]
9. The degree of dissociation of Ca(NO3)2 in a dilute aqueous solution,
containing 7.0 g of salt per 100 g of water at 100°C is 70%. If the vapour
pressure of water at 100°C is 760 mm of Hg, calculate the vapour pressure
of the solution. [Ans. : 745.3 mm of Hg]
10. 2g of C6H5COOH dissolved in 25g of benzene shows depression in freezing
point equal to 1.62K. Molar freezing point depression constant for benzene
is 4.9 K kg mol–1. What is the percentage association of acid if it forms
a dimer in solution? [Ans. : 99.2%]
11. Calculate the amount of NaCl which must added to one kg of water so that
the freezing point is depressed by 3K. Given Kf = 1.86 K kg mol–1, Atomic
mass : Na = 23, Cl = 35.5). [Ans. : 0.81 mol NaCl]
12. Three molecules of a solute (A) associate in benzene to form species A3.
Calculate the freezing point of 0.25 molal solution. The degree of association
of solute A is found to be 0.8. The freezing point of benzene is 5.5°C and
its Kf value is 5.13 K/m. [Ans. : 4.9°C]
13. A 5% solution of sucrose (C12H22O11) is isotonic with 0.877% solution of
urea. NH2CONH2) Calculate the molecular mass of urea.[Ans. : 59.99 g
mol–1]
14. Osmotic pressure of a 0.0103 molar solution of an electrolyte was found
to be 0.75 atm at 27°C. Calculate Van’t Hoff factor. [Ans. : i = 3]
9. 26 XII – Chemistry
AK
*15. The maximum allowable level of nitrates in drinking water is 45 mg nitrate
ions/dm3. Express this level in ppm? [Ans. : 45 ppm]
16. 75.2 g of Phenol (C6H5OH) is dissolved in 1 kg solvent of Kf = 14 Km–1,
if the depression in freezing point is 7K, then find the % of phenol that
dimerises. [Ans. : 75%]
*17. An aqueous solution of glucose boils at 100.01°C. The molal boiling point
elevation constant for water is 0.5 K kg mol–1. What is the number of
glucose molecule in the solution containing 100 g of water.
[Ans. : 1.2 × 1021 molecules]
18. A bottle of commercial H2SO4 [density = 1.787 g/mL] is labelled as 86%
by mass.
(a) What is the molarity of the acid?
(b) What volume of the acid has to be used to make 1 litre 0.2 M
H2SO4?
(c) What is the molality of the acid?
[Ans. : 15.7 M, 12.74 mL, 62.86 m]
19. A solution containing 30g of non-volatile solute exactly in 90g of water has
a vapour pressure of 2.8 kPa at 298 K. Furhter, 18 g of water is then
added to the solution and the new vapour pressure becomes 2.9 kPa at
298 K. Calculate :
(i) molar mass of the solute
(ii) Vapour pressure of water at 298 K. [Ans. : 34 g mol–1, 3.4 kPa]
20. The vapour pressure of pure liquids A and B are 450 and 750 mm Hg
respectively, at 350K. Find out the composition of the liquid mixture if total
vapour pressure is 600 mm Hg. Also find the composition of the vapour
phase. [Ans. : XA = 0.4, XB = 0.6, YA = 0.3, YB = 0.7]
21. An aqueous solution of 2% non-volatile solute exerts a pressure of 1.004
bar at the normal boiling point of the solvent. What is the molar mass of
the solute? [Ans. : 41.35 g mol–1]
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